Chapters 8 & 9 Flashcards
4 elements that can have an expanded octet
Sulfur, phosphorus, silicon, and chlorine
linear bond angle & #e⁻ groups
180 & 2
trigonal planar bond angle & #e⁻ groups
120 & 3
tetrahedral bond angle & #e⁻ groups
109.5 & 4
trigonal bipyramidal bond angle & #e⁻ groups
90 from top, 120 from center; 5
octahedral bond angle & #e⁻ groups
90 & 6
name for “middle” atoms & “top/bottom” atoms on tri-bipyr & octa shapes
equatorial & axial
Name & bond angle of - 1 e⁻ group from tri-planar
bent & <120
Name & bond angle of - 1 e⁻ group from tetrahedral
trigonal pyramidal & <109.5
Name & bond angle of - 2 e⁻ groups from tetrahedral
bent & <109.5
Name & bond angle of - 1 e⁻ group from trigonal-bipyramidal
see-saw & <90, <120, <180
Name & bond angle of - 2 e⁻ groups from trigonal-bipyramidal
T-shaped & <90, >180
Name & bond angle of - 3 e⁻ groups from trigonal-bipyramidal
Linear & 180
what types of atoms do e⁻ groups tend to replace
equatorial atoms
Name & bond angle of - 1 e⁻ groups from octahedral
square-pyramidal & <90, >180
Name & bond angle of - 2 e⁻ groups from octahedral
square planar & 90, 180
Name & bond angle of - 3 e⁻ groups from octahedral
T-shaped & <90, >180
Name & bond angle of - 4 e⁻ groups from octahedral
Linear & 180
5 geometries that are always polar
bent, trig-pyramidal, see-saw, T-shape, square pyramid
linear hybridization
sp
trigonal planar hybridization
sp²
tetrahedral hybridization
sp³
trigonal bipyramidal hybridization
dsp³
octahedral hybridization
d²sp³
what does the superscripted number on hybridizations mean
the # of orbitals it superscripts; like p² would mean 2 p orbitals
define sigma bond & symbol
σ; share e⁻ on internuclear axis (in between 2 atoms’ nuclei)
define pi bond
shared e⁻ NOT on internuclear axis; instead above/below it
sigma and pi bonds for each bond multiple
single = 1 σ double = 1 σ & 1 π triple = 1 σ & 2π
what does delocalized resonance bonding mean?
the e⁻ are all around the mol instead of in the bond
how to calculate formal charge of an atom
atom val e⁻ - # atom non-bond e⁻ - # bonds to atom
2 ways to tell the best resonance structure
the best one has the most evenly-distributed formal atom charges & the neg charges are on the most elecneg atom
def lattice E
amt E to separate 1 mol ion comp into gas ions; endothermic rxn
2 ways to compare lattice E
bigger charge on atoms in the ion = bigger LE (like, MgO is better than NaF)
smaller ion itself = bigger LE
how to determine polarity when the element in common between the two comps does NOT have the highest elecneg
1) cancel out that element in common
2) between the other 2 elements, the comp that has the HIGHER elecneg one is the more polar one
how to determine polarity when the element in common between the two comps DOES have the highest elecneg
1) cancel out that element in common
2) between the other 2 elements, the comp that has the LOWER elecneg is the more polar one
octet rule exceptions/facts x 3
Be & B can have less than octet
any atoms n = 3+ can have more than octet
basically only C, N, O, and F work with the rule lmao
