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General chemistry II > Unit 2 (ch 12,18,14) > Flashcards

Unit 2 (ch 12,18,14) Flashcards

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1
Q

mixture of solid metals

A

alloys

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2
Q

Use alloys to…

A

alter and improve properties of individual metals

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3
Q

Metallic bonds consist of (blank)

A

shared electron pools

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4
Q

Describe metallic bond

Are electrons easy or hard to pull away?

A

valence orbitals overlap with neighbors to give delocalized electron pool
-easy

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5
Q

What happens when more metal ions bind together?

A

End up with a band of valence and/or conduction energy levels (valence and conduction bands)

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6
Q

Semiconductors principle/explanation

A

valence and conduction bands are separated by a band gap, which varies in energy depending on compounds

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7
Q

larger band gaps =

A

higher energy between the two bands, harder for electrons to move between them

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8
Q

structures of metals

A

different, highly ordered ways that atoms can arrange to give a layer organization of metals

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9
Q

What are unit cells?

A

smallest repeating units, stack together to form crystalline structure

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10
Q

Dimensions of the unit cells are determined by

A

packing of atoms

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11
Q

length of cubic

A

2r

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12
Q

BCC radius

A

0.4330 times length

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13
Q

FCC radius

A

0.3536 times length

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14
Q

Alloys

A

different atoms either substitute or fit between the originals

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15
Q

interstitial alloys

A

new atoms fit between the regular ones

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16
Q

What type of hole has the most space?

A

cubic

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17
Q

What is the ratio equation for the holes?

A

r guest/ r host

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18
Q

What is the cubic holes ratio?

A

0.73-1.00

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19
Q

NaCl is a compound where (blank) holes are filled by

A

octahedral, Na+ ions

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20
Q

1st law of thermodynamics

A

energy not created nor destroyed, just transferred

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21
Q

to determine the spontaneity of a process, we look at

A

entropy of system, surroundings, and universe

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22
Q

2nd law of thermodynamics

A

energy wants to spread out

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23
Q

Spontaneous means

A

no input is needed for the process to occur- doesn’t always happen fast

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24
Q

microstates represent

A

unique arrangements of different options/states

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25
Q

by moving to areas of greater heat/energy or larger volumes, what happens?

A

more microstates are accessible and entropy increases

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26
Q

molecules have three types of motion/freedom- they are?

A

vibrational, translational, rotational

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27
Q

at lower temperatures, how does this affect microstates?

A

fewer accessible microstates, less energy to access more of them

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28
Q

colder things will spontaneously do what?

A

absorb energy from warmer ones- ice will melt, because liquid water has greater entropy

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29
Q

what processes are isothermal?

A

melting/freezing and boiling/condensation

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30
Q

define isothermal

A

energy goes to breaking molecules apart or bringing them together

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31
Q

What does it mean to be a state function? Example?

A

route from initial to final doesn’t matter, only change and entropy

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32
Q

delta S system =

A

delta S final- delta S initial

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33
Q

delta S system =

A

qrev/T (K)

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34
Q

q=

A

heat that can leave or enter a system from the surroundings

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35
Q

what are forward and reverse processes?

A

melting and freezing are equal and opposite

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36
Q

for a process to be spontaneous, delta S univ must be

A

positive

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37
Q

delta S universe =

A

delta S system + delta S surroundings

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38
Q

Why does ice melt or water freeze spontaneously?

A

changes in temp give differences in the entropy for otherwise equal and opposite systems

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39
Q

dissolving a solid or diluting a solution is (blank)

A
  • spontaneous
  • solute molecules gain more freedom/disorder by entering system, even if some of the solvent molecules become slightly more ordered
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40
Q

interstitial

A

nonhost fills holes in host

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41
Q

substitutional

A

host replaced with non-host

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42
Q

types of substititutional

A

heterogeneous- clumps

homogeneous- random, even distribution

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43
Q

solids are usually composed of

A

mix of elements

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44
Q

alloy

A

mixture of metals with the goal of improving the properties of metals (stronger, corrosion resistant, conductive)

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45
Q

what are a few examples of common alloys?

A 
Brass (cu and zn)
Stainless steel (Fe and Cr)
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46
Q

metallic bond

A

shared pool of electrons where atoms are densely packed and valence orbitals overlap

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47
Q

band theory explains what?

A

sea of electrons

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48
Q

molecular orbits form

A

valence band

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49
Q

Are metals good conductors?

A

yes

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50
Q

semiconductors

A
  • electronics
  • valence and conduction bands separated by gap
  • less energy by shifting atoms
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51
Q

doping semiconductors changes (blank)

A

band gap

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52
Q

if an element gives extra electrons it (blank)

A

raises valence bond

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53
Q

if an element gives holes- missing electrons it (blank)

A

lowers conduction band

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54
Q

if the element gives extra electrons it is known as the

A

n type (extra negative)

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55
Q

if the element gives holes, it is known as the

A

p type (extra positive)

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56
Q

no current means there is

A

no electron flow and electrons stuck in valence bond

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57
Q

current means there is

A

electron flow and electrons move from valence to conduction band

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58
Q

structures of metals

A

metal atoms can solidify in highly ordered “crystalline lattice”

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59
Q

hexagonal close packed (HCP) has what type of layering?

