General Chemistry Tests (Bootcamp) Flashcards
(158 cards)
1
Q
A
2
Q
phase diagram
A
3
Q
Gibbs Equation
A
∆G=∆H-T∆S
4
Q
∆G is negative means
A
spontaneous
5
Q
∆G is positive means
A
non spontaneous
6
Q
∆G = 0 means
A
rxn is at equilibrium
7
Q
first order rxn rate constant
A
S^-1
y-axis: [ln]concentration
8
Q
second order rate constant
A
M^-1 S^-1
y axis: 1/concentration
9
Q
third order rate constant
A
M^-2 S^-1
10
Q
zero order graph
A
y axis: concentration
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)
12
Q
strong bases
A
group 1 metal hydroxides
Mg(OH)2
Ca(OH)2
Sr(OH)2
Ba(OH)2
13
Q
ideal gas law
A
PV=nRT
P1 x V1 / n1 x T1 = P2 x V2/ n2 x T2
14
Q
osmotic pressure
A
π= iMRT
pi = osmotic pressure
i = van hoff factor
M= molarity
R= constant (0.082)
15
Q
an uncharged element not bonded to other elements (H2, Na, Cl2) have an oxidation number of:
A
zero
16
Q
a monoatomic ion ( K+, S^2-, Mg^2+. Al^2+) have an oxidation number of
A
charge of ion
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
18
Q
freezing point equation
A
∆Tf= -Kf mi
i = van hoff factor
19
Q
the smallest van hoff factor =
A
highest freezing point
20
Q
density of gas formula
A
P= PM/RT
21
Q
colligative properties
A
freezing point
boiling point
vapor pressure
osmotic pressure
22
Q
non colligative properties
A
surface tension
color
solubility
viscosity
23
Q
half life for first order rxn
A
t1/2 = (0.693)/k
24
Q
alpha decay
A
nuclear product: 4/2 alpha product
result: reduces mass + atomic #
likely for: large nuclei
25
B decay ( B emission )
Nuclear particle: 0/-1 B product
Result: Neutron --> proton
Likely for: N/Z ration too high (too many neutrons)
26
B+ decay (positron emmission)
Nuclear particle: 0/+1 B product
Result: Proton -> neutron
Likely for: N/Z ratio too low (too many protons)
27
electron capture
nuclei particle: 0/-1 B reactant
result: proton-> neutron
likely for? N/Z ration too low (too many protons)
28
gamma decay
nuclear particle: 0/0 y product
result: no change
likely for: unpredictable
29
if the forward + backward activation energy = each other then,
enthalpy must be ZERO
30
keq =
[products]/[reactants]
31
increased keq =
increased amount of products
32
decreased keq =
increased amount of reactants
33
oxidized
compound losing electrons (becoming more positive)
34
reduced
compound gaining electrons ( becoming more negative)
35
reducing agent
oxidized in a chemical rxn
36
oxidizing agent
reduced in a chemical rxn
37
combustion rxn
CxHy + O2 --> _CO2 + _H2O
38
atomic size decreases from
from left to right (along a period)
bc of the increase of effective nuclear charge
39
atomic size increases when
going down a column
bc of adding electron shells and electron shielding
40
solubles
Group 1 metal cations
nitrate ( NO3-)
Perchlorate (ClO4-)
Acetate (C2H3O2-)
Ammonium ( NH4+)
41
Insolubles
Silver (Ag+)
Lead (Pb2+)
Sulfide (S 2-)
Hydroxide (OH-)
Dimercury (Hg2 2+)
Carbonate (CO3 -2)
Phosphate ( PO4 3-)
42
freezing point equation
tf= -ikfm
t= temp change
i= vanhoff
kf= constant
m= molarity
43
boiling point
temperature at which vapor pressure of the liquid equals the surrounding pressure
44
normal boiling point
temperature at which vapor pressure of the liquid equals 1 atmosphere of pressure
45
PV= nRT
pressure and temp are directly related
46
molarity of a solution
M= mol of solute/ L of the solution
47
volatility
ability of a liquid to evaporate
weak intermolecular forces
48
half life
mass remaining = (original mass) (1/2) ^2
49
HCl HF conjugate bases
Cl- F-
50
Ionic
interaction:ionic
properties: increases MP, brittle, hard
examples: NaCl, MgO
51
52
Metallic
interaction: metallic bonding
properties: variable hardness and MP, conducting
examples: Fe, Mg
53
Molecular
interaction: hydrogen bonding, dipole-dipole, london dispersion
properties: decreases M.P and nonconducting
Examples: H2, CO2
54
Network
interaction: covalent bonding
properties: increased M.P, hard, nonconducting
examples: C(diamond), SiO2 (Quartz)
55
pH formulas
pH+pOH=14
pH= 14-pOH
10^-ph = [H+]
56
internal energy
∆E=q+w
∆E = change in internal energy
q= change in heat
w= amount of work done or to the system
57
+q
heat is transferred to the system (from surrounding)
58
-q (exothermic)
heat is transferred to the surroundings (from the system)
59
+w
the surrounding does work on the system (compression)
60
-w
the system does work on the surrounding (expansion)
61
kinetic theory of gases
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,
62
saturated
contains the maximum amount of solute that a solvent can dissolve
rate of dissolution = crystallization
63
Alkali metals
react vigorously upon contact with water
64
Activated complex
unstable arrangement of atoms that exists momentarily at the peak of the activation energy barrier (transition state)
65
isotope
2 or more atoms that have the same atomic # but different atomic masses
same number of protons but different number of neutrons
66
homogenous mixtures
separated using distillations
different boiling points are used
evaporated compound cooled through the condenser and collected on other end of flask
67
How to balance rxns under acidic conditions:
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
Ideal Gas Assumptions
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
when do real gases behave ideally?
