Ions
A positively charged ion
Bond that forms between atoms that vary greatly in electronegativity
ionic
The most electronegative element is _ with a value of _
fluorine, 4.0
VSEPR stands for:
valence shell electron pair repulsion
Force of attraction between molecules
intermolecular forces
Energy required to remove 1 electron from an atom of an element
ionization energy
Chemical bond resulting from sharing of electrons
covalent bond
Elements most likely involved in multiple bonds
C, N, O
VSEPR theory is based on the idea that:
Opposite charges separated by a short distance
dipole
Energy change when electrons are acquired by a neutral atom
electron affinity
Group of covalently bonded atoms
molecule
Charged group of covalently bonded atoms
polyatomic ion
Short hand description(s) for bent geometry
AB2E, AB2E2
hydrogen bonding
Elements on the right side of the periodic table tend to form _ because they have a _ electron affinity.
anions, large negative
Lewis structures
If electrons are not shared equally among atoms this type of bond forms
polar covalent
AB3E indicates this type of geometry
triangular pyramidal
dipole - induced dipole
Central atom of a Lewis structure should be the most
electropositive
A link between atoms due to electrons being lost, gained, or shared
chemical bond
5 atoms of fluorine bonded to 1 sulfur would have this geometry
triangular bipyramidal
Would Krypton or Argon have a stronger bond between their like atoms? Why? What type of bond is it?
Krypton, more electrons to induce dipoles, London Dispersion Forces