A

ababab

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60
Q

cubic close packed (CCP) has what type of layering?

A

abcabcabc and each atom touches 12 atoms

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61
Q

what type of cells have the densest packing?

A

HCP and CCP 74%

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62
Q

packing efficiency

A

volume of atoms/volume of cell x 100

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63
Q

Cubic

A

layers just stack on top of each other (52%)

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64
Q

What type of layer does cubic have?

A

aaaaaa

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65
Q

What type of layering does body centered cubic have?

A

ababab- 68%

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66
Q

unit cell dimensions are determined by what?

A

packing of atoms

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67
Q

simple cubic unit cell

A

length- 2r
one atom per unit cell
1 corner atom per unit cell

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68
Q

body centered cubic unit cell

A

length- r= 0.4330l
two atoms per unit cell
1 full in middle, 1 corner

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69
Q

face centered cubic

A

length- r= 0.2526l
4 atoms per unit cell
3 face, 1 corner

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70
Q

alloys

A

mixture of different metals

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71
Q

subsitutional alloy

A

-new metal atoms take place of original

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72
Q

3 types of subsitutional alloys

A

homogeneous
heterogeneous
intermetallic

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73
Q

homogeneous

A

randomly but evenly distributed

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74
Q

heterogeneous

A

clumps or groups of replaced atoms

75
Q

intermetallic

A

uniform composition and stoichiometry

76
Q

alloys can make metals

A

harder (harder for atoms to slide past each other)

77
Q

interstitial alloy

A

host stays in pattern and holes are filled with other atoms

78
Q

types of holes

A

tetrahedral
octahedral
cubic

79
Q

tetrahedral

A

smaller, 4 host atoms, FCC and HCC

80
Q

octahedral

A

larger FCC and HCC

81
Q

cubic

A

middle of simple cube and when filled looks like BCC

82
Q

radius of host: other RATIO

A

r other/ r host

83
Q

what is the ratio for tetrahedral?

A

0.2:0.4

84
Q

what is the ratio for octahedral?

A

0.4:0.7

85
Q

what is the ratio for cubic?

A

0.7:1.0

86
Q

if there is little carbon, the substance is often

A

malleable

87
Q

metals are described as

A

cations in sea of electrons

88
Q

what are the types of nonmental cystals?

A

covalent network
molecular solids
ionic solids

89
Q

covalent network

A

solids held together by covalent bonds (e- sharing)

90
Q

what forms network covalent solids?

A

C bonds

91
Q

C-C bonds form

A

allotropes

92
Q

diamond formation

A

4 covalent bonds, carbon (STRONG)

93
Q

graphite formation

A

3 covalent bonds-carbon held together with dispersion

94
Q

fullerenes

A

soccer ball shaped carbon bonds

95
Q

molecular solids

A

molecular held together with imf

range from H bonds and DD (H2O/ice) to ID weak forces holding solid together (CO2, O2S8)

96
Q

ionic solids

A

cation and anion, ion-ion force

  • bigger ion is in crystal lattice and one in hole
  • maintain strict stoichiometric ratio
  • ordered structure
97
Q

Why don’t ionic solids have alloys?

A

strict pattern and structure

98
Q

solid, inorganic compound which has been heated

A

ceramic

99
Q

what are common ceramics?

A

Si and SiO2 (silica)

100
Q

amorphous solid

A

obsidion, no crystal lattice or order

101
Q

Superconductors

A

atoms vibrating resist flowage (super cold = vibrating stops)

102
Q

characteristics of metallic solids

A

malleable and breakable

103
Q

characteristics of ionic solids

A

hard and brittle

104
Q

what two types of structures have close packing?

A

HCC and FCC

105
Q

what two types of structures have square packing?

A

BCC and SC

106
Q

HCC stacking pattern

A

abababab

107
Q

FCC/cubic closest packed stacking pattern

A

abcabc

108
Q

BCC stacking pattern

A

ababab

109
Q

SC stacking pattern

A

aaa

110
Q

malleable means

A

easily bent and damaged

111
Q

metallic elements have (blank) electronegatives than nonmetals

A

lower- bonding e not tight

112
Q

(blank) has more valence than host semimetal

A

dopant

113
Q

p type semiconductor

A

dopant has fewer valance electrons than host

114
Q

meissner effect

A

magnet floating above superconducting material

115
Q

1st law of thermodynamics

A

energy not created or destroyed, just transferred

energy allows work

116
Q

spontaneous vs nonspontaneous

A

do or don’t require intervention of some sort

117
Q

2nd law of thermodynamics

A

entropy helps determine spontaneity
energy wants to spread out
universe tends to disorder

118
Q

for a spontaneous process, the entropy of the universe (blank)

A

increases

119
Q

Microstates

A

unique arrangement of things
-arrangement is energy level
deflating tire

120
Q

three types of motion for gas molecules

A

translational, rotational, virbrational

121
Q

Boltzmann distribution

A
  • indiv. molecules might change energy but system stays same

- shows all possible states a molecule can occupy

122
Q

higher temp or greater volume gives (blank)

