Final Exam Flashcards
electron geometries
2 domains: linear 3 domains: trigonal planar 4 domains: tetrahedral 5 domains: trigonal bipyramidal 6 domains: octahedral
linear molecular geometry
2 situations-both 180 degrees
- 2 bonding groups, 0 lone pairs, nonpolar
- 2 bonding groups, 3 lone pairs, polar
trigonal planar molecular geometry(pairs, angle and polarity)
3 bonding pairs, 0 lone pairs, 120 degrees, nonpolar
bent molecular geometry(pairs, angle and polarity)
2 situations
- 2 bonded pairs, 1 lone pair, <120 degrees, polar
- 2 bonded pairs, 2 lone pairs, «109.5 degrees, polar
tetrahedral molecular geometry(pairs, angle and polarity)
4 bonded pairs, 0 lone pairs, 109.5 degrees, nonpolar
trigonal pyramidal molecular geometry(pairs, angle and polarity)
3 bonding pairs, 1 lone pair, <109.5 degrees, polar
trigonal bipyramidal molecular geometry(pairs, angle and polarity)
5 bonded pairs, 0 lone pairs, 120 degrees for equitorial bonds, 90 degrees for axial bonds, nonpolar
seesaw molecular geometry(pairs, angle and polarity)
4 bonded pairs, 1 lone pair, <120 degrees for equitorial, <109.5 degrees for axial bonds, polar
T-shaped molecular geometry(pairs, angle and polarity)
3 bonding pairs, 2 lone pairs, <90 degrees, polar
octahedral molecular geometry(pairs, angle and polarity)
6 bonding pairs, 0 lone pairs, 90 degres, nonpolar
square pyramidal molecular geometry(pairs, angle and polarity)
5 bonding pairs, 1 lone pair, <90 degrees, polar
square planar molecular geometry(pairs, angle and polarity)
4 bonding pairs, 2 lone pairs, 90 degrees, NONpolar
principle quantum number
n, defines energy levels
angular momentum quantum number
l, defines subshells, ranges from 0 to n-1 0=s 1=p 2=d 3=f 4=g
magnetic quantum number
ml, ranges from -l to l
spin quantum number
ms, value of + or - 1/2,
ionization energy trend+equation
increases going up and to the right
X(g) = X^+(g) + e-
effective nuclear charge definition+trend
increases going up and to the right
the charge an electron experiences from being attracted to the nucleus and from being repelled by other electrons
electron affinity definition+equation+trend
energy change that occurs when an electron is added to a gaseous atom
X(g)+e- = X-(g)
Cl- has most electron affinity, halogens(17) have highest of all columns, then column 16 then column 1. Column 2 has 0 or almost 0 electron affinity.
absorbing vs emitting energy
Absorption: increase n
Emission: decrease n
ion dipole interaction
ions and polar solvents
dipole dipole interactions
two polar molecules being attracted to each other
H bond
H bonded to F, N or O
lattice energy/enthalpy including reaction
🔼Hlattice, always negative, M+(g) + X-(g) = MX(s) whem neagtive, opposite if positive
🔼Hhydration
enthalpy change that occurds when gases are dissolved in water
M+(g) + X-(g) = M+(aq) + X-(aq)
**charges can differ
🔼Hsolution equation with lattice energy and enthalpy of hydration
🔼Hsolution=🔼Hhydration + 🔼Hlattice
🔼Hsolution is much smalle rin magnitude than 🔼Hhydration and 🔼Hlattice
🔼Hlattice trend
increases as charge difference increases, decreases as atomic radius increases
🔼Hhydratiobn trends
inverse relationship with atomic radius
difference between voltaic and electrolytic cell
not spontaneous, takes energy from surroundings, negatively charged cathode and postively charged anode
corrosion
a sacrificial anode with a lower reduction potential can be in contact with what is being corroded, and the corroding substance will become the cathode and no longer corrode
ionic compound properties
- hard
- brittle
- high boiling/melting points
- conduct electricity when dissolved in water
properties of covalent compounds
- low melting/boiling points
- brittle
- poor conductors of heat and electricity evenw hen dissolved in water