Studied by 1 person
resonance
situation in which one Lewis structure is
insufficient to describe the bonding in a
molecule and the average of multiple
structures is observed
ideal gas
hypothetical gas whose physical properties
are perfectly described by the gas laws
valence bond theory
model that describes the changes in the atomic
orbitals of an atom when it forms a covalent
compound
Dalton’s law of partial
pressures
total pressure of a mixture of ideal gases is
equal to the sum of the partial pressures of the
component gases
pi bond (π pi)
bond formed by side-by-side overlap of
atomic orbitals, in which the electron density
is found on opposite sides of the internuclear
axis
diffusion
movement of an atom or molecule from a
region of relatively high concentration to one
of relatively low concentration
hybridization
description of bonding that involves atomic
orbitals overlapping to form σ or π bonds,
within which pairs of electrons are shared
valence shell electron-pair
repulsion theory (VSEPR
theory used to predict the bond angles in a
molecule based on positioning regions of high
electron density as far apart as possible to
minimize electrostatic repulsion
hypervalent molecule
molecule containing at least one main group
element that has more than eight electrons in
its valence shell
covalent bond
bond formed when electrons are shared
between atoms
Lewis symbol
symbol for an element or monatomic ion that
uses a dot to represent each valence electron
in the element or ion
hybrid orbital
orbital created by combining atomic orbitals
on a central atom
formal charge
charge that would result on an atom by taking
the number of valence electrons on the neutral
atom and subtracting the nonbonding
electrons and the number of bonds
ideal gas law
relation between the pressure, volume,
amount, and temperature of a gas under
conditions derived by combination of the
simple gas laws
effusion
transfer of gaseous atoms or molecules from a
container to a vacuum through very small
openings
ionization energy
energy required to remove an electron from a
gaseous atom or ion
sigma bond (σ bond)
covalent bond formed by overlap of atomic
orbitals along the internuclear axis
electron-pair geometry
arrangement around a central atom of all
regions of electron density (bonds, lone pairs,
or unpaired electrons)
electromagnetic radiation
energy transmitted by waves that have an
electric-field component and a magnetic-field
component
ionic bond
strong electrostatic force of attraction between
cations and anions in an ionic compound
