TEST 1- CHEM1211 + Ch. 10, 12 Flashcards
1
Q
2 regions of electron density with 0 lone pairs
A
Linear, linear, 180
2
Q
2 regions of electron density with 1 lone pair
A
Linear, linear, 180
3
Q
3 regions of electron density with 0 lone pairs
A
Trigonal planar, trigonal planar, 120
4
Q
3 regions of electron density with 1 lone pair
A
Trigonal planar, bent, 120
5
Q
4 regions of electron density with 0 lone pairs
A
Tetrahedral, tetrahedral, 109.5
6
Q
4 regions of electron density with 1 lone pair
A
Tetrahedral, trigonal pyramidal, 109.5
7
Q
4 regions of electron density with 2 lone pairs
A
Tetrahedral, bent, 109.5
8
Q
5 regions of electron density with 0 lone pairs
A
Trigonal bipyramidal, trigonal bipyramidal, 90 or 120
9
Q
5 regions of electron density with 1 lone pair
A
Trigonal bipyramidal, seasaw, 90 or 120
10
Q
5 regions of electron density with 2 lone pairs
A
Trigonal bipyramidal, T-shaped, 90 or 120
11
Q
5 regions of electron density with 3 lone pairs
A
Trigonal bipyramidal, linear, 90 or 120
12
Q
6 regions of electron density with 0 lone pairs
A
Octahedral, octahedral, 90 or 180
13
Q
6 regions of electron density with 1 lone pair
A
Octahedral, square pyramidal, 90 or 180
14
Q
6 regions of electron density with 2 lone pairs
A
Octahedral, square planar, 90 or 180
15
Q
Always polar
A
Bent, trigonal pyramidal, seesaw, T-shaped, square pyramidal
16
Q
Not always polar
A
Linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral, square planar
17
Q
Salts consisting of K+
A
Always soluble
18
Q
Salts consisting of Na+
A
Always soluble
19
Q
Salts consisting of NH4+
A
Always soluble
20
Q
Salts consisting of CH3COO- (acetic acid)
A
Always soluble
21
Q
Salts consisting of ClO3- and ClO4-
A
Always soluble
22
Q
Salts consisting of NO3-
A
Always soluble
23
Q
Salts consisting of Br-
A
Soluble, insoluble with Hg2 2+, Pb 2+ , Ag+
24
Q
Salts consisting of Cl-
A
Soluble, insoluble with Hg2 2+, Pb 2+ , Ag+
25
Salts consisting of I-
Soluble, insoluble with Hg2 2+, Pb 2+ , Ag+
26
Salts consisting of F-
Soluble, insoluble with Ba 2+, Ca 2+, Pb 2+, Sr 2+, Ag+
27
Salts consisting of SO4 2-
Soluble, insoluble with Ba 2+, Ca 2+, Pb 2+, Sr 2+, Ag+
28
Compounds with OH-
Insoluble, soluble with Ba 2+, K+, Na+
29
Salts consisting of S 2-
Insoluble, soluble with Ba 2+, K+, Na+, NH 4+
30
Salts consisting of CO3 2-
Insoluble, soluble with K+, Na+, NH4+
31
Compounds consisting of O 2-
Insoluble, soluble with Ba+, K+, Na+
32
Salts consisting of PO4 3-
Insoluble, soluble with K+, Na+, NH4+
33
CrO4 2- solubility
Insoluble, soluble with NH4 +, alkali metal cations
34
C2O4 2- Solubility
Insoluble, soluble with NH4 +, alkali metal cations
35
Vapor pressure and temperature trend
Vapor pressure increases, temperature increases
36
Vapor pressure and IMF trend
Vapor pressure increases, IMF decreases
37
Vapor pressure and boiling point trend
Vapor pressure increases, boiling point decreases
38
IMF and heat of vaporization trend
IMF increase, heat of vaporization increases
39
Does temperature change during a phase change?