under low pressure and high temperature
70
kinetic energy = temperature
71
↑ ksp =
high solubility
72
↓ksp =
least solubility
73
work done when a gas is heated at constant pressure
w= -P∆V= -P(V2-V1)
74
partial pressure equation
P1 = x1(Pr)
75
electron domain: 2
non bonding electron pairs: 0
hybridization: sp
electron domain geometry: linear
molecular geometry: linear
bond angle: 180
76
electron domain: 3
non bonding electron pairs: 0
hybridization: sp2
electron domain geometry: trigonal planar
molecular geometry: trigonal planar
bond angle: 120
77
electron domain: 3
non bonding electron pairs: 1
hybridization: sp2
electron domain geometry: trigonal planar
molecular geometry: bent
bond angle: < 120
78
electron domain: 4
non bonding electron pairs: 0
hybridization: sp3
electron domain geometry: tetrahedral
molecular geometry: tetrahedral
bond angle: 109.5
79
electron domain: 4
non bonding electron pairs: 1
hybridization: sp3
electron domain geometry: tetrahedral
molecular geometry: trigonal pyramidal
bond angle: < 109.5
80
electron domain: 4
non bonding electron pairs: 2
hybridization: sp3
electron domain geometry: tetrahedral
molecular geometry: bent
bond angle: <<109.5
81
electron domain: 5
non bonding electron pairs: 0
hybridization: sp3d
electron domain geometry: trigonal bipyramid
molecular geometry: trigonal bypryramid
bond angle: 90, 120, 180
82
electron domain: 5
non bonding electron pairs: 1
hybridization: sp3d
electron domain geometry: trigonal bipyramid
molecular geometry: see saw
bond angle: < 90, < 120
83
electron domain: 5
non bonding electron pairs: 2
hybridization: sp3d
electron domain geometry: trigonal bipyramid
molecular geometry: t-shaped
bond angle: < 90
84
electron domain: 5
non bonding electron pairs: 3
hybridization: sp3d
electron domain geometry: trigonal bipyramid
molecular geometry: linear
bond angle: 180
85
electron domain: 6
non bonding electron pairs: 0
hybridization: sp3d2
electron domain geometry: octahedral
molecular geometry: octahedral
bond angle: 90
86
electron domain: 6
non bonding electron pairs: 1
hybridization: sp3d2
electron domain geometry: octahedral
molecular geometry: square pyramid
bond angle: <90
87
electron domain: 6
non bonding electron pairs: 2
hybridization: sp3d2
electron domain geometry: octahedral
molecular geometry: square planar
bond angle: 90
88
heat of rxn in a bomb calorimeter
qrxn= -c (∆T)
c= heat capacity
89
how do you separate a homogenous mixture?
distillation
then use a condenser to cool evaporated compounds involved in distillations
90
buret is used in
titrations
determines concentrations
91
pipette
transfer small volumes
92
filter
separate heterogeneous mixture
93
separatory funnel
separates heterogenous mixtures
94
why does a nucleus weigh less than the sum of its neutrons and protons?
