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Chapter 1
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electronegative
describes an element that readily acquires an electron.
electronegativity
the tendency of an atom to pull electrons toward itself.
electrostatic attraction
an attractive force between opposite charges.
electrostatic potential map
a map that shows how electrons are distributed in a molecule.
(potential map)
equilibrium constant
the ratio of products to reactants at equilibrium.
excited-state electronic
the electronic configuration that results when an electron in the ground state has
configuration
moved to a higher-energy orbital.
formal charge
the number of valence electrons
-
(the number of nonbonding electrons
+
the
number of bonds).
free radical (radical)
a species with an unpaired electron.
ground-state electronic
a description of the orbitals the electrons of an atom occupy when they are all in
configuration
their lowest available energy orbitals.
Heisenberg uncertainty
a principle that states that both the precise location and the momentum of an
principle
atomic particle cannot be simultaneously determined.
Hund’s rule
a rule that states that when there are degenerate orbitals, an electron will occupy an
empty orbital before it will pair up with another electron.
hybrid orbital
an orbital formed by hybridizing (mixing) atomic orbitals.
hydride ion
a negatively charged hydrogen (a hydrogen atom with an extra electron).
hydrogen ion (proton)
a positively charged hydrogen (a hydrogen atom without its electron).
ionic compound
a compound composed of a positive ion and a negative ion held together by
electrostatic attraction.
ionization energy
the energy required to remove an electron from an atom.
isotopes
atoms with the same number of protons but a different number of neutrons.
Kekulé structure
a model that represents the bonds between atoms as lines.
Lewis structure
a model that represents the bonds between atoms as lines or dots and the lone-pair
electrons as dots.
lone-pair electrons
valence electrons not used in bonding.
(nonbonding electrons)