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1Etymology

2Modern principles

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2.1Matter

2.1.1Atom

2.1.2Element

2.1.3Compound

2.1.4Molecule

2.1.5Substance and mixture

2.1.6Mole and amount of substance

2.2Phase

2.3Bonding

2.4Energy

2.5Reaction

2.6Ions and salts

2.7Acidity and basicity

2.8Redox

2.9Equilibrium

2.10Chemical laws

3History

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3.1Definition

3.2Background

4Practice

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4.1Subdisciplines

4.2Interdisciplinary

4.3Industry

4.4Professional societies

5See also

6References

7Bibliography

8Further reading

9External links

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Chemistry

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From Wikipedia, the free encyclopedia

Scientific field of study

For other uses, see Chemistry (disambiguation). "Chemical science" redirects here. For the journal, see Chemical Science (journal). Not to be confused with Kemistry.

Part of a series onChemistryScience of matter

Index

Outline

Glossary

History (timeline)

Key components

Matter

Phase

Bond

Chemical reaction

Ion

Acid–base reaction

Redox

Chemical equilibrium

Chemical law

Branches

Analytical chemistry

Biochemistry

Organic chemistry

Inorganic chemistry

Physical chemistry

Research

Chemist (list)

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Chemistry is the scientific study of the properties and behavior of matter.[1] It is a physical science within the natural sciences that studies the chemical elements that make up matter and compounds made of atoms, molecules and ions: their composition, structure, properties, behavior and the changes they undergo during reactions with other substances.[2][3][4][5] Chemistry also addresses the nature of chemical bonds in chemical compounds.

In the scope of its subject, chemistry occupies an intermediate position between physics and biology.[6] It is sometimes called the central science because it provides a foundation for understanding both basic and applied scientific disciplines at a fundamental level.[7] For example, chemistry explains aspects of plant growth (botany), the formation of igneous rocks (geology), how atmospheric ozone is formed and how environmental pollutants are degraded (ecology), the properties of the soil on the Moon (cosmochemistry), how medications work (pharmacology), and how to collect DNA evidence at a crime scene (forensics).

Chemistry has existed under various names since ancient times.[8] It has evolved, and now chemistry encompasses various areas of specialisation, or subdisciplines, that continue to increase in number and interrelate to create further interdisciplinary fields of study. The applications of various fields of chemistry are used frequently for economic purposes in the chemical industry.

Etymology

Main article: Etymology of chemistry

The word chemistry comes from a modification during the Renaissance of the word alchemy, which referred to an earlier set of practices that encompassed elements of chemistry, metallurgy, philosophy, astrology, astronomy, mysticism, and medicine. Alchemy is often associated with the quest to turn lead or other base metals into gold, though alchemists were also interested in many of the questions of modern chemistry.[9]

The modern word alchemy in turn is derived from the Arabic word al-kīmīā (الكیمیاء). This may have Egyptian origins since al-kīmīā is derived from the Ancient Greek χημία, which is in turn derived from the word Kemet, which is the ancient name of Egypt in the Egyptian language.[10] Alternately, al-kīmīā may derive from χημεία 'cast together'.[11]

Modern principles

Laboratory, Institute of Biochemistry, University of Cologne in Germany

The current model of atomic structure is the quantum mechanical model.[12] Traditional chemistry starts with the study of elementary particles, atoms, molecules,[13] substances, metals, crystals and other aggregates of matter. Matter can be studied in solid, liquid, gas and plasma states, in isolation or in combination. The interactions, reactions and transformations that are studied in chemistry are usually the result of interactions between atoms, leading to rearrangements of the chemical bonds which hold atoms together. Such behaviors are studied in a chemistry laboratory.

The chemistry laboratory stereotypically uses various forms of laboratory glassware. However glassware is not central to chemistry, and a great deal of experimental (as well as applied/industrial) chemistry is done without it.

Solutions of substances in reagent bottles, including ammonium hydroxide and nitric acid, illuminated in different colors

A chemical reaction is a transformation of some substances into one or more different substances.[14] The basis of such a chemical transformation is the rearrangement of electrons in the chemical bonds between atoms. It can be symbolically depicted through a chemical equation, which usually involves atoms as subjects. The number of atoms on the left and the right in the equation for a chemical transformation is equal. (When the number of atoms on either side is unequal, the transformation is referred to as a nuclear reaction or radioactive decay.) The type of chemical reactions a substance may undergo and the energy changes that may accompany it are constrained by certain basic rules, known as chemical laws.

Energy and entropy considerations are invariably important in almost all chemical studies. Chemical substances are classified in terms of their structure, phase, as well as their chemical compositions. They can be analyzed using the tools of chemical analysis, e.g. spectroscopy and chromatography. Scientists engaged in chemical research are known as chemists.[15] Most chemists specialize in one or more sub-disciplines. Several concepts are essential for the study of chemistry; some of them are:[16]

Matter

Main article: Matter

In chemistry, matter is defined as anything that has rest mass and volume (it takes up space) and is made up of particles. The particles that make up matter have rest mass as well – not all particles have rest mass, such as the photon. Matter can be a pure chemical substance or a mixture of substances.[17]

Atom

Main article: Atom

A diagram of an atom based on the Rutherford model

The atom is the basic unit of chemistry. It consists of a dense core called the atomic nucleus surrounded by a space occupied by an electron cloud. The nucleus is made up of positively charged protons and uncharged neutrons (together called nucleons), while the electron cloud consists of negatively charged electrons which orbit the nucleus. In a neutral atom, the negatively charged electrons balance out the positive charge of the protons. The nucleus is dense; the mass of a nucleon is approximately 1,836 times that of an electron, yet the radius of an atom is about 10,000 times that of its nucleus.[18][19]

The atom is also the smallest entity that can be envisaged to retain the chemical properties of the element, such as electronegativity, ionization potential, preferred oxidation state(s), coordination number, and preferred types of bonds to form (e.g., metallic, ionic, covalent).

Element

Standard form of the periodic table of chemical elements. The colors represent different blocks of elements.

Main article: Chemical element

A chemical element is a pure substance which is composed of a single type of atom, characterized by its particular number of protons in the nuclei of its atoms, known as the atomic number and represented by the symbol Z. The mass number is the sum of the number of protons and neutrons in a nucleus. Although all the nuclei of all atoms belonging to one element will have the same atomic number, they may not necessarily have the same mass number; atoms of an element which have different mass numbers are known as isotopes. For example, all atoms with 6 protons in their nuclei are atoms of the chemical element carbon, but atoms of carbon may have mass numbers of 12 or 13.[19]

The standard presentation of the chemical elements is in the periodic table, which orders elements by atomic number. The periodic table is arranged in groups, or columns, and periods, or rows. The periodic table is useful in identifying periodic trends.[20]

Compound

Carbon dioxide (CO2), an example of a chemical compound

Main article: Chemical compound

A compound is a pure chemical substance composed of more than one element. The properties of a compound bear little similarity to those of its elements.[21] The standard nomenclature of compounds is set by the International Union of Pure and Applied Chemistry (IUPAC). Organic compounds are named according to the organic nomenclature system.[22] The names for inorganic compounds are created according to the inorganic nomenclature system. When a compound has more than one component, then they are divided into two classes, the electropositive and the electronegative components.[23] In addition the Chemical Abstracts Service has devised a method to index chemical substances. In this scheme each chemical substance is identifiable by a number known as its CAS registry number.

Molecule

Main article: Molecule

A ball-and-stick representation of the caffeine molecule (C8H10N4O2)

A molecule is the smallest indivisible portion of a pure chemical substance that has its unique set of chemical properties, that is, its potential to undergo a certain set of chemical reactions with other substances. However, this definition only works well for substances that are composed of molecules, which is not true of many substances (see below). Molecules are typically a set of atoms bound together by covalent bonds, such that the structure is electrically neutral and all valence electrons are paired with other electrons either in bonds or in lone pairs.

Thus, molecules exist as electrically neutral units, unlike ions. When this rule is broken, giving the "molecule" a charge, the result is sometimes named a molecular ion or a polyatomic ion. However, the discrete and separate nature of the molecular concept usually requires that molecular ions be present only in well-separated form, such as a directed beam in a vacuum in a mass spectrometer. Charged polyatomic collections residing in solids (for example, common sulfate or nitrate ions) are generally not considered "molecules" in chemistry. Some molecules contain one or more unpaired electrons, creating radicals. Most radicals are comparatively reactive, but some, such as nitric oxide (NO) can be stable.

A 2-D structural formula of a benzene molecule (C6H6)

The "inert" or noble gas elements (helium, neon, argon, krypton, xenon and radon) are composed of lone atoms as their smallest discrete unit, but the other isolated chemical elements consist of either molecules or networks of atoms bonded to each other in some way. Identifiable molecules compose familiar substances such as water, air, and many organic compounds like alcohol, sugar, gasoline, and the various pharmaceuticals.

However, not all substances or chemical compounds consist of discrete molecules, and indeed most of the solid substances that make up the solid crust, mantle, and core of the Earth are chemical compounds without molecules. These other types of substances, such as ionic compounds and network solids, are organized in such a way as to lack the existence of identifiable molecules per se. Instead, these substances are discussed in terms of formula units or unit cells as the smallest repeating structure within the substance. Examples of such substances are mineral salts (such as table salt), solids like carbon and diamond, metals, and familiar silica and silicate minerals such as quartz and granite.

One of the main characteristics of a molecule is its geometry often called its structure. While the structure of diatomic, triatomic or tetra-atomic molecules may be trivial, (linear, angular pyramidal etc.) the structure of polyatomic molecules, that are constituted of more than six atoms (of several elements) can be crucial for its chemical nature.

Substance and mixture

Examples of pure chemical substances. From left to right: the elements tin (Sn) and sulfur (S), diamond (an allotrope of carbon), sucrose (pure sugar), and sodium chloride (salt) and sodium bicarbonate (baking soda), which are both ionic compounds.