A

more potential microstates

123
Q

more microstates means

A

increased entropy

124
Q

colder things spontaneously (blank)

A

absorb energy from warmer things

125
Q

melting and boiling processes are (blank)

A

isothermal

126
Q

entropy is a (blank)

A

“state function”

127
Q

what does it mean if something is a “state function”

A

only initial and final states matter

128
Q

delta S system

A

S final - S initial

129
Q

delta S system or entropy for isothermal process

A

q reversible/ T (k)

130
Q

forward and reverse processes are

A

equal

131
Q

S univ =

A

S sys + S surroundings

132
Q

heat transfer to cooler system is

A

spontaneous

133
Q

greater temperature difference =

A

greater entropy change for univ

134
Q

entropy related to dissolving solutes in solvents

A

gain freedom of motion once dissolved

135
Q

dilution process is

A

spontaneous- more disorder

136
Q

3rd law of thermodynamics

A

at 0 K, entropy=0

137
Q

Gibbs free energy

A

delta Hrxn - T(delta S)

138
Q

If G < 0, S univ

A

> 0 spontaneous

139
Q

If G>0, S univ

A

<0 nonspontanous

140
Q

If G = 0

A

no change in system

141
Q 
delta H (-) and delta S (+)
delta G =
spontaneous or nonspontaneous?
A

delta G <0

spontaneous

142
Q 
delta H (-) and delta S (-)
delta G =
spontaneous or nonspontaneous?
A

delta G <0 at lower temp

spontaneous at lower temp

143
Q 
delta H (+) and delta S (+)
delta G =
spontaneous or nonspontaneous?
A

delta G <0 at high temp

spontaneous at high temp

144
Q 
delta H (+) and delta S (-)
delta G =
spontaneous or nonspontaneous?
A

delta G>0

not spontaneous

145
Q

What is the 3rd law of thermodynamics?

A

“perfect” crystalline material at 0 K, entropy = 0

146
Q

What does Gibbs free energy relate?

A

delta S and H sys and the energy available to do work

147
Q

If delta G = <0, delta S univ > 0, spontaneous or nonspontaneous?

A

spontaneous

148
Q

If delta G > 0, delta S univ < 0, spontaneous or nonspontaneous?

A

nonspontanous

149
Q

if delta H is - and delta S is + , delta G is? Spontaneous?

A

always < 0, always spontaneous

150
Q

if delta H is - and delta S is - , delta G is? Spontaneous?

A

< 0 at lower temp, spontaneous at lower temp

151
Q

if delta H is + and delta S is + , delta G is? Spontaneous?

A

< 0 at higher temp, spontaneous at higher temp

152
Q

if delta H is + and delta S is - , delta G is? Spontaneous?

A

always > 0, never spontaneous

153
Q

system becomes colder, q rev is (blank)

A

+ (gaining energy)

154
Q

system becomes hotter, q rev is (blank)

A
  • (losing energy)
155
Q

What is an example of a coupled reaction?

A

delta G can power other reactions that are nonspontaneous- combustion of glucose drives ADP phosphorylation to form ATP

156
Q

kinetics is the study of

A

rates of reactions

157
Q

Describe catalytic converters in cars

A

remove NO

158
Q

production rate is

A

+

159
Q

consumption rate is

A

-

160
Q

slope =

A
  • rate
161
Q

the overall reaction order is the

A

sum of the exponents

162
Q

increased molecules and concentration (blank) rate

A

increases

163
Q

if a line is linear, it is

A

first order

164
Q

pseudo first order

A

one of reactants is way larger than the other so it becomes the only one that matters

165
Q

step 1 is the (blank)

A

slowest

166
Q

rate determining step

A

slowest step

167
Q

if collisions are increased, (blank) increases

A

concentration

168
Q

subscripts tell us what?

A

reaction order

169
Q

overall rate depends on the (blank) in the rate determining step?

A

concentrations

170
Q

1st order reaction in relation to graph

A

if ln(x) vs t is straight line

171
Q

activation energy equation

A

ln (k2)- ln (k1) = Ea/R (1/T2-1/T2)

172
Q

higher Ea =

A

slower reaction

173
Q

if Ea is smaller, reaction is

A

faster

174
Q

if Ea is larger, reaction is

A

slower

175
Q

if the graph starts at higher energy then goes to lower, the reaction is going to be (blank) and delta H is going to be (blank)

A

exothermic, negative

176
Q

if the graph starts at lower energy and goes to higher energy, the reaction is going to be (blank) and delta H is going to be (blank)

A

endothermic, positive

177
Q

how to find slope

A

ln(k1)-ln(k2)/ (1/T1-1/T2)

178
Q

Reaction mechanisms describe what

A

molecularity

179
Q

unimolecular

A

one molecule in rate

180
Q

bimolecular

A

two molecules

181
Q

three molecules

A

ter

182
Q

step 1 is the

A

rate determining step, slow

183
Q

rate laws are determined by

A

the slowest step

General chemistry II (4 decks)

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