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CHEM1212 > TEST 1- CHEM1211 + Ch. 10, 12 > Flashcards

TEST 1- CHEM1211 + Ch. 10, 12 Flashcards

1
Q

2 regions of electron density with 0 lone pairs

A

Linear, linear, 180

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2
Q

2 regions of electron density with 1 lone pair

A

Linear, linear, 180

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3
Q

3 regions of electron density with 0 lone pairs

A

Trigonal planar, trigonal planar, 120

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4
Q

3 regions of electron density with 1 lone pair

A

Trigonal planar, bent, 120

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5
Q

4 regions of electron density with 0 lone pairs

A

Tetrahedral, tetrahedral, 109.5

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6
Q

4 regions of electron density with 1 lone pair

A

Tetrahedral, trigonal pyramidal, 109.5

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7
Q

4 regions of electron density with 2 lone pairs

A

Tetrahedral, bent, 109.5

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8
Q

5 regions of electron density with 0 lone pairs

A

Trigonal bipyramidal, trigonal bipyramidal, 90 or 120

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9
Q

5 regions of electron density with 1 lone pair

A

Trigonal bipyramidal, seasaw, 90 or 120

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10
Q

5 regions of electron density with 2 lone pairs

A

Trigonal bipyramidal, T-shaped, 90 or 120

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11
Q

5 regions of electron density with 3 lone pairs

A

Trigonal bipyramidal, linear, 90 or 120

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12
Q

6 regions of electron density with 0 lone pairs

A

Octahedral, octahedral, 90 or 180

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13
Q

6 regions of electron density with 1 lone pair

A

Octahedral, square pyramidal, 90 or 180

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14
Q

6 regions of electron density with 2 lone pairs

A

Octahedral, square planar, 90 or 180

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15
Q

Always polar

A

Bent, trigonal pyramidal, seesaw, T-shaped, square pyramidal

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16
Q

Not always polar

A

Linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral, square planar

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17
Q

Salts consisting of K+

A

Always soluble

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18
Q

Salts consisting of Na+

A

Always soluble

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19
Q

Salts consisting of NH4+

A

Always soluble

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20
Q

Salts consisting of CH3COO- (acetic acid)

A

Always soluble

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21
Q

Salts consisting of ClO3- and ClO4-

A

Always soluble

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22
Q

Salts consisting of NO3-

A

Always soluble

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23
Q

Salts consisting of Br-

A

Soluble, insoluble with Hg2 2+, Pb 2+ , Ag+

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24
Q

Salts consisting of Cl-

A

Soluble, insoluble with Hg2 2+, Pb 2+ , Ag+

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25
Q

Salts consisting of I-

A

Soluble, insoluble with Hg2 2+, Pb 2+ , Ag+

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26
Q

Salts consisting of F-

A

Soluble, insoluble with Ba 2+, Ca 2+, Pb 2+, Sr 2+, Ag+

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27
Q

Salts consisting of SO4 2-

A

Soluble, insoluble with Ba 2+, Ca 2+, Pb 2+, Sr 2+, Ag+

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28
Q

Compounds with OH-

A

Insoluble, soluble with Ba 2+, K+, Na+

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29
Q

Salts consisting of S 2-

A

Insoluble, soluble with Ba 2+, K+, Na+, NH 4+

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30
Q

Salts consisting of CO3 2-

A

Insoluble, soluble with K+, Na+, NH4+

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31
Q

Compounds consisting of O 2-

A

Insoluble, soluble with Ba+, K+, Na+

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32
Q

Salts consisting of PO4 3-

A

Insoluble, soluble with K+, Na+, NH4+

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33
Q

CrO4 2- solubility

A

Insoluble, soluble with NH4 +, alkali metal cations

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34
Q

C2O4 2- Solubility

A

Insoluble, soluble with NH4 +, alkali metal cations

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35
Q

Vapor pressure and temperature trend

A

Vapor pressure increases, temperature increases

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36
Q

Vapor pressure and IMF trend

A

Vapor pressure increases, IMF decreases

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37
Q

Vapor pressure and boiling point trend

A

Vapor pressure increases, boiling point decreases

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38
Q

IMF and heat of vaporization trend

A

IMF increase, heat of vaporization increases

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39
Q

Does temperature change during a phase change?

A

No

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40
Q

Volatile

A

Easy to evaporate

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41
Q

Boiling point

A

Liquid vapor pressure = external pressure

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42
Q

Normal boiling point

A

Vapor pressure = 1 atm

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43
Q

IMF and enthalpy of vaporization trend

A

IMF increases, enthalpy decreases

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44
Q

Dynamic equilibrium

A

Rate of vaporization = rate of condensation

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45
Q

IMF and viscosity trend

A

IMF increases, viscosity increases

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46
Q

IMF and surface tension trend

A

IMF increases, surface tension increases

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47
Q

Large contact between molecules means

A

Strong attraction

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48
Q

Each type of cubic cell will have one or more of these

A

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

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49
Q

Simple cubic cell unit number of atoms in the cell

A

1 atom

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50
Q

Simple cubic unit cell radius as it relates to length (a)