A chemical substance is a kind of matter with a definite composition and set of properties.[24] A collection of substances is called a mixture. Examples of mixtures are air and alloys.[25]

Mole and amount of substance

Main article: Mole

The mole is a unit of measurement that denotes an amount of substance (also called chemical amount). One mole is defined to contain exactly 6.02214076×1023 particles (atoms, molecules, ions, or electrons), where the number of particles per mole is known as the Avogadro constant.[26] Molar concentration is the amount of a particular substance per volume of solution, and is commonly reported in mol/dm3.[27]

Phase

Diagram showing relationships among the phases and the terms used to describe phase changes

Main article: Phase

In addition to the specific chemical properties that distinguish different chemical classifications, chemicals can exist in several phases. For the most part, the chemical classifications are independent of these bulk phase classifications; however, some more exotic phases are incompatible with certain chemical properties. A phase is a set of states of a chemical system that have similar bulk structural properties, over a range of conditions, such as pressure or temperature.

Physical properties, such as density and refractive index tend to fall within values characteristic of the phase. The phase of matter is defined by the phase transition, which is when energy put into or taken out of the system goes into rearranging the structure of the system, instead of changing the bulk conditions.

Sometimes the distinction between phases can be continuous instead of having a discrete boundary' in this case the matter is considered to be in a supercritical state. When three states meet based on the conditions, it is known as a triple point and since this is invariant, it is a convenient way to define a set of conditions.

The most familiar examples of phases are solids, liquids, and gases. Many substances exhibit multiple solid phases. For example, there are three phases of solid iron (alpha, gamma, and delta) that vary based on temperature and pressure. A principal difference between solid phases is the crystal structure, or arrangement, of the atoms. Another phase commonly encountered in the study of chemistry is the aqueous phase, which is the state of substances dissolved in aqueous solution (that is, in water).

Less familiar phases include plasmas, Bose–Einstein condensates and fermionic condensates and the paramagnetic and ferromagnetic phases of magnetic materials. While most familiar phases deal with three-dimensional systems, it is also possible to define analogs in two-dimensional systems, which has received attention for its relevance to systems in biology.

Bonding

Main article: Chemical bond

An animation of the process of ionic bonding between sodium (Na) and chlorine (Cl) to form sodium chloride, or common table salt. Ionic bonding involves one atom taking valence electrons from another (as opposed to sharing, which occurs in covalent bonding).

Atoms sticking together in molecules or crystals are said to be bonded with one another. A chemical bond may be visualized as the multipole balance between the positive charges in the nuclei and the negative charges oscillating about them.[28] More than simple attraction and repulsion, the energies and distributions characterize the availability of an electron to bond to another atom.

The chemical bond can be a covalent bond, an ionic bond, a hydrogen bond or just because of Van der Waals force. Each of these kinds of bonds is ascribed to some potential. These potentials create the interactions which hold atoms together in molecules or crystals. In many simple compounds, valence bond theory, the Valence Shell Electron Pair Repulsion model (VSEPR), and the concept of oxidation number can be used to explain molecular structure and composition.

An ionic bond is formed when a metal loses one or more of its electrons, becoming a positively charged cation, and the electrons are then gained by the non-metal atom, becoming a negatively charged anion. The two oppositely charged ions attract one another, and the ionic bond is the electrostatic force of attraction between them. For example, sodium (Na), a metal, loses one electron to become an Na+ cation while chlorine (Cl), a non-metal, gains this electron to become Cl−. The ions are held together due to electrostatic attraction, and that compound sodium chloride (NaCl), or common table salt, is formed.

In the methane molecule (CH4), the carbon atom shares a pair of valence electrons with each of the four hydrogen atoms. Thus, the octet rule is satisfied for C-atom (it has eight electrons in its valence shell) and the duet rule is satisfied for the H-atoms (they have two electrons in their valence shells).

In a covalent bond, one or more pairs of valence electrons are shared by two atoms: the resulting electrically neutral group of bonded atoms is termed a molecule. Atoms will share valence electrons in such a way as to create a noble gas electron configuration (eight electrons in their outermost shell) for each atom. Atoms that tend to combine in such a way that they each have eight electrons in their valence shell are said to follow the octet rule. However, some elements like hydrogen and lithium need only two electrons in their outermost shell to attain this stable configuration; these atoms are said to follow the duet rule, and in this way they are reaching the electron configuration of the noble gas helium, which has two electrons in its outer shell.

Similarly, theories from classical physics can be used to predict many ionic structures. With more complicated compounds, such as metal complexes, valence bond theory is less applicable and alternative approaches, such as the molecular orbital theory, are generally used. See diagram on electronic orbitals.

Energy

Main article: Energy

In the context of chemistry, energy is an attribute of a substance as a consequence of its atomic, molecular or aggregate structure. Since a chemical transformation is accompanied by a change in one or more of these kinds of structures, it is invariably accompanied by an increase or decrease of energy of the substances involved. Some energy is transferred between the surroundings and the reactants of the reaction in the form of heat or light; thus the products of a reaction may have more or less energy than the reactants.

A reaction is said to be exergonic if the final state is lower on the energy scale than the initial state; in the case of endergonic reactions the situation is the reverse. A reaction is said to be exothermic if the reaction releases heat to the surroundings; in the case of endothermic reactions, the reaction absorbs heat from the surroundings.

Chemical reactions are invariably not possible unless the reactants surmount an energy barrier known as the activation energy. The speed of a chemical reaction (at given temperature T) is related to the activation energy E, by the Boltzmann's population factor

−

{\displaystyle e^{-E/kT}}

– that is the probability of a molecule to have energy greater than or equal to E at the given temperature T. This exponential dependence of a reaction rate on temperature is known as the Arrhenius equation.

The activation energy necessary for a chemical reaction to occur can be in the form of heat, light, electricity or mechanical force in the form of ultrasound.[29]

A related concept free energy, which also incorporates entropy considerations, is a very useful means for predicting the feasibility of a reaction and determining the state of equilibrium of a chemical reaction, in chemical thermodynamics. A reaction is feasible only if the total change in the Gibbs free energy is negative,

≤

{\displaystyle \Delta G\leq 0\,}

; if it is equal to zero the chemical reaction is said to be at equilibrium.

There exist only limited possible states of energy for electrons, atoms and molecules. These are determined by the rules of quantum mechanics, which require quantization of energy of a bound system. The atoms/molecules in a higher energy state are said to be excited. The molecules/atoms of substance in an excited energy state are often much more reactive; that is, more amenable to chemical reactions.

The phase of a substance is invariably determined by its energy and the energy of its surroundings. When the intermolecular forces of a substance are such that the energy of the surroundings is not sufficient to overcome them, it occurs in a more ordered phase like liquid or solid as is the case with water (H2O); a liquid at room temperature because its molecules are bound by hydrogen bonds.[30] Whereas hydrogen sulfide (H2S) is a gas at room temperature and standard pressure, as its molecules are bound by weaker dipole-dipole interactions.

The transfer of energy from one chemical substance to another depends on the size of energy quanta emitted from one substance. However, heat energy is often transferred more easily from almost any substance to another because the phonons responsible for vibrational and rotational energy levels in a substance have much less energy than photons invoked for the electronic energy transfer. Thus, because vibrational and rotational energy levels are more closely spaced than electronic energy levels, heat is more easily transferred between substances relative to light or other forms of electronic energy. For example, ultraviolet electromagnetic radiation is not transferred with as much efficacy from one substance to another as thermal or electrical energy.

The existence of characteristic energy levels for different chemical substances is useful for their identification by the analysis of spectral lines. Different kinds of spectra are often used in chemical spectroscopy, e.g. IR, microwave, NMR, ESR, etc. Spectroscopy is also used to identify the composition of remote objects – like stars and distant galaxies – by analyzing their radiation spectra.

Emission spectrum of iron

The term chemical energy is often used to indicate the potential of a chemical substance to undergo a transformation through a chemical reaction or to transform other chemical substances.

Reaction

Main article: Chemical reaction

During chemical reactions, bonds between atoms break and form, resulting in different substances with different properties. In a blast furnace, iron oxide, a compound, reacts with carbon monoxide to form iron, one of the chemical elements, and carbon dioxide.

When a chemical substance is transformed as a result of its interaction with another substance or with energy, a chemical reaction is said to have occurred. A chemical reaction is therefore a concept related to the "reaction" of a substance when it comes in close contact with another, whether as a mixture or a solution; exposure to some form of energy, or both. It results in some energy exchange between the constituents of the reaction as well as with the system environment, which may be designed vessels—often laboratory glassware.

Chemical reactions can result in the formation or dissociation of molecules, that is, molecules breaking apart to form two or more molecules or rearrangement of atoms within or across molecules. Chemical reactions usually involve the making or breaking of chemical bonds. Oxidation, reduction, dissociation, acid–base neutralization and molecular rearrangement are some examples of common chemical reactions.

A chemical reaction can be symbolically depicted through a chemical equation. While in a non-nuclear chemical reaction the number and kind of atoms on both sides of the equation are equal, for a nuclear reaction this holds true only for the nuclear particles viz. protons and neutrons.[31]

The sequence of steps in which the reorganization of chemical bonds may be taking place in the course of a chemical reaction is called its mechanism. A chemical reaction can be envisioned to take place in a number of steps, each of which may have a different speed. Many reaction intermediates with variable stability can thus be envisaged during the course of a reaction. Reaction mechanisms are proposed to explain the kinetics and the relative product mix of a reaction. Many physical chemists specialize in exploring and proposing the mechanisms of various chemical reactions. Several empirical rules, like the Woodward–Hoffmann rules often come in handy while proposing a mechanism for a chemical reaction.

According to the IUPAC gold book, a chemical reaction is "a process that results in the interconversion of chemical species."[32] Accordingly, a chemical reaction may be an elementary reaction or a stepwise reaction. An additional caveat is made, in that this definition includes cases where the interconversion of conformers is experimentally observable. Such detectable chemical reactions normally involve sets of molecular entities as indicated by this definition, but it is often conceptually convenient to use the term also for changes involving single molecular entities (i.e. 'microscopic chemical events').

Ions and salts

The crystal lattice structure of potassium chloride (KCl), a salt which is formed due to the attraction of K+ cations and Cl− anions. The overall charge of the ionic compound is zero.

Main article: Ion

An ion is a charged species, an atom or a molecule, that has lost or gained one or more electrons. When an atom loses an electron and thus has more protons than electrons, the atom is a positively charged ion or cation. When an atom gains an electron and thus has more electrons than protons, the atom is a negatively charged ion or anion. Cations and anions can form a crystalline lattice of neutral salts, such as the Na+ and Cl− ions forming sodium chloride, or NaCl. Examples of polyatomic ions that do not split up during acid–base reactions are hydroxide (OH−) and phosphate (PO43−).

