exam 3 Flashcards
ionization energy….
increases as the column increases and decreases as you go down a group
after a full shell, after a half shell
ionization energy drops
the 5th electron taken out creates a huge jump in energy, what group is this element in?
group 14, (C, Si, Ge,….)
Electron affinity
energy change from stealing an electron
(ex flourine EA= -349) only negative for the first electron stolen
electron affinity trend
to the right and up (same full shell half shell trend)
electrostatic potential energy equation
Eel is proportional to (Q1 x Q2)/d
Q= attraction d = distance
delocalized
an electron able to travel 3 or more atoms over from the one it came from
covalent bonds
both elements share electrons evenly due to high ionization energy
lewis symbol
basically lewis struct but just one element
cations = anions = (type of energy)
ionization energy. Electron affinity
larger charges = larger _______
lattice energies
larger distance = ______ lattice energy
smaller
Born-Haber cycle
graph to figure out the lattice energy
think deltaH = deltaH1 +deltaH2 +or -…… -lattice energy. in KJ/Mol
Born-Haber cycle rules
must get to a form that is 1 mole to 1 mol in gaseous state
lattice energy equation
( Q1 x Q2 ) / distance
octet rule exemptions
B, P, S, Se, Br, Te, I
lewis structure rules (6)
- count the number of valence
- adjust for electron charge
- Draw skeleton (central atom with single bonds) (central atom is most electro-positive (Fr is king) and or first)
- distribute leftover electrons to other atoms to fill out octet (most electronegative first)
- place any remaining on the central atom
- if center doesn’t have octet, make double bonds
check for lewis structure
- Complete octets?
- formal charges match?
3.multiple lewis structures? - valence structures?
ionic, polar, nonpolar charge difference
> 1.9, POLAR, <0.4 in electronegativity
dipole moment
Q (charge) x r (distance). greater difference = greater dipole
dipole unit
Debyes (D) or (wierd u)
1 debye =
3.33564 x 10^−30 C·m
Angstroms
unit of length, 10^-10 meters
electron charge
1.60 x 10^-19 C
formal charge
extra electrons that added to the normal valence
formal charges for H2O
H= 0 O=0
charge of _ is perfect, _ is preferable, _ is not correct
0,1,2
if to fill a middle octect with 8 fluorine must become positive _______
this CANNOT happen
when you have multiple lewis structure with same charges possible, choose _______
the more EN element
hypervalence
when in period 3 or lower, to reduce formal charge mid atom can expand the valence
resonance structures
LOOK FOR OXYGENS, equavalent lewis structures that describe a molecule, give ya decimal bond orders
bond order
resonance bonds over amount of bonds (double and single are still one) Plus 1
how to fill out octets
start at the outer and then go inner
Take a moment to memorize vseper models and draw them
oky doky
BOISTERIOUS Boron rules
boron can only have 6 electrons to complete the octet
radical
unpaired electron
S and F compounds
SF2, SF4, SF6
Xe and F compounds
XeF4
higher bond order = ______ angstrums
smaller angstrums, the atoms are closer together
bond enthalpy units and sign
KJ/mol, + (its the energy needed to break the bond)
2 bonds, 0 lone pairs, angle?
linear, 180
3 bonds, 0 lone pairs, angle?
Trigonal Planar, 120
4 bonds, 0 lone pairs, angle?
Tetrahedral, 109.5
5 bonds, 0 lone pairs, angle?
trigonal bipyramidal, 120 and 90
6 bonds, 0 lone pairs, angle?
Octahedral, 90
electron domains
bonds or lone pairs in a compound. (double bonds count as one)
2 bonds, 1 lone pair, angle?
bent or angular, <120
3 bonds, 1 lone pair, angle?
trigonal pyramidal, <109.5
2 bonds, 2 lone pairs, angle?
bent (2) or angular, «109.5
Vsepr acronym
Valence Shell Electron Pairs Repulsion
4 bonds, 1 lone pair, angle?
Seesaw, <120 and <90
3 bonds, 2 lone pairs, angle?
T-shape, <90
2 bonds, 3 lone pairs, angle?
linear, 180
5 bonds, 1 lone pair, angle?
square pyramid, <90
4 bonds, 2 lone pairs, angle?
square planar, 90
3 bonds, 3 lone pairs, angle?
T-shape, <90
2 bonds 4 lone pairs, angle?
linear, 180
practice drawing vsepr models
oky doky
trigonal bipyramidal where 120 and 90?
the equatorial (three atom ring) = 120, axis position (like the poles of a planet) = 90
which take up more space? lone pair or bond
lone pair
(fill in chapter 9 part that you missed)
oki
sigma bond
first bond, on axis bond, head to head overlap,
Pi bond
off axis bond, side to side overlap, like two faces melting together.
Pi bonds live in ____
P orbitals
sigma bonds live in ____
hybridized orbitals
double bond = ___
Pi bond
single bond = _____
sigma bond
triple bond = ____
sigma AND pi bond
Pi bonds prevents _____
ROTATION of a single side of a molecule
bonding orbital
the orbital that goes to a lower energy level and is constructively interferring (-energy)
antibonding orbital
the orbital goes up and destructively interferes with the bond (+ energy denoted with star *)
node
area where you’ll never find an electron. only antibonding orbital has node
bond order calculation
1/2 bonding electrons - antibonding electrons = bond order
hybridization
blending S and P orbitalts
study MOS PI bond structures
oki
diamagnetic (die)
spins of electrons being paired that kill magnetism
paramagnetic
has unpaired electrons that can be lined up to become magnetic
born haber process
the steps to find the lattice energy
a planar molecule
has all of its atoms in the same plane (can ya twist the fucker)
0 unpaired electrons = >0 unparied electrons =
diamagnetic paramagnetic
Angstrom = ?
1x 10^-10 m
delocalized pi bonds have 2 e- per ______ while localized just have _____
p orbital, 2
electron domain vs molecular domain
electron does NOT care about nonbonding pairs. molecular DOES care
