unit 2 vocab Flashcards
polar covalent
bonds where electrons are not equally shared
semimetal
metallic bonds where the electrons are more tightly held
dipole arrow
points towards the more electronegative atom
nonbonding atomic radius
distance between centers of adjacent atoms in direct contact but not bonded with eachother
electron groups
general term for lone pairs, bonds, or lone electrons in a molecule
covalent electronegativity
0 - < 0.5 change in EN
polar covalent electronegativity
0.5 - <1.7 change in EN
ionic electronegativity
1.7 + change in EN
electron affinity
how easily an atom will accept an electron
dipole moment
measure of the separation of positive and negative charges in a molecule
percent ionic character
ratio of an atom’s actual dipole moment compared to the dipole moment it’d have if the electron completely transferred, x 100%
debeye (D)
unit used to report dipole moments
resonance structure
two or more valid lewis structures that ae shown with double-headed arrows to indicate the actual structure is intermediate between them
formal charge
the charge an atom in a lewis structure would have if all the bonding electrons were shared equally between the bonded atoms
resonance hybrid
the actual structure of an atom that’s intermediate between two or more resonance structures
free radical
molecular ion with an odd number of electrons in its lewis structure
alloy
beneficial mixture of metals
primary metal
main part of an alloy
impurity
additional part in an alloy
interstitial alloy
atoms of impurity fit between the gaps of the primary metal
substitutional alloy
atoms of impurity replace some of the primary metal
chemical bonds
attraction between the molecules o fone atom and the electron(s) of another
lattice energy
energy required to separate ions in an ionic bond
bond energy
the energy required to break a mol of the bonds in a gaseous state.
electron geometry
the geometrical arrangement of electron groups
molecular geometry
the geometrical arrangement of the atoms in a molecule
hybridization
a mathematical procedure that combines standard atomic orbitals to make hybrid orbitals to better reflect the actual electron distribution
antibonding orbital
a molecular orbital that’s higher in energy than any o the atomic orbitals from which it was formed