Plasma is composed of gaseous matter that has been completely ionized, usually through high temperature.

Acidity and basicity

Hydrogen bromide exists in the gas phase as a diatomic molecule.

Main article: Acid–base reaction

A substance can often be classified as an acid or a base. There are several different theories which explain acid–base behavior. The simplest is Arrhenius theory, which states that acid is a substance that produces hydronium ions when it is dissolved in water, and a base is one that produces hydroxide ions when dissolved in water. According to Brønsted–Lowry acid–base theory, acids are substances that donate a positive hydrogen ion to another substance in a chemical reaction; by extension, a base is the substance which receives that hydrogen ion.

A third common theory is Lewis acid–base theory, which is based on the formation of new chemical bonds. Lewis theory explains that an acid is a substance which is capable of accepting a pair of electrons from another substance during the process of bond formation, while a base is a substance which can provide a pair of electrons to form a new bond. There are several other ways in which a substance may be classified as an acid or a base, as is evident in the history of this concept.[33]

Acid strength is commonly measured by two methods. One measurement, based on the Arrhenius definition of acidity, is pH, which is a measurement of the hydronium ion concentration in a solution, as expressed on a negative logarithmic scale. Thus, solutions that have a low pH have a high hydronium ion concentration and can be said to be more acidic. The other measurement, based on the Brønsted–Lowry definition, is the acid dissociation constant (Ka), which measures the relative ability of a substance to act as an acid under the Brønsted–Lowry definition of an acid. That is, substances with a higher Ka are more likely to donate hydrogen ions in chemical reactions than those with lower Ka values.

Redox

Main article: Redox

Redox (reduction-oxidation) reactions include all chemical reactions in which atoms have their oxidation state changed by either gaining electrons (reduction) or losing electrons (oxidation). Substances that have the ability to oxidize other substances are said to be oxidative and are known as oxidizing agents, oxidants or oxidizers. An oxidant removes electrons from another substance. Similarly, substances that have the ability to reduce other substances are said to be reductive and are known as reducing agents, reductants, or reducers.

A reductant transfers electrons to another substance and is thus oxidized itself. And because it "donates" electrons it is also called an electron donor. Oxidation and reduction properly refer to a change in oxidation number—the actual transfer of electrons may never occur. Thus, oxidation is better defined as an increase in oxidation number, and reduction as a decrease in oxidation number.

Equilibrium

Main article: Chemical equilibrium

Although the concept of equilibrium is widely used across sciences, in the context of chemistry, it arises whenever a number of different states of the chemical composition are possible, as for example, in a mixture of several chemical compounds that can react with one another, or when a substance can be present in more than one kind of phase.

A system of chemical substances at equilibrium, even though having an unchanging composition, is most often not static; molecules of the substances continue to react with one another thus giving rise to a dynamic equilibrium. Thus the concept describes the state in which the parameters such as chemical composition remain unchanged over time.

Chemical laws

Main article: Chemical law

Chemical reactions are governed by certain laws, which have become fundamental concepts in chemistry. Some of them are:

Avogadro's law

Beer–Lambert law

Boyle's law (1662, relating pressure and volume)

Charles's law (1787, relating volume and temperature)

Fick's laws of diffusion

Gay-Lussac's law (1809, relating pressure and temperature)

Le Chatelier's principle

Henry's law

Hess's law

Law of conservation of energy leads to the important concepts of equilibrium, thermodynamics, and kinetics.

Law of conservation of mass continues to be conserved in isolated systems, even in modern physics. However, special relativity shows that due to mass–energy equivalence, whenever non-material "energy" (heat, light, kinetic energy) is removed from a non-isolated system, some mass will be lost with it. High energy losses result in loss of weighable amounts of mass, an important topic in nuclear chemistry.

Law of definite composition, although in many systems (notably biomacromolecules and minerals) the ratios tend to require large numbers, and are frequently represented as a fraction.

Law of multiple proportions

Raoult's law

History

Main article: History of chemistry

For a chronological guide, see Timeline of chemistry.

The history of chemistry spans a period from the ancient past to the present. Since several millennia BC, civilizations were using technologies that would eventually form the basis of the various branches of chemistry. Examples include extracting metals from ores, making pottery and glazes, fermenting beer and wine, extracting chemicals from plants for medicine and perfume, rendering fat into soap, making glass, and making alloys like bronze.

Chemistry was preceded by its protoscience, alchemy, which operated a non-scientific approach to understanding the constituents of matter and their interactions. Despite being unsuccessful in explaining the nature of matter and its transformations, alchemists set the stage for modern chemistry by performing experiments and recording the results. Robert Boyle, although skeptical of elements and convinced of alchemy, played a key part in elevating the "sacred art" as an independent, fundamental and philosophical discipline in his work The Sceptical Chymist (1661).[34]

While both alchemy and chemistry are concerned with matter and its transformations, the crucial difference was given by the scientific method that chemists employed in their work. Chemistry, as a body of knowledge distinct from alchemy, became an established science with the work of Antoine Lavoisier, who developed a law of conservation of mass that demanded careful measurement and quantitative observations of chemical phenomena. The history of chemistry afterwards is intertwined with the history of thermodynamics, especially through the work of Willard Gibbs.[35]

Definition

The definition of chemistry has changed over time, as new discoveries and theories add to the functionality of the science. The term "chymistry", in the view of noted scientist Robert Boyle in 1661, meant the subject of the material principles of mixed bodies.[36] In 1663, the chemist Christopher Glaser described "chymistry" as a scientific art, by which one learns to dissolve bodies, and draw from them the different substances on their composition, and how to unite them again, and exalt them to a higher perfection.[37]

The 1730 definition of the word "chemistry", as used by Georg Ernst Stahl, meant the art of resolving mixed, compound, or aggregate bodies into their principles; and of composing such bodies from those principles.[38] In 1837, Jean-Baptiste Dumas considered the word "chemistry" to refer to the science concerned with the laws and effects of molecular forces.[39] This definition further evolved until, in 1947, it came to mean the science of substances: their structure, their properties, and the reactions that change them into other substances – a characterization accepted by Linus Pauling.[40] More recently, in 1998, Professor Raymond Chang broadened the definition of "chemistry" to mean the study of matter and the changes it undergoes.[41]

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Chemistry

Man has been exposed to changing surroundings ever since he came into existence. He has been quite interested in learning about his surroundings and studying and explaining the things that are happening around him. He has conducted experiments and observations to gather information as a result of his interest. Through the decades, it has also been in charge of many people’s research endeavours around the globe. Systematizing and organising the knowledge acquired in this way was absolutely necessary for the good of humanity.

Science is the name given to this knowledge. So, systematised knowledge that humans have acquired through observations and experimentation may be referred to as science. Due to its vast expansion and variety of subjects, science has been further divided into many branches.

One of the most significant fields of science is chemistry. Chemistry can be summed up as the area of science that studies matter, including its properties, composition, and the changes that occur to it as a result of various activities. Several branches of chemistry have been created based on the specialised disciplines of research.

Table of Content

IntroductionBranches of ChemistryExamples in Daily LifeFree Study MaterialCBSE Chemistry ResourcesFAQs

What is Chemistry?

Chemistry is a subdiscipline of science that deals with the study of matter and the substances that constitute it. It also deals with the properties of these substances and the reactions undergone by them to form new substances. Chemistry primarily focuses on atoms, ions, and molecules which, in turn, make up elements and compounds. These chemical species tend to interact with each other through chemical bonds. It is important to note that the interactions between matter and energy are also studied in the field of chemistry.

The study of elements and compounds’ properties, compositions, and structures, as well as how they can change and the energy that is released or absorbed during such changes, is the subject matter of the science known as chemistry.

Learn more on Interactive Periodic Table

Relationship Between Chemistry and Other Branches of Science

‘Science’ can be defined as the systematic study of the natural universe, its structure, and everything it encompasses. Due to the immensity of the natural universe, science has been divided into several disciplines that deal with certain aspects of the universe. The three primary subcategories of science under which these disciplines can be grouped are:

The Formal Sciences: Involves the study of the language disciplines that concern formal systems. Examples of scientific disciplines that fall under this category include logic and mathematics. Can be thought of as the “language of science”.

The Natural Sciences: Involves the study of natural phenomena through experiments and observations. Chemistry, physics, and biology fall under this category of science.

The Social Sciences: Involves the study of human societies and the relationships between the humans that dwell in these societies. Examples of scientific disciplines that fall under this category include psychology, sociology, and economics.

When the relationships between the major branches of science are considered, chemistry is found to lie close to the centre (as illustrated below).

Thus, chemistry can be viewed as a central science whose roots bore into several other subdisciplines of science.

Branches of Chemistry

The five primary branches of chemistry are physical chemistry, organic chemistry, inorganic chemistry, analytical chemistry, and biochemistry. Follow the buttons provided below to learn more about each individual branch.

Organic Chemistry

Inorganic Chemistry

Physical Chemistry

Biochemistry

Analytical Chemistry

Chemistry Reactions

Apart from these primary branches, there exist several specialized fields of chemistry that deal with cross-disciplinary matters. Some such examples include medicinal chemistry, neurochemistry, materials chemistry, nuclear chemistry, environmental chemistry, polymer chemistry, and thermochemistry.

Examples of Chemistry in Our Daily Lives

Chemical reactions are constantly taking place around us. The human body facilitates thousands of chemical reactions every day. From the digestion of food to the movement of muscles – all bodily actions involve chemical reactions. A few other examples of chemistry in the day-to-day lives of humans are listed below.

The process of photosynthesis that enables plants to convert water, sunlight, and carbon dioxide into glucose and oxygen is a chemical reaction. This process is the foundation upon which the entire food chain is built.

Soaps and detergents used for hygiene work use a chemical process known as emulsification. Furthermore, they are produced using a chemical process known as saponification.

Even the sunscreen used by humans to protect themselves from the harmful UV-A and UV-B radiation of the sun is based on chemistry. These lotions and creams consist of a combination of inorganic and organic compounds that either filter or block the incoming ultraviolet radiation.

Follow the link to learn more about the importance of chemistry in everyday life.

Free Chemistry Study Material

The BYJU’S chemistry section hosts over 1500 chemistry articles for students to use as free study resources. Links to each of these articles have been sorted under their parent concepts and can be found in the collapsible tables provided below.

