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General Chemistry > General Chemistry Tests (Bootcamp) > Flashcards

General Chemistry Tests (Bootcamp) Flashcards

1
Q
A
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2
Q

phase diagram

A
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3
Q

Gibbs Equation

A

∆G=∆H-T∆S

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4
Q

∆G is negative means

A

spontaneous

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5
Q

∆G is positive means

A

non spontaneous

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6
Q

∆G = 0 means

A

rxn is at equilibrium

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7
Q

first order rxn rate constant

A

S^-1

y-axis: [ln]concentration

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8
Q

second order rate constant

A

M^-1 S^-1

y axis: 1/concentration

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9
Q

third order rate constant

A

M^-2 S^-1

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10
Q

zero order graph

A

y axis: concentration

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11
Q

strong acids

A

HCl (hydrochloric acid)
HBr (hydrobromic acid)
HI (hydroiodic acid)
H2SO4 (sulfuric acid)
HNO3 (nitric acid)
HClO3 (chloric acid)
HClO4 (perchloric acid)

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12
Q

strong bases

A

group 1 metal hydroxides
Mg(OH)2
Ca(OH)2
Sr(OH)2
Ba(OH)2

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13
Q

ideal gas law

A

PV=nRT

P1 x V1 / n1 x T1 = P2 x V2/ n2 x T2

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14
Q

osmotic pressure

A

π= iMRT

pi = osmotic pressure
i = van hoff factor
M= molarity
R= constant (0.082)

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15
Q

an uncharged element not bonded to other elements (H2, Na, Cl2) have an oxidation number of:

A

zero

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16
Q

a monoatomic ion ( K+, S^2-, Mg^2+. Al^2+) have an oxidation number of

A

charge of ion

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17
Q

a non metal has a charge of

A

usually negative

-2 O2 usually
-1 with peroxides (H2O2)
+1 hydrogen when bonded to a non metal

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18
Q

freezing point equation

A

∆Tf= -Kf mi

i = van hoff factor

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19
Q

the smallest van hoff factor =

A

highest freezing point

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20
Q

density of gas formula

A

P= PM/RT

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21
Q

colligative properties

A

freezing point
boiling point
vapor pressure
osmotic pressure

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22
Q

non colligative properties

A

surface tension
color
solubility
viscosity

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23
Q

half life for first order rxn

A

t1/2 = (0.693)/k

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24
Q

alpha decay

A

nuclear product: 4/2 alpha product

result: reduces mass + atomic #

likely for: large nuclei

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25
Q

B decay ( B emission )

A

Nuclear particle: 0/-1 B product

Result: Neutron –> proton

Likely for: N/Z ration too high (too many neutrons)

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26
Q

B+ decay (positron emmission)

A

Nuclear particle: 0/+1 B product

Result: Proton -> neutron

Likely for: N/Z ratio too low (too many protons)

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27
Q

electron capture

A

nuclei particle: 0/-1 B reactant

result: proton-> neutron

likely for? N/Z ration too low (too many protons)

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28
Q

gamma decay

A

nuclear particle: 0/0 y product

result: no change

likely for: unpredictable

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29
Q

if the forward + backward activation energy = each other then,

A

enthalpy must be ZERO

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30
Q

keq =

A

[products]/[reactants]

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31
Q

increased keq =

A

increased amount of products

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32
Q

decreased keq =

A

increased amount of reactants

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33
Q

oxidized

A

compound losing electrons (becoming more positive)

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34
Q

reduced

A

compound gaining electrons ( becoming more negative)

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35
Q

reducing agent

A

oxidized in a chemical rxn

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36
Q

oxidizing agent

A

reduced in a chemical rxn

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37
Q

combustion rxn

A

CxHy + O2 –> _CO2 + _H2O

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38
Q

atomic size decreases from

A

from left to right (along a period)

bc of the increase of effective nuclear charge

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39
Q

atomic size increases when

A

going down a column

bc of adding electron shells and electron shielding

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40
Q

solubles

A

Group 1 metal cations

nitrate ( NO3-)

Perchlorate (ClO4-)

Acetate (C2H3O2-)

Ammonium ( NH4+)

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41
Q

Insolubles

A

Silver (Ag+)

Lead (Pb2+)

Sulfide (S 2-)

Hydroxide (OH-)

Dimercury (Hg2 2+)

Carbonate (CO3 -2)

