exam 3 review section Flashcards
effective nuclear charge
basically you have screens (the noble gas config) and your outer valence.
Zeff =?
Z-S
bonding atomic radius
trends smaller to the right and larger down
Cation ____ anion ____
small big
we lose highest ____ value electrons first
n (think p an s block before D)
ionization energy trend (endothermic)
how hard it is to steal your electron. up and right = highest. halfway through p more than p4 and same for s
electron affinity is
how much you want to steal electrons. 1st is exo, second and third is endo
lattice energy
how much energy it take to turn a solid salt into gaseous ions (always endothermic).
coulumbs law
Q1Q2/d
lattice energy increases when and decreases when
charge increases, distance decreases
dipole moment
charge times radius or Q times r basically distance makes the dipole increase
polarity
eletronegativity difference
formal charge
valence electrons - (1/2bonding electrons + a;; non-bonding)
hypervalent
going past 8 valence electrons (10 or 12) only happen in n=3 and beyond
memorize vseper graph
oky doky
lone pairs ____ other angles
decompress (<) (less electron density
double and triple bonds ____ other angles
compress (>) (more electron density
to be polar, you must have ____ and not be _____
polar bonds, symmetrical. symmetry kills polarity
valence bond theory
sigma bonds live in hybrids. H’s have s.
study hybridization
oki
bonding orbital
constructive, bottom
antibonding orbitals
deconstructive, top, gives us nodal planes
study molecular orbitals
oki
memorize molecular charts for energy levels
oki