Acids, Bases, and Salts

Base Meaning

Properties of Bases

Dilute Acids

List of Strong Acids

Weak Acid Examples

Weak Base

Red Cabbage Indicator

Barium Carbonate

Aluminium Phosphate

Neutralization In Everyday Life

Acid Test

Butanoic Acid

Perchloric Acid

Acid Strength

Calculate Ph Of Weak Acid

Hydrobromic Acid

Hypochlorite

Di And Polybasic Acids And Bases

Uses Of Acetic Acid

Hydroiodic Acid

Oxalate

Neutralization

Uses Of Benzoic Acid

Sodium Chlorate

Sulfurous Acid

Ph Of Acids And Bases

Uses Of Citric Acid

Potassium Iodate

Potassium Carbonate

Antacids

Uses Of Folic Acid

Sodium Percarbonate

Sodium Citrate

Acid Anhydrides

Uses Of Sodium Hydroxide

Hydrocyanic Acid

Hypochlorous Acid

Henderson-Hasselbalch Equation

Uses Of Sulfuric Acid

Formic Acid

Ammonium Acetate

Ionisation Of Acids And Bases

Uses Of Oxalic Acid

Dinitrogen Pentoxide

Butyric Acid

Acids And Bases

Uses Of Ascorbic Acid

Phosphorous Acid

Zinc Nitrate

Difference Between Acid And Base

Uses Of Hydrochloric Acid

Peroxydisulfuric Acid

Zinc Acetate

Chromate

Uses Of Nitric Acid

Hypoiodous Acid

Magnesium Nitrate

Sodium Hexametaphosphate

Uses Of Ammonia

Monopotassium Phosphate

Zinc Phosphate

Potassium Bromate

Difference Between Alkali And Base

Dipotassium Phosphate

Potassium Oxide

Magnesium Bicarbonate

Difference Between Sodium Carbonate And Sodium Bicarbonate

Aluminium Hydroxide

Barium Hydroxide

Dichromate

Difference Between Acetic Acid And Glacial Acetic Acid

Sodium Borate

Barium Iodide

Lithium Hydroxide

Carboxylic Acid Formulas

Chloroacetic Acid

Magnesium Phosphate

Trichloroacetic Acid

Lactic Acid Formula

Sodium Dichromate

Salts Types Hydrolysis

Stearic Acid

Lewis Acids And Bases

Copper Hydroxide

Chemical Indicators

Magnesium Hydroxide

Examples Of Bases

Experiments On Properties Of Acids And Bases

Propertries Of Acids And Bases

Potassium Hydroxide

Acetate

Properties Of Acetic Acid Experiment

Ammonium Phosphate

Zinc Carbonate

Nitrous Acid

Aspartic Acid

Hydroxide

Zinc Hydroxide

Chromic Acid

Arrhenius Acid

Salt Hydrolysis

Tannic Acid

Alcohols, Phenols, and Ethers

Uses Of Propanol

Ester Hydrolysis

Phenol Acidity

Bismuth Subsalicylate

Difference Between Alcohol And Phenol

Electrophilic Substitution Reactions Of Phenols

Ether Preparation

Eugenol

Ethanol Formula

Structure Of Alcohols: The Hydroxyl Group

Uses Of Ethers Health Care Industry

Methyl Acetate

Difference Between Ester And Ether

Dehydration Of Alcohols

Phenols Nomenclcature

Phenyl

Mannitol

Ester

Properties Of Ethers

Potassium Acetate

Lucas Test

Physical And Chemical Properties Of Alcohols

Epoxide

Esterification

Benzyl Alcohol

Preparation Of Phenols

Nomenclcature Of Ethers

Uses Of Phenol

Isopropyl Alcohol

Types Of Alcohols

Identification Of Alcohols

Ethanol

Resorcinol

Phenolic Acid

Nomenclature Of Substituted Benzene Compounds

Phenol Physical Chemical Properties

Aldehydes, Ketones, and Carboxylic Acids

acetaldehyde

tollens test

Aldehyde Group

uses of acetone

carboxyl group

physical properties of aldehydes and ketones

formaldehyde

uses of formaldehyde

carboxylic acids acidity

aldehydes and ketones

preparation of dibenzal acetone

formaldehyde formula

uses of carboxylic acids

lactones

test for carboxyl group

difference between aldose and ketose

nomenclature of aldehydes

how to prepare carboxylic acids

preparation of aldehydes

difference between aldehydes and ketones

carbonyl compounds

carboxylic acid properties

ketone preparation

Amines

brown ring test

Phthalimide

difference between nitrate and nitrite

reactions of diazonium salts

uses of amines

dimethylglyoxime

nitrite

oxyacids and ammonia

reactions of amines

acetamide

carbylamine reaction mechanism

nitro compounds

reactions of diazonium salts

hexamine

schmidt reaction

chemical reactions of amines

classification of amines

ammonia and nitric acid formula

zwitterion

oximes

diazonium salts

anilines

kjeldahl method

identification of amines

nitriles

physical properties of amines

Analytical Chemistry

mass spectrometry

spectrophotometer principle

partition chromatography

thin layer chromatography principle

difference between endpoint and equivalence point

volumetric analysis

acid base titration

column chromatography principle

potentiometric titration

gravimetric analysis

color spectrum

non aqueous titration

paper chromatography

infrared spectroscopy

colorimeter

precipitation titration

column chromatography

types of titration

complexometric titration

karl fischer titration

thin layer chromatography

chromatography

spectroscopy

conductometric titration

adsorption chromatography

redox titration

nmr spectroscopy

Uses of Colorimeter

Principle of Uv Visible Spectroscopy

Volhard Method

Classification of Chromatography

Applications of Electrophoresis

Applications of Centrifugation

Uses of Centrifuge

Applications of Chromatography

Atoms and Molecules

argon gas

Isotope Meaning

Element Definition

homonuclear diatomic molecules

molarity

mole concept basics

isotopic mass

difference between atom and molecule

molality

variations of molar conductivity

molecular motion

difference between elements and atoms

mole concept, molar mass, and percentage composition

atomic mass molecular mass

an introduction to atomic number, isotopes and isobars

difference between atom and ion

isotopes and isobars

positron

atomic mass and molecular mass

van der waals forces

law of constant proportions

difference between anions and cations

elements and compounds

Biomolecules

Difference Between Fats And Oils

Complex Carbohydrates

Vitamins Types

Structure Of Glucose And Fructose

Difference Between Glucose And Fructose

Omega 3 Fatty Acids

Glycogen

Amylose

Difference Between Fat And Cholesterol

Asparagine Amino Acid

Lactose

Maltose

Difference Between Herbicides And Pesticides

Protein Structure And Levels Of Protein

Glycine Structure

Monomeric Proteins

Polysaccharides

Disaccharides

Peptides

Tryptophan

Difference Between Starch And Cellulose

The Chemistry Behind Enzyme Catalysis

Monosaccharides

Glycosaminoglycans

Linseed Oil

Function Of Nucleic Acids

Functioning Of Hormones

Enzymes Properties

Monosodium Glutamate

Classification Of Carbohydrates And Thier Structure

Sugar Alcohol

Nucleic Acids

Fehling Test

Importance Of Polysaccharides

Fructose

Denaturation Of Proteins And Its Causes

Carbon and its Compounds

Tetravalency Of Carbon

Carbon Compounds

What Are The Physical And Chemical Properties Of Carbon

Allylic Carbon

Graphite

Difference Between Organic And Inorganic Compounds

Chemical Properties Of Carbon Compounds

Carbon And Its Importance

Anomalous Behaviour Of Carbon

Carbon Dating

Uses Of Oxides Of Carbon Group

CBSE Chemistry

Chemistry Syllabus

Important Questions For Class 12 Chemistry: Chapter 12

Important Questions For Class 12 Chemistry: Chapter 6

Cbse Class 11 Chemistry Practical Syllabus

Tips To Get 90 Marks In Cbse Class 12 Chemistry

Important Questions For Class 11 Chemistry: Chapter 7

Important Questions For Class 12 Chemistry: Chapter 9

Cbse Class 12 Chemistry Practical Syllabus

Mistakes To Avoid In Cbse Class 12 Chemistry Board Exam

Important Questions For Class 12 Chemistry: Chapter 16

Important Questions For Class 12 Chemistry: Chapter 14

Important 5 Marks Questions For Cbse Class 11 Chemistry

Important 3 Marks Questions For Cbse Class 11 Chemistry

Important Questions For Class 11 Chemistry: Chapter 13

Important Questions For Class 12 Chemistry: Chapter 5

Important 3 Marks Questions For Cbse Class 12 Chemistry

Important 2 Marks Questions For Cbse Class 11 Chemistry

Important Questions For Class 12 Chemistry: Chapter 8

Important Questions For Class 12 Chemistry: Chapter 3

Important Questions Class 12 Chemistry

Important 5 Marks Questions For Cbse Class 12 Chemistry

Important Questions For Class 12 Chemistry: Chapter 15

Important Questions For Class 12 Chemistry: Chapter 1

Chemistry Important Questions

Important 2 Marks Questions For Cbse Class 12 Chemistry

Important Questions For Class 12 Chemistry: Chapter 13

Important Questions For Class 12 Chemistry: Chapter 10

Tips For Cbse Class 12 Chemistry

Cbse Chemistry Important Questions

Important Questions For Class 11 Chemistry: Chapter 10

Important Questions For Class 12 Chemistry: Chapter 4

Important Questions For Class 11 Chemistry: Chapter 1

Marks Wise Cbse Important Questions

Important Questions For Class 11 Chemistry Chapter 12

Important Questions For Class 12 Chemistry: Chapter 11

Important Questions For Class 11 Chemistry: Chapter 2

Chemical Reactions And Equations Class 10 Questions Answers

Important Questions For Class 12 Chemistry Chapter 2: Solutions

Important Questions For Class 12 Chemistry: Chapter 7

Important Questions For Class 11 Chemistry:Chapter 3

Important Questions Class 11 Chemistry

Chemical Reactions For Cbse Class 12

Important Questions For Class 11 Chemistry: Chapter 11

Important Questions For Class 11 Chemistry: Chapter 4

Important Questions Class 11 Chemistry:Chapter 5

Important Questions Class 11 Chemistry:Chapter 6

Important Questions Class 11 Chemistry:Chapter 8

Important Questions Class 11 Chemistry: Chapter 14

Important Questions Class 11 Chemistry:Chapter 9

Chemical Bonding and Molecular Structure

Bond Energy

Molecular Structure

Lewis Dot Structures

Chemical Energy

Pcl5 Hybridization

Resonance Effect

Quantum Numbers

Ionic Bond Or Electrovalent Bond

Ionic Bond – Partially Covalent In Nature

Difference Between Ionic, Covalent And Metallic Bonds

Sigma And Pi Bonds

Octet Rule

Single Bond Double Bond And Triple Bond

Difference Between Sigma And Pi Bond

Metallic Bonds

Formal Charge And Its Properties

Limitations Of Octet Rule

Difference Between Polar And Non Polar

Intermolecular Forces Vs Thermal Interactions

Formation Of Ionic Compounds

Bond Parameters

Optical Rotation

Dipole Moment

Standard Enthalpy Of Formation, Combustion, And Bond Dissociation

Valence Bond Theory Linkages In Coordination Compounds

Pi Bonds

Valence Bond Theory

Conditions For The Linear Combination Of Atomic Orbitals

Orbital Overlap

Structure Of Acetylene

Polar Compounds

Atomic Orbitals

Ion Definition

Chemical Compounds

Ethyne

Potassium Ferricyanide

What is DDT?

