Chapter 7 (and 6.3) Review Flashcards
Octet rule exception: _____ have central atom with >8 valence electrons
hypervalent molecules
if no 0 formal charges, then the _____ are the best
smaller non-zero charges
Molecular geometry: 5 ligands, 0 lone pairs
trigonal bipyramidal
bond type when difference in electronegativity is <0.4
pure covalent
Molecular geometry: 5 ligands, 1 lone pair
square pyramidal
Molecular geometry: 4 ligands, 2 lone pairs
square planar
4th quantum number
spin quantum number (ms)
Molecular geometry: 3 ligands, 0 lone pairs
trigonal planar
bond type when difference in electronegativity is >1.8
ionic
Molecular geometry: 2 ligands, 1 lone pair
bent
The 5 Electron Domain Geometries corresponding to 2, 3, 4, 5, and 6 electron groups (ligands and lone pairs)
linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral
Octet rule exception: ____ will have an unpaired electron
odd-electron molecules
Formula for formal charge
v.e. on free atom - # lone pair electrons - (1/2) # bonded electrons
Last two steps for creating Lewis structures
Place on remaining e- on central atom, and then rearrange e- of outer atoms to create multiple bonds and achieve octets for all atoms
Molecular geometry: 2 ligands, 0 lone pairs
linear
bond type when difference in electronegativity is 0.4-1.8
polar covalent
3 components of the electronic structure of an atom
Complete configuration, Orbital diagram, Noble Gas Configuration
Octet rule exception: ______ have <8 electrons around the central atom (usually Be, B, or Al)
Electron-deficient molecules
Molecular geometry: 3 ligands, 2 lone pairs
T-shaped
Molecular geometry: 4 ligands, 1 lone pair
see-saw
3rd quantum number
magnetic quantum number (ml)
it is better to have the more negative formal charges on the more ________ atoms
electronegative
formula for dipole moment
D = qr
q = magnitude of charge
r = distance between charges
distance between atoms in a chem. bond - is determined as the distance at which lowest potential energy is achieved
bond length