Phosphate ( PO4 3-)

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42
Q

freezing point equation

A

tf= -ikfm

t= temp change
i= vanhoff
kf= constant
m= molarity

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43
Q

boiling point

A

temperature at which vapor pressure of the liquid equals the surrounding pressure

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44
Q

normal boiling point

A

temperature at which vapor pressure of the liquid equals 1 atmosphere of pressure

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45
Q

PV= nRT

A

pressure and temp are directly related

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46
Q

molarity of a solution

A

M= mol of solute/ L of the solution

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47
Q

volatility

A

ability of a liquid to evaporate

weak intermolecular forces

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48
Q

half life

A

mass remaining = (original mass) (1/2) ^2

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49
Q

HCl HF conjugate bases

A

Cl- F-

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50
Q

Ionic

A

interaction:ionic

properties: increases MP, brittle, hard

examples: NaCl, MgO

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51
Q
A
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52
Q

Metallic

A

interaction: metallic bonding

properties: variable hardness and MP, conducting

examples: Fe, Mg

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53
Q

Molecular

A

interaction: hydrogen bonding, dipole-dipole, london dispersion

properties: decreases M.P and nonconducting

Examples: H2, CO2

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54
Q

Network

A

interaction: covalent bonding

properties: increased M.P, hard, nonconducting

examples: C(diamond), SiO2 (Quartz)

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55
Q

pH formulas

A

pH+pOH=14

pH= 14-pOH

10^-ph = [H+]

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56
Q

internal energy

A

∆E=q+w

∆E = change in internal energy

q= change in heat

w= amount of work done or to the system

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57
Q

+q

A

heat is transferred to the system (from surrounding)

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58
Q

-q (exothermic)

A

heat is transferred to the surroundings (from the system)

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59
Q

+w

A

the surrounding does work on the system (compression)

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60
Q

-w

A

the system does work on the surrounding (expansion)

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61
Q

kinetic theory of gases

A
  1. gases are composed of particles that do not have defined volume, yet have a defined mass. the size is minuscule in comparison to the distance between them (considered negligible)
  2. there are no intermolecular attractions or repulsions between the gas molecules
  3. gas particles are always in continuous, random motion
  4. collisions between gas particles are elastic, no loss or gain of kinetic energy when particles collide
  5. average kinetic energy is always the same for all gases at a specific temperature, regardless of the identity of the gas. The kinetic energy is proportional to the absolute temperature of the gas,
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62
Q

saturated

A

contains the maximum amount of solute that a solvent can dissolve

rate of dissolution = crystallization

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63
Q

Alkali metals

A

react vigorously upon contact with water

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64
Q

Activated complex

A

unstable arrangement of atoms that exists momentarily at the peak of the activation energy barrier (transition state)

65
Q

isotope

A

2 or more atoms that have the same atomic # but different atomic masses

same number of protons but different number of neutrons

66
Q

homogenous mixtures

A

separated using distillations

different boiling points are used

evaporated compound cooled through the condenser and collected on other end of flask

67
Q

How to balance rxns under acidic conditions:

A

1) Balance all the elements other than H and O
2) Balance O atoms by adding H2O as needed
3) Balance H atoms by adding H+ as needed
4) Balance charge by adding e- as needed

68
Q

Ideal Gas Assumptions

A

1) The volume or size of each individual gas molecule is insignificant
- when the volume or space that a gas occupies is high, the volume of the individual gas particles becomes insignificant compared to the distance between them
- high volume gas = low pressure gas, as pressure and volume are inversely related
- at low pressures, the volume of individual gas particles is insignificant and the gas is likely to behave ideally

2) Gas molecules collisions with each other are perfectly elastic. No intermolecular forces.
- completely overcoming a gas intermolecular forces to create perfectly elastic collisions require very high kinetic energy
- high kinetic energy gas =high temperature gas, as kinetic energy and temperature are directly related
- at high temperature, collisions between gas molecules become elastic and the gas is likely to behave ideally

69
Q

when do real gases behave ideally?