Glaubers Salt

Difference Between Molecule And Compound

Chemical Formula

Ferrous Sulfate

Methyl Salicylate

Difference Between Element And Compound

Calcium Oxide

Potassium Thiocyanate

Diethyl Ether

Uses Of Minerals

Mass Production Of Sulphuric Acid

Lead Acetate

Nitride

Difference Between Ethanol And Methanol

Ethanoic Acid

Phosphorus Trichloride

Titanium Dioxide

Benzoyl Peroxide

The Story Of Washing Soda

Phosphorus Pentachloride

Methyl Ethyl Ketone

Sodium Chloride

Histidine

Sulfur Hexafluoride

Methylene Blue

Sodium Hydroxide

Caco3

Potassium Ferrocyanide

Zinc Oxide

Ammonium Chloride

Kmno4

Xenon Difluoride

Ammonium Dichromate

Phosphoric Acid

Na2Co3

Phosphorus Triiodide

Acetonitrile

Nitric Acid

Nahco3

Barium Bromide

Hydrazine

Lactic Acid

Acetic Acid

Barium Oxide

Anthocyanins

Salicylic Acid

Glucose

Lithium Bromide

Ferric Chloride

Cellulose

Hydrochloric Acid

Cr2O3

Thiourea

Citric Acid

Oxalic Acid

Nahso4

Sodium Sulfide

Phenol

Sodium Hypochlorite

Copper Dichloride

Magnesium Chloride

Chlorine

Acetone

Mercuric Chloride

Sodium Silicate

Calcium Hydroxide

Glycerin

Preparation Properties And Uses Baking Soda

Sodium Dihydrogen Phosphate

Ethylene Glycol

Urea

Sulphur Dioxide

Urethane

Hydroquinone

Sucrose

Properties Of Ddt

Silver Chloride

Potassium Chloride

Ammonia

Iodoform

Iron Oxide

Carbonic Acid

Nitrous Oxide

Glutamic Acid

Gum Arabic

Acetone Formula

Ascorbic Acid

Preparation, Properties, And Uses Of Dioxygen

Manganese Dioxide

Acetylene Formula

Cyanide

Baking Soda, Washing Soda, And Plaster Of Paris

Sodium Fluoride

Ammonium Chloride Formula

Phenolphthalein

Serine

Carbon Disulfide

Borax Formula

Boric Acid

Calcium Sulphate

Nitrogen Dioxide

Citric Acid Formula

Methane

Silver Oxide

Magnesium Carbonate

Ethyl Acetate Formula

Sulfuric Acid

Schiff Bases

Silicon Dioxide

Glycerol Formula

Methanol

Calcium Carbonate

Bromothymol Blue

Potassium Nitrate

Tartaric Acid

Sodium Sulfate

Hydrogen Sulfate

Sodium Thiosulfate

Pyridine

Bicarbonates

Calcium Acetate

Barium Sulfate

Carbon Monoxide

Silver Nitrate

Sodium Cyanide

Cuso4

Benzoic Acid

Thiol

Ammonium Bicarbonate

K2Cr2O7

Ammonium Sulfate

Glutamine

Barium Nitrate

Al2O3

Lindlar Catalyst

Proline

Lead Iodide

Cacl2

Wilkinsons Catalyst

Bleaching Powder And Sodium Hydroxide

Sodium Iodide

Mgso4

Phosphorus Pentoxide

Preparation, Properties, And Uses Of Sodium Chloride

Sodium Bromide

Zinc Sulfate

Phosphorus Oxychloride

Lysine

Sodium Oxide

Phosphate

Sodium Borohydride (Nabh4)

Grignard Reagent

Sodium Phosphate

Aluminium Sulfate

Raney Nickel

Preparation, Properties, And Uses Of Caustic Soda

Sulfur Trioxide

Calcium Carbide

Iron Oxide (Fe3O4)

Acetylsalicylic Acid

K2Cro4

Potassium Iodide

Calcium Phosphate

Ammonium Nitrate

Potassium Bicarbonate

Sodium Acetate

Zinc Chloride (Zncl2)

Fe2O3

K2So4

Ammonium Hydroxide (Nh4Oh)

Sodium Nitrate (Nano3)

Malonic Acid

Potassium Chlorate

Ammonium Oxalate

Sodium Potassium Tartrate

Sodium Metabisulfite

Sodium Sulfite

Calcium Hypochlorite

Calcium Nitrate

Dihydrogen

2-4 Dinitrophenylhydrazine

Chemical Kinetics

Order Of Reaction

How Do Catalysts Affect The Rate Of Chemical Reactions

Collision Theory

Arrhenius Equation

Difference Between Effusion And Diffusion

Pseudo First Order Reaction

Limiting Reagent

Integrated Rate Equation

Zero Order Reaction

Half Life

Rate Law

Activity Selectivity Of Catalyst

Second Order Reaction

Rate Of Reaction

Predicting The Direction Of A Reaction

Catalysis

The Collision Theory Of Chemical Reactions

Structure of Zeolites

Heterogeneous Catalyst

Chemical Reactions and Equations

Combustion Reaction

List Of Chemical Reactions

Nuclear Reaction

Stoichiometric Calculations

Hinsberg Reagent And Test

Balancing Chemical Equations

Addition Reaction

Types Of Chemical Reactions

Diazotization Reaction Mechanism

Decomposition Reaction

Decarboxylation Reaction

Balanced Chemical Equations

Fractional Distillation

Neutralization Reaction

Displacement Reactions

Types Of Chemical Reactions

Elimination Reaction

Exothermic Reaction

Decomposition

Endothermic Reaction

Ziegler Natta Catalyst

Difference Between Oxidation And Reduction

Temperature Dependence Of Chemical Reactions

Chemical Reactions In Everyday Life

Types Of Reactions Experiment

Difference Between Nuclear Reaction And Chemical Reaction

Photochemical Reaction

Difference Between Fission And Fusion

Reactivity Series Experiment

Difference Between Sn1 And Sn2

Substitution Reaction

Precipitation Reaction

Chemical Equation

Hydrolysis

Difference Between Erosion And Corrosion

Precipitation

What is Pyrolysis

Chemistry in Everyday Life

Saponification

Antihistamines

Catabolism

Examples Of Tranquilizers And Antidepressant Drugs

Uses Of Solar Energy

Pesticides

Micelle

Chemicals Used As Food Preservatives

Hydrogen Gas

Soaps And Detergents

Food Chemistry

Drugs And Drug Interactions

Pbo2

Antimicrobial Agents

Harmful Effects Of Radiation

Carbon Monoxide Poisoning

Study The Comparative Cleaning Capacity Of A Sample Of Soap In Soft And Hard Water

Antifertility Drugs

Analgesics: Classification Of Analgesic Drugs

Classification Of Drugs

Anabolism

Science In Everyday Life And Its Importance

Antibiotics: Types And Side Effects

Artificial Sweeteners And Sweetening Agents

Insecticides

Important Compounds Of Silicon

Antioxidants

Antiseptics And Disinfectants

Hard Water and Soft Water

Examples of Antioxidants

Classification of Elements and Periodicity in Properties

What are Noble Gases

Electropositivity

Valence Electrons

Newlands Law Of Octaves

Periodic Properties Of Elements

Chalcogens

Electron Gain Enthalpy

Enthalpy Of Atomisation

Periodicity Of Valence Or Oxidation States Of Elements

Electronegativity Chart

Ionization Enthalpy

Trends In Periodic Properties

Electronic Configuration Of Elements And Stability Of Orbitals

Oxidation State

Difference Between Atomic Mass And Atomic Number

Trends In The Modern Periodic Table

Nomenclature Of Elements With Atomic Number Greater Than 100

Development Of Modern Periodic Table

Difference Between Electronegativity And Electron Affinity

Atomic Radius In The Periodic Table

Ionisationenthalpy

Periodic Trends In Ionisation Enthalpy Of Elements

Atomic Mass Of Elements

Periodic Properties Of Elements And Their Significance

Electron Affinity

Electronegativity Of Elements In Modern Periodic Table

How To Find Atomic Mass

Modern Periodic Table

Electronegativity

Periodic Trends Of Ionic Radii In Modern Periodic Table

Electromeric Effect

Modern Periodic Table And Modern Periodic Law

Memorizing The Periodic Table

Hydrogen Position In The Periodic Table

Electronic Configuration Of First 30 Elements

Mendeleev Periodic Table

Electronic Configuration Trends Across Periods And Groups

Electron Gain Enthalpy Of Elements In Modern Periodic Table

Coal and Petroleum

LPG Composition

Fossil Fuels And Their Impact On Habitats

Nuclear Power Plant

Petroleum

Uses Of Coal

Nuclear Chemistry

Fuel Types

Coal Story

Uses Of Petroleum

Effects Of Burning Fossil Fuels

Formation Of Fossil Fuels

Fuel Effeciency

Types Of Natural Resources

Uses And Advantages Of Natural Gas

Nuclear Energy

Nuclear Power Plant Working

Combustion and Flame

Difference Between Diesel And Petrol Engine

Fire Extinguisher

Combustion Fuels

Candle Flame

Combustion and Flames

Difference Between Articles

Difference Between Evaporation And Boiling

Difference Between Hard Water And Soft Water

Difference Between Accuracy And Precision

Difference Between Endothermic And Exothermic Reactions

Difference Between Baking Soda And Baking Powder

Electrochemistry

Daniell Cell

Fuel Cell

Basic Concepts Of Emf And Cell Notation

Conductors

Concentration Cell

Electrochemistry (Pdf)