No
40
Volatile
Easy to evaporate
41
Boiling point
Liquid vapor pressure = external pressure
42
Normal boiling point
Vapor pressure = 1 atm
43
IMF and enthalpy of vaporization trend
IMF increases, enthalpy decreases
44
Dynamic equilibrium
Rate of vaporization = rate of condensation
45
IMF and viscosity trend
IMF increases, viscosity increases
46
IMF and surface tension trend
IMF increases, surface tension increases
47
Large contact between molecules means
Strong attraction
48
Each type of cubic cell will have one or more of these
Corners composed of 1/8 of an atom, edges composed of 1/4 of an atom, faces composed of 1/2 of an atom, centers composed of 1 atom
49
Simple cubic cell unit number of atoms in the cell
1 atom
50
Simple cubic unit cell radius as it relates to length (a)
a = 2r
51
Simple cubic unit cell cooodination number
6
52
Body centered cubic unit number of atoms in the cell
2 atoms
53
Body centered cubic unit radius as it rates to length (a)
a = 4r / Square root 3
54
Body centered cubic unit coordination number
8
55
Face centered cubic unit number of atoms in the cell
4 atoms
56
Face centered cubic unit radius as it relates to the length (a)
a = 4r / Square root 2
57
Face centered cubic unit coordination number
12
58
Worst packing efficiency cell unit type
Simple cubic cell unit because there is only 1 atom in the cell
59
Best packing efficiency cell unit type
Face centered cubic unit because there are 4 atoms per cell
60
Ionic solids
cation and anion held by ionic bonds, high melting points, hard, insulators, conduct electricity when dissolved in liquid
61
Examples of ionic solid
MgCl2, NaCl, KF
62
Lattice energy
energy of formation of a solid crystalline ionic compound from component ions in the gas phase
63
Charge and lattice energy trend
Charge increases, lattice energy increases
64
Distance and ion-ion strength trend
Distances decreases, ion-ion strength increases
65
Effects of greater ion-ion attraction
Melting point increases, boiling point increases, heat of fusion increases, heat of vaporization increases, vapor pressure decreases
66
Ion-dipole
result of electron interference between ion and partial charges on polar molecule
67
Ion-induced dipole
Temporary dipole created due to influence of neighboring ion
68
Dipole-induced dipole
Temporary created due to influence of neighboring dipole (permanent dipole from polar molecule)
69
Induced means
Nonpolar
70
Lowest melting point with ion-ion interactions
Lowest charge and lowest distance (left and down on periodic table)
71
Molecular solids lattice
neutral atoms with discrete covalently bonded molecules at their lattics
72
Are molecular solids polar or nonpolar?
Can be both
73
Properties of molecular solids
Low melting points and mostly soft, insulators that do not conduct electricity
74
Molecular solid examples
CO2, H2, S, I2, H2O, C4H10
75
Atomic solids lattice
Have atoms at their lattices, metallic and network solids, variable
76
Metallic solids definition
Atomic, formed by metal atoms held together by metallic bonds
77
Metallic solids properties
Variable melting points, variable hardness, malleable, shiny, and ductile, conduct heat and electricity very well
78
Metallic solids examples
Cu, Pb, Ni
79
Network solids definition
Atomic solid, made of up covalent bonds of elements of electronegative atoms and viewed as one giant molecule
80
Network solids properties
Very high melting points, very hard, do not conduct electricity or heat, insulators
81
Network solids examples
SiC, SiO2, and diamond (C)
82
If negative slope in phase diagram... (WATER)
Density of solid is less than density of liquid
83
Polarizability increases
<- and down a group
84
At higher altitudes, the boiling point of water would be
less than 100C
85
Temperature and viscosity trend
Increase in temperature, increase in viscosity
86
Temperature and surface tension trend
Increase in temperature, increase in surface tension
87
Capillary action occurs when
Cohesive forces are weaker than adhesive
88
Intramolecular versus intermolecular
Intramolecular is within, and intermolecular is between (intra in CH4 is covalent bond, inter in CH4 is london dispersion)
89
Packing efficiency of cubic unit cells
Increases with decrease in empty space (simple- 52%, body- 68%, face- 74%)
90
Density and volume formulas of simple unit cell
d=2r, v=d^3, v=8r^3
91
Density formula for simple unit cell
Density = (molecular weight x 1/6.022x10^23 x 1 atom) / 8r^3
92
Lattice energy increases with
smaller size and increase charge
93
Lowest boiling point means weak or strong attraction
Weak (small charge and big size = low boiling point)
94
Rate of reaction small letters
Balanced molar coefficient
95
In rate of reaction, reactants have a positive or negative in the equation
Negative, A = 1/a x -Change in M A / Change in time
96
For most reactions, as temperature increases, rate
Rate will also increase
97
Units of rate constant K
M^1-(x+y+z) / s (x+y+z is the sum of order exponents)
98
Slow reaction determines
Rate of reaction
99
Four factors that influence rate
Concentration of reactants, frequency factor, activation energy, temperature
100
As concentration of reactants increases
Number of collisions increases, temperature increases, and reaction rate increases
101
Frequency factor
Number of molecular obstructions
102
As obstruction increases
Frequency factor decreases, constant K increases, overall reaction rate decreases
103
Activation energy
Minimum energy to make reaction
104
Activation energy decreases
More molecules have enough energy, reaction rate increases
105
When temperature increases (reaction rate)
Kinetic energy increases, more molecules with enough energy, more successful reactions, more molecular velocity, more frequent collisions, increased reaction rate
106
Unimolecular
One molecule (use coefficients)
107
Arrhenius equation
ln k = ln A - Ea / RT
108
What is A in Arrhenius equation
Collision frequency and molecular orientation
109
When activation energy increases (temperature)
It is more sensitive to temperature
110
Intermediates
Created but not used in the end
111
In endothermic reaction when temperature increases (free energy)
Free energy decreases
112
Does entropy increase or decrease with dissolving?