A

under low pressure and high temperature

70
Q

kinetic energy = temperature

A
71
Q

↑ ksp =

A

high solubility

72
Q

↓ksp =

A

least solubility

73
Q

work done when a gas is heated at constant pressure

A

w= -P∆V= -P(V2-V1)

74
Q

partial pressure equation

A

P1 = x1(Pr)

75
Q

electron domain: 2
non bonding electron pairs: 0

A

hybridization: sp
electron domain geometry: linear
molecular geometry: linear
bond angle: 180

76
Q

electron domain: 3
non bonding electron pairs: 0

A

hybridization: sp2
electron domain geometry: trigonal planar
molecular geometry: trigonal planar
bond angle: 120

77
Q

electron domain: 3
non bonding electron pairs: 1

A

hybridization: sp2
electron domain geometry: trigonal planar
molecular geometry: bent
bond angle: < 120

78
Q

electron domain: 4
non bonding electron pairs: 0

A

hybridization: sp3
electron domain geometry: tetrahedral
molecular geometry: tetrahedral
bond angle: 109.5

79
Q

electron domain: 4
non bonding electron pairs: 1

A

hybridization: sp3
electron domain geometry: tetrahedral
molecular geometry: trigonal pyramidal
bond angle: < 109.5

80
Q

electron domain: 4
non bonding electron pairs: 2

A

hybridization: sp3
electron domain geometry: tetrahedral
molecular geometry: bent
bond angle: «109.5

81
Q

electron domain: 5
non bonding electron pairs: 0

A

hybridization: sp3d
electron domain geometry: trigonal bipyramid
molecular geometry: trigonal bypryramid
bond angle: 90, 120, 180

82
Q

electron domain: 5
non bonding electron pairs: 1

A

hybridization: sp3d
electron domain geometry: trigonal bipyramid
molecular geometry: see saw
bond angle: < 90, < 120

83
Q

electron domain: 5
non bonding electron pairs: 2

A

hybridization: sp3d
electron domain geometry: trigonal bipyramid
molecular geometry: t-shaped
bond angle: < 90

84
Q

electron domain: 5
non bonding electron pairs: 3

A

hybridization: sp3d
electron domain geometry: trigonal bipyramid
molecular geometry: linear
bond angle: 180

85
Q

electron domain: 6
non bonding electron pairs: 0

A

hybridization: sp3d2
electron domain geometry: octahedral
molecular geometry: octahedral
bond angle: 90

86
Q

electron domain: 6
non bonding electron pairs: 1

A

hybridization: sp3d2
electron domain geometry: octahedral
molecular geometry: square pyramid
bond angle: <90

87
Q

electron domain: 6
non bonding electron pairs: 2

A

hybridization: sp3d2
electron domain geometry: octahedral
molecular geometry: square planar
bond angle: 90

88
Q

heat of rxn in a bomb calorimeter

A

qrxn= -c (∆T)

c= heat capacity

89
Q

how do you separate a homogenous mixture?

A

distillation

then use a condenser to cool evaporated compounds involved in distillations

90
Q

buret is used in

A

titrations
determines concentrations

91
Q

pipette

A

transfer small volumes

92
Q

filter

A

separate heterogeneous mixture

93
Q

separatory funnel

A

separates heterogenous mixtures

94
Q

why does a nucleus weigh less than the sum of its neutrons and protons?

A

some of the nucleuses mass is converted into nuclear binding energy

95
Q

electron affinity

A

energy is released when an atom gains an electron

96
Q

electron negativity

A

tendency for an atom to attract electrons to itself in a bond

97
Q

ionization energy

A

amount of energy required for an atom to lose an electron

98
Q

real gas exhibits ideal gas behavior

A

at high temperature and low pressure

99
Q

strongest interactions

A

largest charge and small size

100
Q

lewis acid

A

accepts an electron pair

101
Q

lewis base

A

donates an electron pair

102
Q

rotten egg smell

A

sulfur

H2S

103
Q

List order of energy of waves from least to strongest

A

Radiowaves < Microwaves < Infrared < Visible Light < Ultraviolet < X-Rays < Gamma rays

104
Q

energy of wave is inverse to

A

wavelength

105
Q

heating curve

A
106
Q

voltaic/galvanic cell

A
107
Q

electrolytic cell

A
108
Q

diatomic elements

A

Hydrogen
- gas

Nitrogen
- gas

Oxygen
-gas

Fluorine
- gas

Chlorine
- gas

Bromine
- liquid

Iodine
- solid

109
Q

Arrhenius Equation

A

k= Ae^(-Ea/RT)

110
Q

According to Arrhenius Equation, an increase in temp. causes:

