UNIT THREE Flashcards
covalent bond
electron pairs shared between atoms, form molecular compounds
iconic bond
electron pairs shared unequally between atoms, form ionic compounds
metallic bond
results from attraction between metal atoms and surrounding electrons
cation
positively charged ion
anion
negatively charged ion
nonpolar-covalent bond
covalent bond where bonding electrons are shared equally by bonded atoms
polar-covalent bond
covalent bond where bonded electrons have unequal attraction for the shared electrons
octet rule
chemical compounds form to have 8 electrons in the highest occupied energy level
electron-dot notation
shows only valence electrons around atomic symbol
Lewis dot structure
uses electron-dot notation to represent compounds
resonance structures
multiple structures that can represent the bonding in a single compound
polyatomic ions
charged groups of two or more covalent bonded atoms
oxoanion
polyatomic ion that contains oxygen
acids
release H+ when dissolved in water
VSEPR
“valence-shell, electron-pair repulsion”
repulsion between valence electrons causes them to be oriented as far as possible
intermolecular forces
forces of attraction between molecules
dipole
created by equal but opposite charges separated by a short distance
dipole-dipole forces
forces of attraction between polar molecules
percent composition
percent by mass of each element in a compound
molecular formula
exact number and type of atom present in one molecule of a compound
empirical formula
simplest whole number ratio of elements in a compound
AB3
trigonal planar
AB2E
bent/v-shaped
AB4
tetrahedral
AB3E
trigonal pyramid
AB2E2
bent/v-shaped
AB5
trigonal bipyramidal
AB6
octahedral
AB2
linear
