Chp. 2 Vocab

A measure of atomic mass; 1/12 of the mass of an atom of C12.

For a chemical element, the number of protons within the atomic nucleus.

The weighted average of the atomic masses of an atom’s naturally occurring isotopes. It may be expressed in terms of atomic mass units (on an atomic basis), or the mass per mole of atoms.

An early atomic model in which electrons are assumed to revolve around the nucleus in discrete orbitals.

The energy required to separate two atoms that are chemically bonded to each other. It may be expressed on a per-atom basis or per mole of atoms.

A force between charged particles such as ions; the force is attractive when the particles are of opposite charge.

A primary interatomic bond that is formed by the sharing of electrons between neighboring atoms.

For an atom, the manner in which possible electron states are filled with electrons.

For an atom, having a tendency to ACEPT valence electrons. Also used to describe nonmetallic elements.

One of a set of discrete, quantized energies that are allowed for electrons. In the atomic case, each state is specified by four quantum numbers.

For an atom, having a tendency to RELEASE valence electrons. Also used to describe metallic elements.

A normally filled electron energy state from which an electron excitation may occur.

A strong secondary interatomic bond that exists between a bound hydrogen atom (its unscreened proton) and the electrons of adjacent atoms.

A coulombic interatomic bond that exists between two adjacent and oppositely charged ions.

Atoms of the same element that have different atomic masses.

A primary interatomic bond involving the nondirectional sharing of nonlocalized valence electrons (“sea of electrons”) that are mutually shared by all the atoms in the metallic solid.

The quantity of a substance corresponding to 6.022x10^23 atoms or molecules.

For an individual atom, at most two electrons, which necessarily have opposite spins, can occupy the same state.

The arrangement of the chemical elements with increasing atomic number according to the periodic variation in electron structure. Nonmetallic elements are positioned at the far right-hand side of the table.

A molecule in which there exists a permanent electric dipole moment by virtue of the asymmetrical distribution of positively and negatively charged regions.

Interatomic bonds that are relatively strong and for which bonding energies are relatively large. Primary bonding types are ionic, covalent, and metallic.

. A branch of physics that deals with atomic and subatomic systems; it allows only discrete values of energy. By contrast, for classical mechanics, continuous energy values are permissible.

A set of four numbers, the values of which are used to label possible electron states. Three of the quantum numbers are integers that specify the size, shape, and spatial orientation of an electron’s probability density; the fourth number designates spin orientation.

Interatomic and intermolecular bonds that are relatively weak and for which bonding energies are relatively small. Normally, atomic or molecular dipoles are involved. Examples of secondary bonding types are van der Waals forces and hydrogen bonding.