A

a = 2r

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51
Q

Simple cubic unit cell cooodination number

A

6

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52
Q

Body centered cubic unit number of atoms in the cell

A

2 atoms

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53
Q

Body centered cubic unit radius as it rates to length (a)

A

a = 4r / Square root 3

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54
Q

Body centered cubic unit coordination number

A

8

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55
Q

Face centered cubic unit number of atoms in the cell

A

4 atoms

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56
Q

Face centered cubic unit radius as it relates to the length (a)

A

a = 4r / Square root 2

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57
Q

Face centered cubic unit coordination number

A

12

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58
Q

Worst packing efficiency cell unit type

A

Simple cubic cell unit because there is only 1 atom in the cell

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59
Q

Best packing efficiency cell unit type

A

Face centered cubic unit because there are 4 atoms per cell

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60
Q

Ionic solids

A

cation and anion held by ionic bonds, high melting points, hard, insulators, conduct electricity when dissolved in liquid

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61
Q

Examples of ionic solid

A

MgCl2, NaCl, KF

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62
Q

Lattice energy

A

energy of formation of a solid crystalline ionic compound from component ions in the gas phase

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63
Q

Charge and lattice energy trend

A

Charge increases, lattice energy increases

64
Q

Distance and ion-ion strength trend

A

Distances decreases, ion-ion strength increases

65
Q

Effects of greater ion-ion attraction

A

Melting point increases, boiling point increases, heat of fusion increases, heat of vaporization increases, vapor pressure decreases

66
Q

Ion-dipole

A

result of electron interference between ion and partial charges on polar molecule

67
Q

Ion-induced dipole

A

Temporary dipole created due to influence of neighboring ion

68
Q

Dipole-induced dipole

A

Temporary created due to influence of neighboring dipole (permanent dipole from polar molecule)

69
Q

Induced means

A

Nonpolar

70
Q

Lowest melting point with ion-ion interactions

A

Lowest charge and lowest distance (left and down on periodic table)

71
Q

Molecular solids lattice

A

neutral atoms with discrete covalently bonded molecules at their lattics

72
Q

Are molecular solids polar or nonpolar?

A

Can be both

73
Q

Properties of molecular solids

A

Low melting points and mostly soft, insulators that do not conduct electricity

74
Q

Molecular solid examples

A

CO2, H2, S, I2, H2O, C4H10

75
Q

Atomic solids lattice

A

Have atoms at their lattices, metallic and network solids, variable

76
Q

Metallic solids definition

A

Atomic, formed by metal atoms held together by metallic bonds

77
Q

Metallic solids properties

A

Variable melting points, variable hardness, malleable, shiny, and ductile, conduct heat and electricity very well

78
Q

Metallic solids examples

A

Cu, Pb, Ni

79
Q

Network solids definition

A

Atomic solid, made of up covalent bonds of elements of electronegative atoms and viewed as one giant molecule

80
Q

Network solids properties

A

Very high melting points, very hard, do not conduct electricity or heat, insulators

81
Q

Network solids examples

A

SiC, SiO2, and diamond (C)

82
Q

If negative slope in phase diagram… (WATER)

A

Density of solid is less than density of liquid

83
Q

Polarizability increases

A

<- and down a group

84
Q

At higher altitudes, the boiling point of water would be

A

less than 100C

85
Q

Temperature and viscosity trend

A

Increase in temperature, increase in viscosity

86
Q

Temperature and surface tension trend

A

Increase in temperature, increase in surface tension

87
Q

Capillary action occurs when

A

Cohesive forces are weaker than adhesive

88
Q

Intramolecular versus intermolecular

A

Intramolecular is within, and intermolecular is between (intra in CH4 is covalent bond, inter in CH4 is london dispersion)

89
Q

Packing efficiency of cubic unit cells

A

Increases with decrease in empty space (simple- 52%, body- 68%, face- 74%)

90
Q

Density and volume formulas of simple unit cell

A

d=2r, v=d^3, v=8r^3

91
Q

Density formula for simple unit cell

A

Density = (molecular weight x 1/6.022x10^23 x 1 atom) / 8r^3

92
Q

Lattice energy increases with

A

smaller size and increase charge

93
Q

Lowest boiling point means weak or strong attraction

A

Weak (small charge and big size = low boiling point)

94
Q

Rate of reaction small letters

A

Balanced molar coefficient

95
Q

In rate of reaction, reactants have a positive or negative in the equation

A

Negative, A = 1/a x -Change in M A / Change in time

96
Q

For most reactions, as temperature increases, rate

A

Rate will also increase

97
Q

Units of rate constant K

A

M^1-(x+y+z) / s (x+y+z is the sum of order exponents)

98
Q

Slow reaction determines

A

Rate of reaction

99
Q

Four factors that influence rate

A

Concentration of reactants, frequency factor, activation energy, temperature

100
Q

As concentration of reactants increases

A

Number of collisions increases, temperature increases, and reaction rate increases

