ionic
bond type between a metal (cation) and a nonmetal (anion) / transfer of electrons
polar covalent
type of bond between two nonmetals / shares electrons unequally (EN diff. of 0.3 or less)
nonpolar covalent
type of bond between two nonmetals / shares electrons equally (EN diff. equal or more than 0.4)
metallic
bond type between two metals / electrons not associated, travel freely, “electron sea”, DELOCALIZED
single bond
weakest / longest bond / fewest shared electrons
triple bond
strongest / shortest bond / most shared electrons
alloy
combining two or more metals
substitutional alloy
atoms have similar radii / one atom substitutes for another atom in the lattice
interstitiual alloy
super obvious difference in radii / smaller atoms fill up the space in the larger atoms
resonance
mobile bonds when multiple structures are identical
formal charge
hypothetical charge used to predict the most dominant or accurate lewis structure / VE - lines - dots = FC
VSEPR theory
valence shell electron pair repulsion / like charges repel / bonds and lone pairs will arrange themselves in order to minimize repulsion
bond hybridization
it is possible for orbitals to morph into new hybrid orbitals to allow for the maximum amount of bonds
electrostatic force
positive cations are attracted to negative anions