Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
28 Cards in this Set
- Front
- Back
|
A measure of atomic mass; one-twelfth of the mass of an atom of C12.
|
atomic mass unit (amu).
|
|
|
For a chemical element, the number of protons within the atomic nucleus.
|
atomic number (Z).
|
|
|
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.
|
atomic weight (A).
|
|
|
An early atomic model in which electrons are assumed to revolve around the nucleus in discrete orbitals.
|
Bohr atomic model.
|
|
|
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.
|
bonding energy.
|
|
|
A force between charged particles such as ions; the force is attractive when the particles are of opposite charge.
|
coulombic force.
|
|
|
A primary interatomic bond that is formed by the sharing of electrons between neighboring atoms.
|
covalent bond.
|
|
|
A pair of equal yet opposite electrical charges that are separated by a small distance.
|
dipole (electric).
|
|
|
For an atom, the manner in which possible electron states are filled with electrons.
|
electron configuration.
|
|
|
For an atom, having a tendency to accept valence electrons. Also, a term used to describe nonmetallic elements.
|
electronegative.
|
|
|
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.
|
electron state (level).
|
|
|
For an atom, having a tendency to release valence electrons. Also, a term used to describe metallic elements.
|
electropositive.
|
|
|
A normally filled electron energy state from which an electron excitation may occur.
|
ground state.
|
|
|
A strong secondary interatomic bond that exists between a bound hydrogen atom (its
unscreened proton) and the electrons of adjacent atoms. |
hydrogen bond.
|
|
|
A coulombic interatomic bond that exists between two adjacent and oppositely charged ions.
|
ionic bond.
|
|
|
Atoms of the same element that have different atomic masses.
|
isotopes.
|
|
|
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.
|
metallic bond.
|
|
|
The quantity of a substance corresponding to 6.022 _ 1023 atoms or molecules.
|
mole.
|
|
|
The postulate that for an individual atom, at most two electrons, which necessarily have opposite spins, can occupy the same state.
|
Pauli exclusion principle.
|
|
|
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.
|
periodic table.
|
|
|
A molecule in which there exists a permanent electric dipole moment by virtue of
the asymmetrical distribution of positively and negatively charged regions. |
polar molecule.
|
|
|
Interatomic bonds that are relatively strong and for which bonding energies are relatively
large. Primary bonding types are ionic, covalent, and metallic |
primary bonds.
|
|
|
A branch of physics that deals with atomic and subatomic systems; it allows only
discrete values of energy that are separated from one another. By contrast, for classical mechanics, continuous energy values are permissible. |
quantum mechanics.
|
|
|
A set of four numbers, the values of which are used to label possible electron states. Three of the quantum numbers are integers, which also specify the size, shape, and spatial orientation
of an electron’s probability density; the fourth number designates spin orientation. |
quantum numbers.
|
|
|
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. |
secondary bonds.
|
|
|
The electrons in the outermost occupied electron shell, which participate in interatomic bonding.
|
valence electrons
|
|
|
A secondary interatomic bond between adjacent molecular dipoles that may be permanent
or induced. |
van der Waals bond.
|
|
|
An atomic model in which electrons are treated as being wavelike.
|
wave-mechanical model.
|
