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chemical bond
strong attractive forces which hold atoms together
ionic bonding
bonding that results in the transfer of one or more atoms to another
covalent bonding
bonding that results from the sharing of one or more electron pairs by two atoms
metallic bonding
bonding that results from attraction of positively charged metal ions for mobile electrons that are delocalized throughout the metallic crystal
lattice enthalpy
the energy necessary to separate the ions of an ionic solid into isolated gas phase ions
octet rule
States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons
Lewis Dot Structure
diagram of a molecule using dots to represent valence electrons
double bond
A chemical bond formed when atoms share two pairs of electrons
triple bond
A chemical bond formed when atoms share three pairs of electrons
incomplete octet
These elements are stable with fewer than eight electrons in their valence shell and include hydrogen (2), helium (2), lithium (2), beryllium (4), and boron (6).
expanded octet
when a molecule has more than 8 electrons around the central atom
odd electron species
molecules or ions with an odd number of electrons
Electron negativity
measure of the ability of an atom in a molecule to attract bonding electrons to itself
dipole moment
measure of the degree of charge separation in a bond of in a molecule
formal charge
the hypothetical charge that an atom in a molecule acquires when the bonding electrons are assumed to be shared equally between the atoms
Resonance
the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure
delocalized bonding
a type of bonding in which a bonding pair of electrons is spread over a number of atoms rather than localized between two
bond length
the average distance between the nuclei of two bonded atoms
bond energy
the energy required to break a chemical bond and form neutral isolated atoms
bond order
the number of shared electron pairs between two atoms
decreases
as bond order increases, bond length ____ (inverse relationship)
increases
as bond order increases, bond energy _____ (direct relationship)
