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PCAT > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

1
Q

Cobalt names and charges

A

Co2+ Cobaltous. Cobalt II

Co3+. Cobaltic. Cobalt III

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2
Q

Iron charges and names

A

Fe2+, Ferrous iron II

Fe3+ ferric iron III

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4
Q

Mass number

A

A number of protons and neutrons

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6
Q

Atomic number

A

Z

Number of protons in the nuc

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7
Q

Sulfate

A

2-

SO4

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8
Q

carbonate

A

2-

CO3

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9
Q

Perchlorate

A

1-

ClO4

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10
Q

bicarbonate

A

-1

HCO3

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11
Q

Chlorate

A

1-

ClO3

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12
Q

peroxide

A

2-

O2

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13
Q

phosphate

A

3-

PO4

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14
Q

permanganate

A

1-

Mn04

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15
Q

Hypochlorite

A

-1

ClO

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16
Q

Nitrate

A

-1

NO3

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17
Q

Idea Gas Law

A

PV=nRT R=.082

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18
Q

Idea Gas Law Proportionality

A

opposite sides are directly proportional; same side is inversely proportional

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19
Q

Law of Partial Pressures

A

Ptotal=P1+P2+P3….

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20
Q

Gas collected over water (wet)

A

must subtract the vapor pressure of water from the total gas pressure

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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)

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22
Q

Kinetic Molecular Model

A
  1. gaseous molecules are widely dispersed
    2 gas molecules travel in random straight motion
  2. avg KE is directly proportional to abs T of the gas.
    4Collisions of molecules are ellastic (no momentum loss)
  3. collisions due to the molecules and walls of container
  4. do not attract each other
  5. volume occupied by molecule negligible to V of the container.
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23
Q

Electronegativity (EN) and periodic trend

A

capacity of molecule to attract bonded electrons

Increases across; decreases down

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24
Q

EN and bond values

A

<.5 non- Polar
.5-1.9 polar covalent
1.9+ Ionic

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25
Q

Hydrogen bonding

A

very strong dipole bonds that invole a polar molecule conainting an H bonded to F, O, N`

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26
Q

Relattive Strenghs of intermolecular forced

A

Ion-Ion> H-Bonds> dipole-dipole> london (van der waals)

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27
Q

BP, MP and Intermolecular attractions

A

non-polar: larger molecules increase BP/MP
polar: smaller size increase BP+MP

STABILITY DOES NOT AFFECT BP/MP

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28
Q

Density

A

d=m/v

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29
Q

Specific Gravity

A

SGx=dx/dwater

When H20 is liquid; SG=d. SG>1 sink in h20 SG<1 float

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30
Q

Molarity

A

M= mol/V (L)

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31
Q

Percent by Mass

A

%(w/w)= (m sol x100)/(m soln)

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32
Q

Percent by Mass/volume

A

%(w/V)= (m sol (g) *100)/(V soln (mL))

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33
Q

Molality

A

m= (mol sol/ mass solv in Kg)

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34
Q

Mole Fraction

A

Xi= (mol of i)/ (total mol)X

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35
Q

Colligative property (pressure)

A

dissolving non volatile solvent into volative solution decreases pressure lower than pressure of original soln

P = Xsol * Po

36
Q

Colligative property (boiling point) `

A

Dissolving nonvolatile solvent into volatile solution increases BP

deltaTb= Kb * m

37
Q

Colligative property (freezing point)

A

dissolving a solute in a solvent lowers FP

deltaTf=Kf * m

38
Q

Greatest Colligative Effect Problems

A

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
Q

common weak strong electrolytes

A
  1. water soluable strong acids (HCl, HNO3, H2SO4)
  2. water soluable strong bases (NaOH, KOH)
  3. Walter soluble salts (NaCl, KNO3, K2SO4, NH4Cl)
40
Q

common weak electrolytes

A
  1. water soluble weak acids (CH3COOH)

2. water soluable weak bases (NH3)

41
Q

common non-electrolytes

A
  1. sugars like glucose and sucrose

2 alcohols like methanol and ethanol

42
Q

dilutions

A

adding more solvent to a soln doesnt change solute present

Mi x Vi= Mf x Vf and %i * Vi= %f * Vf

43
Q

Acid Properties

A

Taste sour
turns litmus red
leaves phenolphthalein colorless
pH below 7

44
Q

Basic Properties

A

Taste bitter; feel slippery
turns litmus blue
turns phenolphthalein pink
ph greater than 7

