Inorganic Chemistry Flashcards
1
Q
Cobalt names and charges
A
Co2+ Cobaltous. Cobalt II
Co3+. Cobaltic. Cobalt III
2
Q
Iron charges and names
A
Fe2+, Ferrous iron II
Fe3+ ferric iron III
4
Q
Mass number
A
A number of protons and neutrons
6
Q
Atomic number
A
Z
Number of protons in the nuc
7
Q
Sulfate
A
2-
SO4
8
Q
carbonate
A
2-
CO3
9
Q
Perchlorate
A
1-
ClO4
10
Q
bicarbonate
A
-1
HCO3
11
Q
Chlorate
A
1-
ClO3
12
Q
peroxide
A
2-
O2
13
Q
phosphate
A
3-
PO4
14
Q
permanganate
A
1-
Mn04
15
Q
Hypochlorite
A
-1
ClO
16
Q
Nitrate
A
-1
NO3
17
Q
Idea Gas Law
A
PV=nRT R=.082
18
Q
Idea Gas Law Proportionality
A
opposite sides are directly proportional; same side is inversely proportional
19
Q
Law of Partial Pressures
A
Ptotal=P1+P2+P3….
20
Q
Gas collected over water (wet)
A
must subtract the vapor pressure of water from the total gas pressure
21
Q
Molar Volume
A
at STP one mole of a gas would occupy a volume of 22.4 L. (1mol=22.4L at STP)
22
Q
Kinetic Molecular Model
A
- gaseous molecules are widely dispersed
2 gas molecules travel in random straight motion - avg KE is directly proportional to abs T of the gas.
4Collisions of molecules are ellastic (no momentum loss) - collisions due to the molecules and walls of container
- do not attract each other
- volume occupied by molecule negligible to V of the container.
23
Q
Electronegativity (EN) and periodic trend
A
capacity of molecule to attract bonded electrons
Increases across; decreases down
24
Q
EN and bond values
A
<.5 non- Polar
.5-1.9 polar covalent
1.9+ Ionic
25
Q
Hydrogen bonding
A
very strong dipole bonds that invole a polar molecule conainting an H bonded to F, O, N`
26
Q
Relattive Strenghs of intermolecular forced
A
Ion-Ion> H-Bonds> dipole-dipole> london (van der waals)
27
BP, MP and Intermolecular attractions
non-polar: larger molecules increase BP/MP
polar: smaller size increase BP+MP
STABILITY DOES NOT AFFECT BP/MP
28
Density
d=m/v
29
Specific Gravity
SGx=dx/dwater
When H20 is liquid; SG=d. SG>1 sink in h20 SG<1 float
30
Molarity
M= mol/V (L)
31
Percent by Mass
%(w/w)= (m sol x100)/(m soln)
32
Percent by Mass/volume
%(w/V)= (m sol (g) *100)/(V soln (mL))
33
Molality
m= (mol sol/ mass solv in Kg)
34
Mole Fraction
Xi= (mol of i)/ (total mol)X
35
Colligative property (pressure)
dissolving non volatile solvent into volative solution decreases pressure lower than pressure of original soln
P = Xsol * Po
36
Colligative property (boiling point) `
Dissolving nonvolatile solvent into volatile solution increases BP
deltaTb= Kb * m
37
Colligative property (freezing point)
dissolving a solute in a solvent lowers FP
deltaTf=Kf * m
38
Greatest Colligative Effect Problems
soln with the largest solute concetration yields the greatest effect (lowest VP, higest BP, lowest FP, or largest osmotic pressure)
[Ionic solutes]>[non-ionic]
39
common weak strong electrolytes
1. water soluable strong acids (HCl, HNO3, H2SO4)
2. water soluable strong bases (NaOH, KOH)
3. Walter soluble salts (NaCl, KNO3, K2SO4, NH4Cl)
40
common weak electrolytes
1. water soluble weak acids (CH3COOH)
| 2. water soluable weak bases (NH3)
41
common non-electrolytes
1. sugars like glucose and sucrose
| 2 alcohols like methanol and ethanol
42
dilutions
adding more solvent to a soln doesnt change solute present
Mi x Vi= Mf x Vf and %i * Vi= %f * Vf
43
Acid Properties
Taste sour
turns litmus red
leaves phenolphthalein colorless
pH below 7
44
Basic Properties
Taste bitter; feel slippery
turns litmus blue
turns phenolphthalein pink
ph greater than 7
45
arrhenius acid/base
Acid generates Hydronium ion and base generates hydroxide ions
46
bronsted lowry acid/base
acid is a proton donor
| base if a proton acceptor
47
Lewis Definition
Acid is electron pair acceptor
| base is electron pair donator
48
Common strong acids
HCL, HNO3, H2SO4, HCLO4
49
Common weak acids
CH3COOH, HF, H2CO3, H3PO4
50
common strong bases
metal hydroxide salts typically strong bases
51
weak bases
NH3
52
Cojugate base ions
Conjugate base of a weak acid is a weak base
conjugate base of a strong acid is not a base.