101
Q

Frequency factor

A

Number of molecular obstructions

102
Q

As obstruction increases

A

Frequency factor decreases, constant K increases, overall reaction rate decreases

103
Q

Activation energy

A

Minimum energy to make reaction

104
Q

Activation energy decreases

A

More molecules have enough energy, reaction rate increases

105
Q

When temperature increases (reaction rate)

A

Kinetic energy increases, more molecules with enough energy, more successful reactions, more molecular velocity, more frequent collisions, increased reaction rate

106
Q

Unimolecular

A

One molecule (use coefficients)

107
Q

Arrhenius equation

A

ln k = ln A - Ea / RT

108
Q

What is A in Arrhenius equation

A

Collision frequency and molecular orientation

109
Q

When activation energy increases (temperature)

A

It is more sensitive to temperature

110
Q

Intermediates

A

Created but not used in the end

111
Q

In endothermic reaction when temperature increases (free energy)

A

Free energy decreases

112
Q

Does entropy increase or decrease with dissolving?

A

Increase

113
Q

Diamond v graphite entropy

A

Diamond is less than graphite

114
Q

In a spontaneous reaction, Change in free energy

A

Is negative

115
Q

First order reaction equation

A

ln (|A|) = -kt + ln([A0])

116
Q

The half-life for a first-order reaction will always be independent of

A

The concentration

117
Q

First order reaction Half Life

A

(Half Life) t1/2 = 0.693 / k
ln 2 = 0.693

118
Q

Plot of ln [A] versus time will produce what kind of line with a first order reaction?

A

A straight line with slope = -k

119
Q

Second order reaction equation

A

1 / [A] - 1 / [A0] = kt

120
Q

Half life second order reaction equation

A

(Half Life) t/12 = 1 / k[A0]

121
Q

The half-life for a second order equation will always be

A

Dependent on concentration

122
Q

If you increase the initial concentration, the half life

A

Will shorten

123
Q

First-order reaction plot y axis

A

ln (concentration)

124
Q

Second-order reaction plot y-axis

A

1 / concentration

125
Q

A plot of 1 / [A] will produce what kind of line in second order?

A

A straight line with slope = k

126
Q

Zero-order reaction equation

A

[A] = [A0] - kt

127
Q

Zero-order reaction half-life equation

A

(Half Life) t1/2 = [A0] / 2k

128
Q

The half-life for a zero-order reaction will always

A

Be dependent on concentration

129
Q

If you increase the initial concentration, the half-life

A

Will lengthen

130
Q

Zero-order reaction equation plot y-axis

A

Concentration

131
Q

A plot [A] will produce what line in a zero-order reaction?

A

A straight line with slope = -k

132
Q

Collision Theory

A

The number of collisions between molecules per second is proportional to the reaction rate

133
Q

As concentration of reactants increases, the initial rate will

A

Increase

134
Q

As concentration of reactants increase, frequency of collisions

A

Increases

135
Q

As temperature of reaction increases, reaction rate

A

Increases, the number of reactant molecules with enough energy to undergo chemical reactions will increase

136
Q

As temperature increases, occurrence of correct molecular orientations

A

Increases, and reaction rate increases

137
Q

If activation energy (Ea) is low

A

Energy to react is low and more molecules will have enough energy to react

138
Q

Decreasing activation energy will

A

Increase reaction rate

139
Q

Reactants on coordinate diagrams

A

Far left

140
Q

Products on coordinate diagram

A

Far right

141
Q

Transition states on coordinate diagram

A

Peaks, activated complex

142
Q

Transition state corresponds to

A

The molecules associated with the reactants having the correct orientation and energy to react although they have yet to react

143
Q

Intermediates on coordinate diagram

A

Local minima

144
Q

Number of reaction steps on coordinate diagram

A

Number of transition states

145
Q

Activated energy in coordinate diagram

A

Energy between reactant and corresponding transition state

146
Q

Change in enthalpy on coordinate diagram

A

Difference in energy between reactants and products (endo is +, exo is -)

147
Q

Enzyme catalysts and activation energy

A

Will lower activation energy and result in the reaction occurring much quicker than it would have

148
Q

Enzyme catalysts will alter

A

Kinetics but not alter the thermodynamics

149
Q

As frequency factor increases, the rate constant

A

Increases

150
Q

What combination of activation energy and temperature will increase rate constant

A

Low activation energy and high temperature

151
Q

Elementary mechanistic step in fast equilibrium

A

The rate of forward = rate of reverse

152
Q

Equation showing rate of forward = rate of reverse

A

A2 -> 2B
Rate (forward) = kf [A2]
Rate (reverse) = kr [B]^2
kr [B]^2 = kf [A2]

153
Q

Catalyst versus reaction intermediate

A

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
Q

From (s) to (l)

A

Attractive forces are broken

155
Q

Energy is what from high to low order

A

Added

156
Q

Reverse reactions change what

A

Thermicity, read from right to left rather than left to right

157
Q

Activation energy is from

A

reactions to transitions state

CHEM1212 (5 decks)

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