Increase
113
Diamond v graphite entropy
Diamond is less than graphite
114
In a spontaneous reaction, Change in free energy
Is negative
115
First order reaction equation
ln (|A|) = -kt + ln([A0])
116
The half-life for a first-order reaction will always be independent of
The concentration
117
First order reaction Half Life
(Half Life) t1/2 = 0.693 / k
ln 2 = 0.693
118
Plot of ln [A] versus time will produce what kind of line with a first order reaction?
A straight line with slope = -k
119
Second order reaction equation
1 / [A] - 1 / [A0] = kt
120
Half life second order reaction equation
(Half Life) t/12 = 1 / k[A0]
121
The half-life for a second order equation will always be
Dependent on concentration
122
If you increase the initial concentration, the half life
Will shorten
123
First-order reaction plot y axis
ln (concentration)
124
Second-order reaction plot y-axis
1 / concentration
125
A plot of 1 / [A] will produce what kind of line in second order?
A straight line with slope = k
126
Zero-order reaction equation
[A] = [A0] - kt
127
Zero-order reaction half-life equation
(Half Life) t1/2 = [A0] / 2k
128
The half-life for a zero-order reaction will always
Be dependent on concentration
129
If you increase the initial concentration, the half-life
Will lengthen
130
Zero-order reaction equation plot y-axis
Concentration
131
A plot [A] will produce what line in a zero-order reaction?
A straight line with slope = -k
132
Collision Theory
The number of collisions between molecules per second is proportional to the reaction rate
133
As concentration of reactants increases, the initial rate will
Increase
134
As concentration of reactants increase, frequency of collisions
Increases
135
As temperature of reaction increases, reaction rate
Increases, the number of reactant molecules with enough energy to undergo chemical reactions will increase
136
As temperature increases, occurrence of correct molecular orientations
Increases, and reaction rate increases
137
If activation energy (Ea) is low
Energy to react is low and more molecules will have enough energy to react
138
Decreasing activation energy will
Increase reaction rate
139
Reactants on coordinate diagrams
Far left
140
Products on coordinate diagram
Far right
141
Transition states on coordinate diagram
Peaks, activated complex
142
Transition state corresponds to
The molecules associated with the reactants having the correct orientation and energy to react although they have yet to react
143
Intermediates on coordinate diagram
Local minima
144
Number of reaction steps on coordinate diagram
Number of transition states
145
Activated energy in coordinate diagram
Energy between reactant and corresponding transition state
146
Change in enthalpy on coordinate diagram
Difference in energy between reactants and products (endo is +, exo is -)
147
Enzyme catalysts and activation energy
Will lower activation energy and result in the reaction occurring much quicker than it would have
148
Enzyme catalysts will alter
Kinetics but not alter the thermodynamics
149
As frequency factor increases, the rate constant
Increases
150
What combination of activation energy and temperature will increase rate constant
Low activation energy and high temperature
151
Elementary mechanistic step in fast equilibrium
The rate of forward = rate of reverse
152
Equation showing rate of forward = rate of reverse
A2 -> 2B
Rate (forward) = kf [A2]
Rate (reverse) = kr [B]^2
kr [B]^2 = kf [A2]
153
Catalyst versus reaction intermediate
Catalyst: consumed in earlier step and regenerated in equal amount in later step
Reaction intermediate: formed in earlier step and consumed in equal amount in later step
154
From (s) to (l)
Attractive forces are broken
155
Energy is what from high to low order
Added
156
Reverse reactions change what
Thermicity, read from right to left rather than left to right
157
Activation energy is from
reactions to transitions state