53
pH and pOH
pH=-log[H+] pOH=-log[OH-]
[H+]=in log(-pH) and {OH-]=in log(-pOH)
Kw=[H+}[OH-}=1x10^-14
54
buffer
combination of a weak acid and a weak base that resists changes in pH
55
Acid/Base SToichiometry formula
nA x MA x VA = nB x MB x VB
n is the capacity to donate/accept protons
HCL=1 H2SO4=2
NAOH=1 CA(OH)2=2
56
Energy Units
SH H20= 1 cal= 4.18 J
57
heat equation (no change in state)
q=mass x SH x deltaT
58
Entropy (dS)
disorder increased dS is +; rxn spontaneous
| disorder decreased dS is -; rnx non-spon
59
Enthalpy (dH)
evolves heat, exothermic, - , spontaneous
absorbs heat, endothermic, +, non-spon
60
Gibb's Free Energy (dS)
energy is produced, -, spontaneous
energy is consumed, +, non-spon
zero, nil, at EQ.
61
quantum numbers
1st: shell (n)
2nd: subshell (l)
3rd orbital (ml)
4th spin (ms)
62
pauli eclusion principle
no two electrons in the same atom can have the same set of 4 quantum numbers
63
hund's rule
electrons in the same subshell occupy availible orbitals singly, before paring up
64
aufbau principle
electrons occupy the loweste energy orbitals available
65
coordinate covalent bonds
one atom donates both shared electrons in a bond (lewis acid/base rxn_
66
charles law
as T increases V increases
67
Hig temp/ low pressure (states)
gas> liquid> solid
68
Low temperative/ high pressure (states
solid>liquid>gas
69
When do gases deviate from idea behavior
high pressure and low temperature
70
Keq values
Keq>>1 P favored over R
Keq = 1 neither R or P favored
Keq<<<1 R favored over P
71
Le Chatlelier's Principle
a system at equilibrium is subjected to stress, eq shifts in a direction that alleviates stress
72
Teperatiure and eq
if heat is a product; incr temperature shifts to reactants and vice versa
73
Generally soluable ions
alkali and ammonium compounds
acetates, chlorates, nitrates, and perchlorates
Pb Hg and Ag salts when pared with above anions
74
Insoluble ions
Pb Hg and Ag unless paired with soluable anions!
75
van't Hoff factor (i)
```
binary salt (NaCl)= 2
CaCl2= 3
solvation species= 1
```
76
Ka/Kb and acid/base strength
large values imply strong
| small values imply weak
77
Reduction table reduced/ oxidized species
Most easily reduced species bottom left; least easily top left
most easily oxidiezed at top right; least easily oxidied at bottom right.
78
Galvanic Cell
= redox rxn spontaneous
- creates electron flow
- oxidation at anode
- reduction at cathode
- cathode is +
- anode is -
- electrons flow from anode to cathode
79
electrolytic cell
- rxn nonspontaneous
- requires electron flow
- anode is +
- cathode is -
80
B- decay
decreases number of neutrons
increases number of protons
adds 1 to atomic number
.
81
B+ (positron) decay
Increases number of neutrons
decreases number of protons
subtracts one from atomic number
82
alpha decay
decreaes number of nutetrons and protons by 2 each
subtracts 4 from mass number and 2 from atomic
83
half life formula
N=N0 (1/2)^t/t1/2
