Inorganic Chemistry Flashcards
Cobalt names and charges
Co2+ Cobaltous. Cobalt II
Co3+. Cobaltic. Cobalt III
Iron charges and names
Fe2+, Ferrous iron II
Fe3+ ferric iron III
Mass number
A number of protons and neutrons
Atomic number
Z
Number of protons in the nuc
Sulfate
2-
SO4
carbonate
2-
CO3
Perchlorate
1-
ClO4
bicarbonate
-1
HCO3
Chlorate
1-
ClO3
peroxide
2-
O2
phosphate
3-
PO4
permanganate
1-
Mn04
Hypochlorite
-1
ClO
Nitrate
-1
NO3
Idea Gas Law
PV=nRT R=.082
Idea Gas Law Proportionality
opposite sides are directly proportional; same side is inversely proportional
Law of Partial Pressures
Ptotal=P1+P2+P3….
Gas collected over water (wet)
must subtract the vapor pressure of water from the total gas pressure
Molar Volume
at STP one mole of a gas would occupy a volume of 22.4 L. (1mol=22.4L at STP)
Kinetic Molecular Model
- 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.
Electronegativity (EN) and periodic trend
capacity of molecule to attract bonded electrons
Increases across; decreases down
EN and bond values
<.5 non- Polar
.5-1.9 polar covalent
1.9+ Ionic
Hydrogen bonding
very strong dipole bonds that invole a polar molecule conainting an H bonded to F, O, N`
Relattive Strenghs of intermolecular forced
Ion-Ion> H-Bonds> dipole-dipole> london (van der waals)
BP, MP and Intermolecular attractions
non-polar: larger molecules increase BP/MP
polar: smaller size increase BP+MP
STABILITY DOES NOT AFFECT BP/MP
Density
d=m/v
Specific Gravity
SGx=dx/dwater
When H20 is liquid; SG=d. SG>1 sink in h20 SG<1 float
Molarity
M= mol/V (L)
Percent by Mass
%(w/w)= (m sol x100)/(m soln)
Percent by Mass/volume
%(w/V)= (m sol (g) *100)/(V soln (mL))
Molality
m= (mol sol/ mass solv in Kg)
Mole Fraction
Xi= (mol of i)/ (total mol)X
Colligative property (pressure)
dissolving non volatile solvent into volative solution decreases pressure lower than pressure of original soln
P = Xsol * Po
Colligative property (boiling point) `
Dissolving nonvolatile solvent into volatile solution increases BP
deltaTb= Kb * m
Colligative property (freezing point)
dissolving a solute in a solvent lowers FP
deltaTf=Kf * m
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]
common weak strong electrolytes
- water soluable strong acids (HCl, HNO3, H2SO4)
- water soluable strong bases (NaOH, KOH)
- Walter soluble salts (NaCl, KNO3, K2SO4, NH4Cl)
common weak electrolytes
- water soluble weak acids (CH3COOH)
2. water soluable weak bases (NH3)
common non-electrolytes
- sugars like glucose and sucrose
2 alcohols like methanol and ethanol
dilutions
adding more solvent to a soln doesnt change solute present
Mi x Vi= Mf x Vf and %i * Vi= %f * Vf
Acid Properties
Taste sour
turns litmus red
leaves phenolphthalein colorless
pH below 7
Basic Properties
Taste bitter; feel slippery
turns litmus blue
turns phenolphthalein pink
ph greater than 7
arrhenius acid/base
Acid generates Hydronium ion and base generates hydroxide ions
bronsted lowry acid/base
acid is a proton donor
base if a proton acceptor
Lewis Definition
Acid is electron pair acceptor
base is electron pair donator
Common strong acids
HCL, HNO3, H2SO4, HCLO4
Common weak acids
CH3COOH, HF, H2CO3, H3PO4
common strong bases
metal hydroxide salts typically strong bases
weak bases
NH3
Cojugate base ions
Conjugate base of a weak acid is a weak base
conjugate base of a strong acid is not a base.
pH and pOH
pH=-log[H+] pOH=-log[OH-]
[H+]=in log(-pH) and {OH-]=in log(-pOH)
Kw=[H+}[OH-}=1x10^-14
buffer
combination of a weak acid and a weak base that resists changes in pH
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
Energy Units
SH H20= 1 cal= 4.18 J
heat equation (no change in state)
q=mass x SH x deltaT
Entropy (dS)
disorder increased dS is +; rxn spontaneous
disorder decreased dS is -; rnx non-spon
Enthalpy (dH)
evolves heat, exothermic, - , spontaneous
absorbs heat, endothermic, +, non-spon
Gibb’s Free Energy (dS)
energy is produced, -, spontaneous
energy is consumed, +, non-spon
zero, nil, at EQ.
quantum numbers
1st: shell (n)
2nd: subshell (l)
3rd orbital (ml)
4th spin (ms)
pauli eclusion principle
no two electrons in the same atom can have the same set of 4 quantum numbers
hund’s rule
electrons in the same subshell occupy availible orbitals singly, before paring up
aufbau principle
electrons occupy the loweste energy orbitals available
coordinate covalent bonds
one atom donates both shared electrons in a bond (lewis acid/base rxn_
charles law
as T increases V increases
Hig temp/ low pressure (states)
gas> liquid> solid
Low temperative/ high pressure (states
solid>liquid>gas
When do gases deviate from idea behavior
high pressure and low temperature
Keq values
Keq»1 P favored over R
Keq = 1 neither R or P favored
Keq«<1 R favored over P
Le Chatlelier’s Principle
a system at equilibrium is subjected to stress, eq shifts in a direction that alleviates stress
Teperatiure and eq
if heat is a product; incr temperature shifts to reactants and vice versa
Generally soluable ions
alkali and ammonium compounds
acetates, chlorates, nitrates, and perchlorates
Pb Hg and Ag salts when pared with above anions
Insoluble ions
Pb Hg and Ag unless paired with soluable anions!
van’t Hoff factor (i)
binary salt (NaCl)= 2 CaCl2= 3 solvation species= 1
Ka/Kb and acid/base strength
large values imply strong
small values imply weak
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.
Galvanic Cell
= redox rxn spontaneous
- creates electron flow
- oxidation at anode
- reduction at cathode
- cathode is +
- anode is -
- electrons flow from anode to cathode
electrolytic cell
- rxn nonspontaneous
- requires electron flow
- anode is +
- cathode is -
B- decay
decreases number of neutrons
increases number of protons
adds 1 to atomic number
.
B+ (positron) decay
Increases number of neutrons
decreases number of protons
subtracts one from atomic number
alpha decay
decreaes number of nutetrons and protons by 2 each
subtracts 4 from mass number and 2 from atomic
half life formula
N=N0 (1/2)^t/t1/2