Battery Types

Lead-Acid Battery

Standard Hydrogen Electrode

Difference Between Cell And Battery

Galvanic Cell

Electrochemical Cell

Cathode And Anode

Difference Between Primary Cell And Secondary Cell

Specific Conductivity And Molar Conductivity

Electrolysis Products

Electrolytic Conductance Factors Affecting Conductance

Electrodes

Laws Of Electrolysis

Standard Electrode Potential

Electrophoresis Technique Used For Dna Analysis

Difference Between Galvanic Cells And Electrolytic Cells

Kohlrausch Law

Nonelectrolyte

Battery Definition

Elements of the Periodic Table

Sodium

First 20 Elements

Helium

Lawrencium

Calcium

Ununoctium

Fluorine

Bohrium

Titanium

Ununpentium

Neon

Berkelium

Phosphorus

Actinium

Magnesium

Neptunium

Scandium

Radium

Aluminum

Uranium

Iron

Seaborgium

Arsenic

Americium

Argon

Thorium

Rubidium

Nobelium

Cobalt

Curium

Europium

Mercury

Potassium

Rutherfordium

Molybdenum

Protactinium

Nickel

Californium

Ruthenium

Fermium

Vanadium

Erbium

Tellurium

Plutonium

Manganese

Mendelevium

Xenon

Francium

Gallium

Lead

Neodymium

Radon

Selenium

Hassium

Niobium

Bismuth

Bromine

Dysprosium

Iodine

Gadolinium

Silver

Gold

Hydrogen

Thallium

Palladium

Germanium

Yttrium

Polonium

Nihonium

Dubnium

Cesium

Astatine

Meitnerium

Einsteinium

Nitrogen

Tungsten

Antimony

Lanthanum

Carbon

Platinum

Darmstadtium

Lithium

Promethium

Terbium

Flerovium

Zirconium

Silicon

Osmium

Ununseptium

Barium

Strontium

Lutetium

Livermorium

Sulfur

Oxygen

Tantalum

Tin

Krypton

Boron

Iridium

Rhodium

Copper

Samarium

Holmium

Technetium

Chromium

Praseodymium

Rhenium

Cadmium

Zinc

Cerium

Hafnium

Copernicium

Roentgenium

Beryllium

Thulium

Indium

Ytterbium

Environmental Chemistry

Droughts

Properties Of Soil

Waste Management And Garbage Disposal

Difference Between Evaporation And Condensation

Deforestation

Oxygen Cycle

Forest Conservation

Acid Rain

Ozone Layer

Soil Formation

Sewage Management Methods

Leaching Process

Nuclear Fuel Cycle

Dependence Of Life On Water

Importance Of Forests

Ozone

Natural Resources (Pdf)

Carbon Tetrachloride And Its Effects On The Environment

Interdependence Of Plants And Animals

Biodegradable And Non Biodegradable Polymers

Environmental Chemistry (Pdf)

Global Warming Due To The Greenhouse Effect

Industrial Waste And Its Types

Dichloromethane The Uses And Effects On Environment

Agricultural Chemistry

Ecosystem Components

Reforestation

Uses Of Chloroform

Plastic Pollution

Effects Of Ozone Layer Depletion

Environmental Pollution

Atmospheric Pollutants And The Reactions

Uses Of Fossil Fuels

Biodegradable And Non Biodegradable Waste

Recycling Of Waste Product

Strategies To Control Pollution And Reduce Waste

Difference Between Vaporization And Evaporation

Importance Of Air

Sewage

Green Chemistry The Alternative Tool

Difference Between Thermoplastic And Thermosetting Plastic

Drainage Systems

Waste

Carcinogenicity And Toxicity

Difference Between Cng And Lpg

Soil Pollution

Eutrophication

Freons Ddt Carbontetrachloride

Recycling Of Paper

Natural Resources

Environmental Toxicology

Water Cycle And The Processes Involved

Sericulture And Health Problems

Scarcity Of Products For Sustenance

Which Gases Cause Acid Rain

Effects of Radioactive Pollution

What is Green Chemistry

Effects of Environmental Pollution

Effects of Acid Rain

Equilibrium

Steady State

Law Of Mass Action Or Law Of Chemical Equilibrium

Homogeneous Equilibrium

Solubility Product Constant

Equilibrium Involving Dissolution Of Solid Or Gases

Energy Change Due To Equilibrium

Calculating Equilibrium Concentrations

Heterogeneous Equilibrium

Common Ion Effect

Fibre to Fabric

Man Made Fibres

Synthetic Rubber

Natural Fibres

Moriculture

Animal Fibre

Jute Fibre

Sericulture

Types of Fabric

Cotton Cultivation

Extraction Of Wool

Nylon Fabric And Polyester Fibres

Silkworm

Clothing Fabric

Introduction To Wool

Silk

Plant Fibers

Fibrous Materials Uses

Sericulture Rearing Of Silkworm

General Principles and Processes of Isolation of Elements

Zone Refining

Types Of Minerals

Extraction Of Iron

Rocks And Minerals

Haber Process

Extraction Of Metals From Ores And Minerals

Ores And Minerals

Processes Of Metallurgy

Zinc Extraction Metallurgy

Concentration Of The Ore

Mineral Resources

Extraction Of Copper

Extraction Of Crude Metal From Concentrated Ore

Steam Distillation

Refining

Occurrence And Extraction Of Aluminium

Haloalkanes and Haloarenes

Zone Refining

Types Of Minerals

Extraction Of Iron

Rocks And Minerals

Haber Process

Extraction Of Metals From Ores And Minerals

Ores And Minerals

Processes Of Metallurgy

Zinc Extraction Metallurgy

Concentration Of The Ore

Mineral Resources

Extraction Of Copper

Extraction Of Crude Metal From Concentrated Ore

Steam Distillation

Refining

Occurrence And Extraction Of Aluminium

Halogenation of Alkanes

What are Minerals

HydrocarbonsHydrocarbons

Thermoplastic Polymers

Alkene

Physical And Chemical Properties Of Benzene

Aromatic Hydrocarbons

Physical Properties Of Alkynes

Methylene

Conformation

Benzene

Methods Of Preparation Of Alkenes

Butane

Preparation Of Benzene

Structure Of Benzene

Influence Of Functional Group In Mono Substituted Benzene

Ethane

Nomenclature Of Saturated Hydrocarbons

Aromaticity

Chemical Properties Of Alkenes

Ethylene

Preparation Of Alkanes

Triple Bond In Alkynes

Electrophilic Addition Alkenes

Acetylene

Unsaturated Hydrocarbons

Addition Reactions Of Alkynes

Alkynes Acidity

Propane

Saturated Hydrocarbons

Electrophilic Substitution Of Benzene

Toluene

Isomers Of Butane

Aliphatic Hydrocarbons

Nomenclature Of Alkanes, Alkenes, And Alkynes

Alkanes

Oxidative Cleavage Of Alkenes Ozonolysis

Conformation Of Cyclohexane

Preparation Of Alkynes

Physical Properties Of Alkenes

Physical Properties Of Alkanes And Their Variations

Xylene

Pyrolysis Of Hydrocarbons

Cycloalkanes

Physical Properties Of Alkenes

Hexane

Aromatic Compounds

Combustion Of Alkanes

Conformers

Hydrogen

Hydrogen Fuel

Uses Of Hydrogen

Isotopes Of Hydrogen

Preparation Of Hydrogen And Its Various Uses

Hydrogen Chloride

Laboratory Preparation of Hydrogen Gas

Protium

Is Matter Around Us Pure?