A

increase in rxn rate

increase in collision frequency

increase in rate constant

111
Q

specific heat equation

A

q=mcs (Tf-Ti)

112
Q

coordinate diagrams

A

if products and reactants are at the same level = isothermic

if products are at a lower level than the reactant, then ∆H is negative = exothermic (gives off heat)

113
Q

if products are at a higher level than reactants, then

A

it is endothermic ( consumes heat )

114
Q

activation energy determines

A

the minimum energy input necessary to start rxn

it is the high between the reactants and top of the hill

115
Q

transition metals

A

High MP

several oxidation states

tendency to form brightly colored compounds

often paramagnetic

d block that are unfilled or half filled

116
Q

metalloids

A
117
Q

standard electrochemical cell potential

A

E cell = E reduction + E oxidation

+ E cell = spontaneous for oxidation reduction

118
Q

titration curves

A

per straight line = amount of H in it

119
Q

Q < K

A

shift to right (products)

120
Q

Q > K

A

equilibrium shifts left (reactants)

121
Q

Q=K

A

at equilibrium

122
Q

zero order

A

horizontal and verticles both decrease

123
Q

second order

A

horizontal increase
verticles decrease

124
Q

first order

A

horizontals stay the same
verticles decrease

125
Q

the normal freezing point

A

1 atm

126
Q

the normal boiling point

A

1 atm

127
Q

Grahams Law of Effusion

A

describes rate at which gas escapes or effuses from a container relative to another gas

128
Q

when solute is added to a liquid:

A

Increase in BP
Increase in osmotic pressure
decrease in vapor pressure
decrease in freezing point

129
Q

crystalline solids

A

longe range order

consistent crystal structure

well defined melting temp

break with cleavage along a straight plane

130
Q

amorphous solids

A

short range order

no consistent structure

broad range of melting temperature

irregular breakage patterns

131
Q

strong base and strong acid

A

ex. HCl and NaOH

salt formed: NaCl (neutral)

pH at equivalence: 7

132
Q

weak acid and strong base

A

ex. HF + NaOH

Salt formed: NaF (basic)

pH equivalence: >7

133
Q

weak base and strong acid

A

ex. NH3 + HCl

salt formed: NH3 + HCl

salt formed: NH4Cl (acidic)

pH at equivalence: <7

134
Q

state function ( valve does not depend on how that state was achieved )

A

enthalpy
volume
mass
gibbs free energy

135
Q

path functions (process matters + depend on the transition of the state )

A

work
heat
heat capacity

136
Q

heat energy equation

A

q= mc∆t

q= heat transferred
m= mass
c= specific heat
t=temp change

137
Q

charles law

A

v1/t1 = v2/t2

138
Q

gases that are in the same temperature =

A

same kinetic energy

139
Q

increase in temperature =

A

decreases in gases solubility

140
Q

increase in pressure =

A

increase in gases solubility

141
Q

Alkaline Buffer solution

A

mixture of weak base and conjugate acid

142
Q

Acidic Buffer solution

A

mixture of a weak acid + conjugate base

143
Q

isotope with the atomic mass closest to the avg. atomic mass is the

A

MOST ABUNDANT

144
Q

spontaneous at all temps =

A
  • ∆H
    +∆S
    -T∆S
  • ∆G
145
Q

non spontaneous at all temps.

A

+∆H
- ∆S
+ T∆S
+∆G

146
Q

spontaneous at low temp.

A

(-)∆H
(-) ∆S
+ T∆S
∆G depends

147
Q

spontaneous at high temp.

A

+ ∆H
+ ∆S
- T∆S
∆G depends

148
Q

a reducing agent is

A

oxidized

149
Q

an oxidizing agent is

A

reduced

150
Q

the molecule with the lowest reducing potential will be

A

oxidized in a chemical rxn

151
Q

intermediates and products never appear

A

in the rate equation

152
Q

intermediates are always

A

consumed in a rxn

153
Q

temperature is related to

A

pressure, kinetic energy, and vapor pressure

154
Q

lowering the KE will

A

cause the gas particles to condense

155
Q

solutes with smaller solubilities product constant (ksp) valves

A

precipitate first

156
Q

boyles law

A

pressure is inversely related to volume

157
Q

metals are

A

good conductors of electricity

malleable

ductile

high melting point

158
Q

when determining bond angles

A

the more lone pairs around the central atom = smaller the overall bond angles

General Chemistry (3 decks)

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