45
Q

arrhenius acid/base

A

Acid generates Hydronium ion and base generates hydroxide ions

46
Q

bronsted lowry acid/base

A

acid is a proton donor

base if a proton acceptor

47
Q

Lewis Definition

A

Acid is electron pair acceptor

base is electron pair donator

48
Q

Common strong acids

A

HCL, HNO3, H2SO4, HCLO4

49
Q

Common weak acids

A

CH3COOH, HF, H2CO3, H3PO4

50
Q

common strong bases

A

metal hydroxide salts typically strong bases

51
Q

weak bases

A

NH3

52
Q

Cojugate base ions

A

Conjugate base of a weak acid is a weak base

conjugate base of a strong acid is not a base.

53
Q

pH and pOH

A

pH=-log[H+] pOH=-log[OH-]
[H+]=in log(-pH) and {OH-]=in log(-pOH)
Kw=[H+}[OH-}=1x10^-14

54
Q

buffer

A

combination of a weak acid and a weak base that resists changes in pH

55
Q

Acid/Base SToichiometry formula

A

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
Q

Energy Units

A

SH H20= 1 cal= 4.18 J

57
Q

heat equation (no change in state)

A

q=mass x SH x deltaT

58
Q

Entropy (dS)

A

disorder increased dS is +; rxn spontaneous

disorder decreased dS is -; rnx non-spon

59
Q

Enthalpy (dH)

A

evolves heat, exothermic, - , spontaneous

absorbs heat, endothermic, +, non-spon

60
Q

Gibb’s Free Energy (dS)

A

energy is produced, -, spontaneous

energy is consumed, +, non-spon

zero, nil, at EQ.

61
Q

quantum numbers

A

1st: shell (n)
2nd: subshell (l)
3rd orbital (ml)
4th spin (ms)

62
Q

pauli eclusion principle

A

no two electrons in the same atom can have the same set of 4 quantum numbers

63
Q

hund’s rule

A

electrons in the same subshell occupy availible orbitals singly, before paring up

64
Q

aufbau principle

A

electrons occupy the loweste energy orbitals available

65
Q

coordinate covalent bonds

A

one atom donates both shared electrons in a bond (lewis acid/base rxn_

66
Q

charles law

A

as T increases V increases

67
Q

Hig temp/ low pressure (states)

A

gas> liquid> solid

68
Q

Low temperative/ high pressure (states

A

solid>liquid>gas

69
Q

When do gases deviate from idea behavior

A

high pressure and low temperature

70
Q

Keq values

A

Keq»1 P favored over R
Keq = 1 neither R or P favored
Keq«<1 R favored over P

71
Q

Le Chatlelier’s Principle

A

a system at equilibrium is subjected to stress, eq shifts in a direction that alleviates stress

72
Q

Teperatiure and eq

A

if heat is a product; incr temperature shifts to reactants and vice versa

73
Q

Generally soluable ions

A

alkali and ammonium compounds

acetates, chlorates, nitrates, and perchlorates

Pb Hg and Ag salts when pared with above anions

74
Q

Insoluble ions

A

Pb Hg and Ag unless paired with soluable anions!

75
Q

van’t Hoff factor (i)

A 
binary salt (NaCl)= 2
CaCl2= 3
solvation species= 1
76
Q

Ka/Kb and acid/base strength

A

large values imply strong

small values imply weak

77
Q

Reduction table reduced/ oxidized species

A

Most easily reduced species bottom left; least easily top left

most easily oxidiezed at top right; least easily oxidied at bottom right.

78
Q

Galvanic Cell

A

= redox rxn spontaneous

  • creates electron flow
  • oxidation at anode
  • reduction at cathode
  • cathode is +
  • anode is -
  • electrons flow from anode to cathode
79
Q

electrolytic cell

A
  • rxn nonspontaneous
  • requires electron flow
  • anode is +
  • cathode is -
80
Q

B- decay

A

decreases number of neutrons
increases number of protons
adds 1 to atomic number
.

81
Q

B+ (positron) decay

A

Increases number of neutrons
decreases number of protons
subtracts one from atomic number

82
Q

alpha decay

A

decreaes number of nutetrons and protons by 2 each

subtracts 4 from mass number and 2 from atomic

83
Q

half life formula

A

N=N0 (1/2)^t/t1/2

PCAT (5 decks)

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