Pure Substances And Mixtures

Condensation

Filtration

Separation Techniques

Difference Between Compound And Mixture

Mixtures

Handpicking

Sieving

Salt Water

Heterogeneous And Homogeneous Mixtures

Separation

Separation Techniques For Obtaining Gases From Air

Uses Of Air

Distillation

Threshing

What Are Homogenous Mixtures

Difference Between Pure Substance And Mixture

Decantation

Physical Separation Methods

Crystallization

Separation Of Mixtures

Centrifugation

Sedimentation

Winnowing

Components Of Air

Destructive Distillation

Azeotropic Distillation

Materials: Metals and Non-metals

Alloy Meaning

Chemical Properties Of Metals

Sorting Materials Into Groups

Barium Chloride

Silver Carbonate

Strontium Chloride

Materials

Sncl2

Metalloids

Matter in Our Surroundings

Chemistry: The Study Of Matter

Intensive And Extensive Properties Of Matter

Difference Between Ideal Gas And Real Gas

Uses Of Water

Physical Nature Of Matter

Characteristics Of Particles Of Matter

Evaporation Causes Cooling

List of Strong Acids

Named Reactions

Wurtz Reaction

Aldol Condensation

Reformatsky Reaction

Hoffmann Bromamide Reaction Mechanism

Gattermann Reaction

Clemmensen Reduction

Schotten Baumann Reaction

Perkin Reaction Mechanism

Anti Markovnikov Addition

Friedel Crafts Alkylation And Acylation

Hunsdiecker Reaction

Diels Alder Reaction Mechanism

Cannizzaro Reaction Mechanism

Wittig Reaction

Dehydration Synthesis

Ozonolysis Of Alkenes Alkynes Mechanism

Etard Reaction Mechanism

Maillard Reaction

Coumarin Synthesis

Gattermann Koch Reaction Mechanism

Balz Schiemann Reaction Mechanism

Coupling Reaction

Oppenauer Oxidation

Michael Addition Mechanism

Ronsenmund Reduction Mechanism

Acetylation

Robinson Annulation

Birch Reduction Mechanism

Grignard Reaction Mechanism

Biuret Test

Woodward Reaction

Hofmann Elimination

Gabriel Phthalimide Synthesis Mechanism

Molischs Test

Williamson Ether Synthesis

Heck Reaction

Stephen Reaction Mechanism

Benedicts Test

Benzoin Condensation

Mannich Reaction Mechanism

Wolff Kishner Reduction Mechanism

Fries Rearrangement

Finkelstein Reaction

Claisen Condensation Mechanism

Wurtz Fittig Reaction Mechanism

Ninhydrin Test

Mitsunobu Reaction

Swern Oxidation

Swarts Reaction

Transesterification

Sonogashira Coupling

Claisen Rearrangement

Fischer Esterification Mechanism

Ullmann Reaction

Curtius Rearrangement

Suzuki Coupling Reaction

Hell Volhard Zelinsky Reaction Mechanism

Methylation

Beckmann Rearrangement

Pinacol Pinacolone Rearrangement

Haloform Reaction Mechanism

Corey House Reaction

Organic Chemistry

Conformational Isomers

Nucleophile

Epimers

Reaction Due To Alpha Hydrogen

Difference Between Electrophile And Nucleophile

Huckel Rule

Cracking Meaning

Functional Groups

Difference Between Cis And Trans

Electrophilic Aromatic Substitution

Difference Between Allotropes And Isomers

Nomenclature Of Organic Compounds

Difference Between Enantiomers And Diastereomers

Non Aromatic Compounds

Phosphorylation

Homologous Series

Electrophilic Substitution Reaction Mechanism

Carbocation Stability

Organometallic Compounds

Benzene Reactions

Sn2 Reaction Mechanism

Isomerism

Organometallic Chemistry

Classification Of Organic Compounds

Sn1 Reaction Mechanism

Types Of Organic Reactions

Cis-Trans Isomerism

Homolytic And Heterolytic Fission

Hydroboration Oxidation Reaction

Electrophilic Substitution

Organic Compounds: Structural Representation

Nucleophilic Addition Reactions

Markovnikov Rule

Metal Carbonyls And Organometallics

Chriality, Recemisation, And Optical Activity

Salt Analysis

Benzene Hexachloride

Organic Solvents

Nomenclature Of Functional Groups

Quantitative Analysis

Rearrangement Reaction

Uses of Rayon

Examples of Enantiomers

Constitutional Isomers

What are Enantiomers

Periodic Classification of Elements

Isotopes Of Elements

Periodic Table Elements

Inner Transition Elements

Physical and Chemical Changes

Crystal Salt

Physical Change

Melting Point

Examples Of Chemical Change

Difference Between Physical And Chemical Change

Reversible And Irreversible Changes

Rusting Of Iron

Chemical Change

Physical And Chemical Changes

Chemical And Physical Changes

Physical Change And Chemical Change

Electrolytes

Pollution of Air and Water

Potable Water

Causes Of Water Pollution

Conservation Of Water

Importance Of Water

Water Management

Water Contamination

Atmospheric Pollution Due To Smog

Water

Drinking Water Standards

Scarcity Of Water

Air Pollution

Physical And Chemical Properties Of Water

Photochemical Smog

Polymers

Advantages and Disadvantages of Plastic

Polyurethane

Polyethylene

Polypropylene

Uses of Rubber

Monomers

Properties of Plastics

Protein Definition

Difference Between Addition And Condensation Polymerization

Nylon

Preparation Of Polythene And Teflon

Differentiate Natural Polymers From Synthetic Polymers

Polystyrene

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Frequently Asked Questions on ChemistryQ1 What Is the Periodic Table?

The periodic table of chemical elements, often called the periodic table, organizes all discovered chemical elements in rows (called periods) and columns (called groups) according to increasing atomic number. In 1869, Russian chemist Dmitri Mendeleev created the framework that became the modern periodic table, leaving gaps for elements that were yet to be discovered.

“Sulphuric acid” is called the king of acids and “Nitric acid” is called the Queen of acids.

Q2 What are the 3 laws of gas?

Boyle’s Law tells us that the volume of gas increases as the pressure decreases. Charles’ Law tells us that the volume of gas increases as the temperature increases. And Avogadro’s Law tell us that the volume of gas increases as the amount of gas increases.

“Sulphuric acid” is called the king of acids and “Nitric acid” is called the Queen of acids.

Q3 What is a chemical change? Is cooking an egg a chemical change?

There are changes all around us like sugar dissolves in water, the lake freezes in winter etc. Some changes are what scientists call chemical changes and some are not. A chemical change takes place when new substances are made that are different from the substances that we started with.

Yes Cooking eggs, for instance, is an example of a chemical change; the egg white and egg yolk change from liquid to solid. The heat makes the proteins in the egg hardens.

Q4 Which acid is called “Kingly Water” and why?

Aqua Regia is the King’s Water, this is because it is strong enough to dissolve gold – the king of metals. It is prepared by mixing three parts of hydrochloric acid with one part nitric acid but in olden days it is prepared to mix and distill salts. For example, we can mix two parts niter with one part Sal. Ammoniac and distill at a high temperature to form Aqua Regia.

“Sulphuric acid” is called the king of acids and “Nitric acid” is called the Queen of acids.

Q5 What are the main branches of chemistry?

Chemistry is the science that studies atoms and molecules along with their properties. All matter is composed of atoms and molecules. There are 5 main branches of chemistry are

Organic chemistry

Inorganic chemistry

Physical chemistry

Biochemistry

Analytical chemistry

Q6 What is the importance of organic chemistry?

Organic chemistry is simply the study of carbon compounds. Organic chemistry is important because it is life studies and all life-related chemical reactions. Organic chemistry initially involves the study of compounds that could be obtained from living organisms.

Approximately 7 million different organic compounds are known present while there are only 1.5 million known inorganic compounds. This large number of organic compounds arise from the unique property of carbon.

Q7 Which compound is known as “Blue Vitriol”?

Blue vitriol is also known as blue copperas. The word blue vitriol has a strict and definite meaning. It means sulphate of copper with the chemical formula CuSO4.5H2O. The chemical name for blue vitriol is Copper (II) Sulphate Pentahydrate. This salt occurs in the form of rhomboidal prisms of a deep blue colour, having an exceedingly harsh and styptic taste.

Similarly, “Green Vitriol” refers to Ferrous Sulphate.

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Anne Marie Helmenstine, Ph.D.

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Ph.D., Biomedical Sciences, University of Tennessee at Knoxville

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Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels.

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Updated on October 03, 2019

Chemistry is the study of matter and energy and the interactions between them. This is also the definition for physics, by the way. Chemistry and physics are specializations of physical science. Chemistry tends to focus on the properties of substances and the interactions between different types of matter, particularly reactions that involve electrons. Physics tends to focus more on the nuclear part of the atom, as well as the subatomic realm. Really, they are two sides of the same coin.

The formal definition of chemistry is probably what you want to use if you're asked this question on a test. You may also need to practice basic chemistry concepts with a quiz.

Why Study Chemistry?

Because understanding chemistry helps you to understand the world around you. Cooking is chemistry. Everything you can touch or taste or smell is a chemical. When you study chemistry, you come to understand a bit about how things work. Chemistry isn't secret knowledge, useless to anyone but a scientist. It's the explanation for everyday things, like why laundry detergent works better in hot water or how baking soda works or why not all pain relievers work equally well on a headache. If you know some chemistry, you can make educated choices about everyday products that you use.

What Fields of Study Use Chemistry?

You could use chemistry in most fields, but it's commonly seen in the sciences and in medicine. Chemists, physicists, biologists, and engineers study chemistry. Doctors, nurses, dentists, pharmacists, physical therapists, and veterinarians all take chemistry courses. Science teachers study chemistry. Fire fighters and people who make fireworks learn about chemistry. So do truck drivers, plumbers, artists, hairdressers, chefs... the list is extensive.

What Do Chemists Do?

Whatever they want. Some chemists work in a lab, in a research environment, asking questions and testing hypotheses with experiments. Other chemists may work on a computer developing theories or models or predicting reactions. Some chemists do field work. Others contribute advice on chemistry for projects. Some chemists write. Some chemists teach. The career options are extensive.

Where Can I Get Help With a Chemistry Science Fair Project?

There are several sources for help. A good starting point is the Science Fair Index on this website. Another excellent resource is your local library. Also, do a search for a topic that interests you using a search engine, such as Google.

Where Can I Find Out More About Chemistry?

Start with the Chemistry 101 Topic Index or list of Questions Chemistry Students Ask. Check out your local library. Ask people about the chemistry involved in their jobs.

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Helmenstine, Anne Marie, Ph.D. (2023, April 5). What Chemistry Is and What Chemists Do. Retrieved from https://www.thoughtco.com/what-is-chemistry-p2-604135

Helmenstine, Anne Marie, Ph.D. "What Chemistry Is and What Chemists Do." ThoughtCo. https://www.thoughtco.com/what-is-chemistry-p2-604135 (accessed March 12, 2024).

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Elizabeth GordonFurman University

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Learning ObjectivesAlchemy Is in No way Chemistry!Alchemy and the ACS (American Chemical Society)Areas of ChemistryChemists at workSummaryContributors and Attributions

Learning Objectives

To recognize the breadth, depth, and scope of chemistry.

Define chemistry in relation to other sciences.

Identify the main disciplines of chemistry.

Match a scientific project with the correct type of chemist.

Chemistry is the study of matter—what it consists of, what its properties are, and how it changes. Being able to describe the ingredients in a cake and how they change when the cake is baked is called chemistry. Matter is anything that has mass and takes up space—that is, anything that is physically real. Some things are easily identified as matter—this book, for example. Others are not so obvious. Because we move so easily through the air, we sometimes forget that it, too, is matter.

Chemistry is one branch of science. Science is the process by which we learn about the natural universe by observing, testing, and then generating models that explain our observations. Because the physical universe is so vast, there are many different branches of science (Figure \(\PageIndex{1}\)). Thus, chemistry is the study of matter, biology is the study of living things, and geology is the study of rocks and the earth. Mathematics is the language of science, and we will use it to communicate some of the ideas of chemistry.

Figure \(\PageIndex{1}\): The Relationships between Some of the Major Branches of Science. Chemistry lies more or less in the middle, which emphasizes its importance to many branches of science.

Although we divide science into different fields, there is much overlap among them. For example, some biologists and chemists work in both fields so much that their work is called biochemistry. Similarly, geology and chemistry overlap in the field called geochemistry. Figure \(\PageIndex{1}\) shows how many of the individual fields of science are related.

There are many other fields of science, in addition to the ones (biology, medicine, etc.) listed

Alchemy Is in No way Chemistry!

