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CHAPTER 1
Remembering General Chemistry: Electronic Structure and Bonding
Important Terms
antibonding molecular
a molecular orbital that results when two atomic orbitals with opposite phases
orbital
interact. Electrons in an antibonding orbital decrease bond strength.
atomic number
the number of protons (or electrons) that a neutral atom has.
atomic mass
the average mass of the atoms in the naturally occurring element.
atomic orbital
an orbital associated with an atom; the three-dimensional area around its nucleus
where electrons are most likely to be found.
aufbau principle
the principle that states that an electron will always go into the available orbital
with the lowest energy.
bond dissociation energy
the amount of energy required to break a bond in a way that allows each of the
atoms to retain one of the bonding electrons; the amount of energy released when
a bond is formed.
bonding molecular orbital
a molecular orbital that results when two atomic orbitals with the same phase
interact. Electrons in a bonding orbital increase bond strength.
bond length
the internuclear distance between two atoms at minimum energy (maximum
stability).
bond order
describes the number of covalent bonds shared by two atoms.
carbanion
a species containing a negatively charged carbon.
carbocation
a species containing a positively charged carbon.
condensed structure
a structure that does not show some (or all) of the covalent bonds.
core electrons
electrons in filled shells.
covalent bond
a bond created as a result of sharing electrons.
degenerate orbitals
orbitals that have the same energy.
dipole
a separation of positive and negative charges.
dipole moment
(
M
)
a measure of the separation of charge in a bond or in a molecule.
double bond
a bond composed of a sigma bond and a pi bond.