some of the nucleuses mass is converted into nuclear binding energy
95
electron affinity
energy is released when an atom gains an electron
96
electron negativity
tendency for an atom to attract electrons to itself in a bond
97
ionization energy
amount of energy required for an atom to lose an electron
98
real gas exhibits ideal gas behavior
at high temperature and low pressure
99
strongest interactions
largest charge and small size
100
lewis acid
accepts an electron pair
101
lewis base
donates an electron pair
102
rotten egg smell
sulfur
H2S
103
List order of energy of waves from least to strongest
Radiowaves < Microwaves < Infrared < Visible Light < Ultraviolet < X-Rays < Gamma rays
104
energy of wave is inverse to
wavelength
105
heating curve
106
voltaic/galvanic cell
107
electrolytic cell
108
diatomic elements
Hydrogen
- gas
Nitrogen
- gas
Oxygen
-gas
Fluorine
- gas
Chlorine
- gas
Bromine
- liquid
Iodine
- solid
109
Arrhenius Equation
k= Ae^(-Ea/RT)
110
According to Arrhenius Equation, an increase in temp. causes:
increase in rxn rate
increase in collision frequency
increase in rate constant
111
specific heat equation
q=mcs (Tf-Ti)
112
coordinate diagrams
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
if products are at a higher level than reactants, then
it is endothermic ( consumes heat )
114
activation energy determines
the minimum energy input necessary to start rxn
it is the high between the reactants and top of the hill
115
transition metals
High MP
several oxidation states
tendency to form brightly colored compounds
often paramagnetic
d block that are unfilled or half filled
116
metalloids
117
standard electrochemical cell potential
E cell = E reduction + E oxidation
+ E cell = spontaneous for oxidation reduction
118
titration curves
per straight line = amount of H in it
119
Q < K
shift to right (products)
120
Q > K
equilibrium shifts left (reactants)
121
Q=K
at equilibrium
122
zero order
horizontal and verticles both decrease
123
second order
horizontal increase
verticles decrease
124
first order
horizontals stay the same
verticles decrease
125
the normal freezing point
1 atm
126
the normal boiling point
1 atm
127
Grahams Law of Effusion
describes rate at which gas escapes or effuses from a container relative to another gas
128
when solute is added to a liquid:
Increase in BP
Increase in osmotic pressure
decrease in vapor pressure
decrease in freezing point
129
crystalline solids
longe range order
consistent crystal structure
well defined melting temp
break with cleavage along a straight plane
130
amorphous solids
short range order
no consistent structure
broad range of melting temperature
irregular breakage patterns
131
strong base and strong acid
ex. HCl and NaOH
salt formed: NaCl (neutral)
pH at equivalence: 7
132
weak acid and strong base
ex. HF + NaOH
Salt formed: NaF (basic)
pH equivalence: >7
133
weak base and strong acid
ex. NH3 + HCl
salt formed: NH3 + HCl
salt formed: NH4Cl (acidic)
pH at equivalence: <7
134
state function ( valve does not depend on how that state was achieved )
enthalpy
volume
mass
gibbs free energy
135
path functions (process matters + depend on the transition of the state )
work
heat
heat capacity
136
heat energy equation
q= mc∆t
q= heat transferred
m= mass
c= specific heat
t=temp change
137
charles law
v1/t1 = v2/t2
138
gases that are in the same temperature =
same kinetic energy
139
increase in temperature =
decreases in gases solubility
140
increase in pressure =
increase in gases solubility
141
Alkaline Buffer solution
mixture of weak base and conjugate acid
142
Acidic Buffer solution
mixture of a weak acid + conjugate base
143
isotope with the atomic mass closest to the avg. atomic mass is the
MOST ABUNDANT
144
spontaneous at all temps =
- ∆H
+∆S
-T∆S
- ∆G
145
non spontaneous at all temps.
+∆H
- ∆S
+ T∆S
+∆G
146
spontaneous at low temp.
(-)∆H
(-) ∆S
+ T∆S
∆G depends
147
spontaneous at high temp.
+ ∆H
+ ∆S
- T∆S
∆G depends
148
a reducing agent is
oxidized
149
an oxidizing agent is
reduced
150
the molecule with the lowest reducing potential will be
oxidized in a chemical rxn
151
intermediates and products never appear
in the rate equation
152
intermediates are always
consumed in a rxn
153
temperature is related to
pressure, kinetic energy, and vapor pressure
154
lowering the KE will
cause the gas particles to condense
155
solutes with smaller solubilities product constant (ksp) valves
precipitate first
156
boyles law
pressure is inversely related to volume
157
metals are
good conductors of electricity
malleable
ductile
high melting point
158
when determining bond angles
the more lone pairs around the central atom = smaller the overall bond angles