As our understanding of the universe has changed over time, so has the practice of science. Chemistry in its modern form, based on principles that we consider valid today, was developed in the 1600s and 1700s. Before that, the study of matter was known as alchemy and was practiced mainly in China, Arabia, Egypt, and Europe.

Alchemy was a somewhat mystical and secretive approach to learning how to manipulate matter. Practitioners, called alchemists, thought that all matter was composed of different proportions of the four basic elements—fire, water, earth, and air—and believed that if you changed the relative proportions of these elements in a substance, you could change the substance. The long-standing attempts to “transmute” common metals into gold represented one goal of alchemy. Alchemy’s other major goal was to synthesize the philosopher’s stone, a material that could impart long life—even immortality. Alchemists used symbols to represent substances, some of which are shown in the accompanying figure. This was not done to better communicate ideas, as chemists do today, but to maintain the secrecy of alchemical knowledge, keeping others from sharing in it.

The first affinity table. Table of different relations observed in chemistry between different substances; Memoirs of the Royal Academy of Sciences, p. 202-212. Alchemists used symbols like these to represent substances.

In spite of this secrecy, in its time alchemy was respected as a serious, scholarly endeavor. Isaac Newton, the great mathematician and physicist, was also an alchemist.

Alchemy and the ACS (American Chemical Society)

While watching the video below and answer the following questions.

Questions

What was the chief goal of an alchemist according to the video?

What could the philosopher’s stone do to urine?

Is Alchemy a true science?

When urine is boiled down to a white paste, what is the name and symbol for the element that was obtained?

List some properties of this element that were discussed in the video.

Did wealthy people produce more of this element than poorer people?

What types of applications (applied science) did this element lead us to?

Instead of collecting urine, how can one collect higher concentrations of this element?

The video discussed phosphoric acid (formula: H3PO4). Name all the elements in this compound.

What were the mentioned applications of phosphoric acid?

What are some of the organic and biochemical applications of element 13?

Areas of Chemistry

The study of modern chemistry has many branches, but can generally be broken down into five main disciplines, or areas of study:

Physical chemistry: Physical chemistry is the study of macroscopic properties, atomic properties, and phenomena in chemical systems. A physical chemist may study such things as the rates of chemical reactions, the energy transfers that occur in reactions, or the physical structure of materials at the molecular level.

Organic chemistry: Organic chemistry is the study of chemicals containing carbon with hydrogen. Carbon is one of the most abundant elements on Earth and is capable of forming a tremendously vast number of chemicals (over twenty million so far). Most of the chemicals found in all living organisms are based on carbon.

Inorganic chemistry: Inorganic chemistry is the study of chemicals that do not, in general, contain carbon. Inorganic chemicals are commonly found in rocks and minerals. One current important area of inorganic chemistry deals with the design and properties of materials involved in energy and information technology.

Analytical chemistry: Analytical chemistry is the study of the composition of matter. It focuses on separating, identifying, and quantifying chemicals in samples of matter. An analytical chemist may use complex instruments to analyze an unknown material in order to determine its various components.

Biochemistry: Biochemistry is the study of chemical processes that occur in living things. Research may cover basic cellular processes up to understanding disease states so better treatments can be developed.

Figure \(\PageIndex{2}\): (left) Measurement of trace metals using atomic spectroscopy. (right) Measuring hormone concentrations.

In practice, chemical research is often not limited to just one of the five major disciplines. A particular chemist may use biochemistry to isolate a particular chemical found in the human body such as hemoglobin, the oxygen-carrying component of red blood cells. He or she may then proceed to analyze the hemoglobin using methods that would pertain to the areas of physical or analytical chemistry. Many chemists specialize in areas that are combinations of the main disciplines, such as bioorganic chemistry or physical organic chemistry.

Chemists at work

The American Chemical Society (ACS) has designed a series of videos illustrating the different fields that a chemist could pursue. Please watch this 2 minute and 23-second video and answer the questions below:

Which type of chemistry does Dr. Jacobs explore (look at the five types of chemists listed above).

How do Dr. Jacobs and her research associates apply their chemistry to a real-world problem?

What types of professionals does Dr. Jacobs collaborate with?

Which are more difficult to characterize and why: proteins or small molecules?

Summary

Chemistry is the study of matter and the changes it undergoes and considers both macroscopic and microscopic information.

Matter is anything that has mass and occupies space.

The five main disciplines of chemistry are physical chemistry, organic chemistry, Inorganic chemistry, analytical chemistry, and biochemistry.

Many civilizations contributed to the growth of chemistry. A lot of early chemical research focused on practical uses. Basic chemistry theories were developed during the nineteenth century. New materials and batteries are a few of the products of modern chemistry.

Contributors and Attributions

Elizabeth R. Gordon (Furman University)

Hayden Cox (Furman University)

This page titled 1.1: What is Chemistry? is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Elizabeth Gordon.

1: Introduction to Chemistry

1.2: Using the Scientific Method

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ChemistryDealing with reality’s most basic elements, from particles to atoms to molecules, chemistry is also known as the central science.By Matt HamblyFacebook / MetaTwitter / X iconWhatsAppLinkedinRedditEmailMike Kiev/AlamySitting between biology and physics, the field of chemistry is sometimes called the central science. This branch of science deals not with the most basic elements of reality, such as fundamental particles, or the complex world of living organisms, but the in-between world of atoms, molecules and chemical processes.Chemistry is the study of matter, analysing its structure, properties and behaviour to see what happens when they change in chemical reactions. As such, it can be considered a branch of physical science, alongside astronomy, physics and earth sciences including geology.An important area of chemistry is the understanding of atoms and what determines how they react. It turns out reactivity is often largely mediated by the electrons that orbit atoms and the way these are exchanged and shared to create chemical bonds.Chemistry has now split into many branches. For instance, analytical chemists might measure the traces of compounds in ancient pottery to discern what people were eating thousands of years ago.AdvertisementBiochemistry is the study of the chemical processes that take place in living organisms, for instance in farming, and on the effect the resulting produce will have on our body’s metabolism.Organic chemistry, the study of compounds which contain carbon, connects up molecules in new ways to build and analyse an array of materials, from drugs to plastics to flexible electronics. Inorganic chemistry is the study of materials based primarily on elements other than carbon. Inorganic compounds can be pigments, fertilisers, catalysts and more.Physical chemistry involves looking at chemistry through the lens of physics to study changes in pressure, temperatures and rates of conversion, for example, as substances react.Chemists help us understand the nature and properties of the world around us and the history of chemistry is replete with discoveries that have furthered this. Antoine Lavoisier paved the way for modern chemistry. He helped give the field structure by developing an ordered language and symbolism. And his understanding of the constituent parts of air, as well as the process of combustion, disproved centuries of incorrect thinking. But there is perhaps no more important chemist than Dmitri Mendeleev, the Russian who in 1869 wrote down the symbols for all the known chemical elements, arranging them according to their atomic weight. He had created the periodic table, making it possible to predict how any given element would react with another, the compounds it would form and what kind of physical properties it would have.Chemists have subsequently given us treatments for cancer, advanced our understanding of radioactive elements and developed mobile X rays for use in field hospitals – and that’s just Marie Curie. Rosalind Franklin helped us understand that DNA was structured as a double helix, paving the way for the modern revolution in genetic science.More recently, advances in chemistry and biology have contributed to the development of vaccines to the coronavirus, using our knowledge of DNA and RNA to create the first approved messenger RNA vaccines (mRNA). From the development of plastics, and with it nylon, waterproof clothing and even bulletproof vests, to the liquid crystal display you are most likely reading this information on, right through to the complete synthesis of medicines, chemistry’s contributions to modern life are myriad.AdvertisementSign up to our weekly newsletterReceive a weekly dose of discovery in your inbox!

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What is chemistry? Simply put, chemistry is the study of the interactions of matter with other matter and with energy. This seems straightforward enough. However, the definition of chemistry includes a wide range of topics that must be understood to gain a mastery of the topic or even take additional courses in chemistry. In this book, we will lay the foundations of chemistry in a topic-by-topic fashion to provide you with the background you need to successfully understand chemistry.

1.1: Prelude to ChemistryGet ready for a fantastic journey through a world of wonder, delight, and knowledge. One of the themes of this book is "chemistry is everywhere," and indeed it is. You would not be alive if it were not for chemistry, because your body is a big chemical machine. If you do not believe it, do not worry. Every chapter in this book contains examples that will show you how chemistry is, in fact, everywhere. So enjoy the ride, and enjoy chemistry.1.2: Basic DefinitionsChemistry is the study of matter and its interactions with other matter and energy. Matter is anything that has mass and takes up space. Matter can be described in terms of physical properties and chemical properties. Physical properties and chemical properties of matter can change. Matter is composed of elements and compounds. Combinations of different substances are called mixtures. Elements can be described as metals, nonmetals, and semimetals.1.3: Chemistry as a ScienceScience is a process of knowing about the natural universe through observation and experiment. Scientists go through a rigorous process to determine new knowledge about the universe; this process is generally referred to as the scientific method. Science is broken down into various fields, of which chemistry is one. Science, including chemistry, is both qualitative and quantitative.1.E: What Is Chemistry? (Exercises)These are exercises and select solutions to accompany the "Beginning Chemistry" Textmap formulated around the Ball et al. textbook.

This page titled 1: What Is Chemistry? is shared under a CC BY-NC-SA 3.0 license and was authored, remixed, and/or curated by Anonymous via source content that was edited to the style and standards of the LibreTexts platform; a detailed edit history is available upon request.

Preface

1.1: Prelude to Chemistry

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Chemistry - Wikipedia

Chemistry | Definition, Topics, Types, History, & Facts | Britannica

Chemistry - Introduction, Branches, Concepts, History & Facts with Free Resources

What Chemistry Is and What Chemists Do

1.1: What is Chemistry? - Chemistry LibreTexts

What is chemistry? | New Scientist

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1: What Is Chemistry? - Chemistry LibreTexts

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比特派钱包手机版app下载|chemistry

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Chemistry - Wikipedia

Chemistry | Definition, Topics, Types, History, & Facts | Britannica

Chemistry - Introduction, Branches, Concepts, History & Facts with Free Resources

What Chemistry Is and What Chemists Do

1.1: What is Chemistry? - Chemistry LibreTexts

What is chemistry? | New Scientist

Chemistry Definition & Meaning - Merriam-Webster

1: What Is Chemistry? - Chemistry LibreTexts

Concept and branches of chemistry | Britannica

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