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Atom
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Atom

For alternative meanings see atom (disambiguation).

Atom

The electrons move rapidly around the nucleus.
Classification
Smallest division of a chemical element

Properties
Mass: atomic mass
Electric Charge: 0 C
Diameter: 10pm to 100pm

An atom is the smallest portion into which a chemical element can be divided while still retaining its chemical properties. Atoms are the basic constituents of molecules and ordinary matter. Atoms are composed of subatomic particles.

Table of contents
1 Atomic theory
2 Structure
3 Models of the atom
4 Etymology
5 See also
6 External link

Atomic theory

Main article: Atomic theory

The atomic theory is a theory of the nature of matter. It states that all matter is composed of atoms.

Structure

Atoms are composed mostly of empty space, but also of smaller subatomic particles. At the center of the atom is a tiny positive nucleus composed of nucleons (protons and neutrons). The rest of the atom contains only the fairly flexible electron shells. Usually atoms are electrically neutral with as many electrons as protons.

Atoms are generally classified by their atomic number, which corresponds to the number of protons in the atom. For example, carbon atoms are those atoms containing 6 protons. All atoms with the same atomic number share a wide variety of physical properties and exhibit the same chemical behavior. The various kinds of atoms are listed in the Periodic table. Atoms having the same atomic number, but different atomic masses (due to their different numbers of neutrons), are called isotopes.

The simplest atom is the hydrogen atom, having atomic number 1 and consisting of one proton and one electron. It has been the subject of much interest in science, particularly in the early development of quantum theory.

The chemical behavior of atoms is largely due to interactions between the electrons. In particular the electrons in the outermost shell, called the valence electrons, have the greatest influence on chemical behavior. Core electrons (those not in the outer shell) play a role, but it is usually in terms of a secondary effect due to screening of the positive charge in the atomic nucleus.

There is a strong tendency for atoms to completely fill (or empty) the outer electron shell, which in hydrogen and helium has space for two electrons, and in all other atoms has space for eight. This is achieved either by sharing electrons with neighboring atoms or by completely removing electrons from other atoms. When electrons are shared a covalent bond is formed between the two atoms. Covalent bonds are the strongest type of atomic bond.

When one or more electrons are completely removed from one atom by another, ions are formed. Ions are atoms that possess a net charge due to an imbalance in the number of protons and electrons. The ion that stole the electron(s) is called an anion and is negatively charged. The atom that lost the electron(s) is called a cation and is positively charged. Cations and anions are attracted to each other due to coulombic forces between the positive and negative charges. This attraction is called ionic bonding and is weaker than covalent bonding.

As mentioned above covalent bonding implies a state in which electrons are shared equally between atoms, while ionic bonding implies that the electrons are completely confined to the anion. Except for a limited number of extreme cases, neither of these pictures is completely accurate. In most cases of covalent bonding, the electron is unequally shared, spending more time around the more electronegative atom, resulting in the covalent bond having some ionic character. Similarly, in ionic bonding the electrons often spend a small fraction of time around the more electropositive atom, resulting in some covalent character for the ionic bond.

Models of the atom

Etymology

The word atom is derived from the
Greek atomos, indivisible, from a-, not, and tomos, a cut.

See also

External link

Particles in Physics - Composite particles Edit
Molecules | Atoms | Atomic nuclei | Hadrons | Baryons | Mesons | Exotic baryons | Exotic mesons | Tetraquarks | Pentaquarks