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CHM 142 +145 > CHM 142 final exam > Flashcards

CHM 142 final exam Flashcards

1
Q

rate of dissappearance

reactants

A

-[Concentration of reactants]/change in time

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2
Q

rate of appearance

products

A

[concentration of products]/change in time (s)

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3
Q

the rate of appearance of one molecule—the rate of disappearance of another molecule

A

equals

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4
Q

equation to find rates of change for a reaction

A

-1/a([A]/change in time)=1/b([B]/change in time)

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5
Q

general rate law

A

R= k[A]^x[B]^y

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6
Q

what can affect the value of k (rate constant)

A

temperature

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7
Q

when a reaction depends on a single reactant to the first order

A

first order reactions

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8
Q

integrated rate law (1st order)

A

ln[A]=-kt+ln[A]initial

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9
Q

what does a first order graph look like?

A

linear line

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10
Q

when a reaction depends on one reactant to the 2nd order or two first order reactants

A

second order reaction

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11
Q

integrated rate law (2nd order)

A

1/[A]=kt+1/[A]initial

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12
Q

what does a second order graph look like?

A

a curved line

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13
Q

integrated rate law (0th order)

A

[A]=-kt+[A]initial

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14
Q

what does a zeroth order graph look like?

A

Horizontal line

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15
Q

1st order half life

A

.693/K

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16
Q

2nd order half life

A

1/(K*[A]0)

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17
Q

rate laws relate—and—

A

rate and concentration

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18
Q

integrated rate laws relate—and —

A

time and concentration

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19
Q

the minimum E required to intiate a chemical reaction

A

Activation energy

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20
Q

the higher the value of E the — rate

A

slower

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21
Q

Arrhenius equation

A

k= Ae^(-Ea/RT)

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22
Q

determining the activation E with one rate constant

A

ln(k)=-Ea/RT +ln(A)

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23
Q

determining the activation E with two rate constants

A

ln(k1/k2)=-Ea/R(1/T2-1/T1)

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24
Q

if a reaction has a slow first step what determines the rate of the reaction?

A

the rate law of the slow first step

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25
Q

what is the equation for finding the eq. constant (K)

A

Keq = [D]^d*[C]^c/[A]^a[B]^b

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26
Q

How do you find the equilibrium constant for gases? (Kp)

A

= Kc(RT)^change in n

n = moles gas product= moles gas reactant R =.08206

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27
Q

True or false concentrations of reactants and products have to be the same during equilibrium?

A

false, they have to be stoichiometrically equivalent

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28
Q

If K»1 the reaction favors—

A

the products, lies to the right

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29
Q

If K < 1 the reaction favors—

A

the reactants, lies to the left

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30
Q

If you are perfoming Hess’s law like calculations to find Kp or Keq name some of the differences between doing it originally and doing it with eq constants

A
  • if you need to ‘flip the sign’ dont flip the sign of the value, inverse it (1/x)
  • if you multiply a reaction you put the Keq or Kp to that numer (3x = Keq^3)
  • at the end you multiply the Keqs and Kps together, not add
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31
Q

Are pure solids and liquids included in eq constants?

A

no, their values are 1

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32
Q

Reaction Quotient (Q)

A

calculated like K but concentrations from any point in the reaction can used, not just at eq.

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33
Q

when Q»k the reaction…

A

shifts left

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34
Q

when Q«K the reaction…

A

shifts right

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35
Q

how will the reaction shift if volume is increased?

A

towards the side of the reaction that produces more moles

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36
Q

If heat is added to an exothermic reaction how will the reaction shift?

A

to the left, reactants

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37
Q

If heat is added to an endothermic reaction how will the reaction shift?

A

to the right, to the products

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38
Q

Do catalysts affect the values of Keq

A

no, only how fast it is reached

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39
Q

Buffer

A

a solution that contains an acid and its weak base that has resistance to pH change

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40
Q

Henderson Hasselbalch equation

A

pH=Pka + log [base]/[acid]

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41
Q

When choosing a buffer, choose one with a — about equal to the desired —

A

Pka, pH

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42
Q

If a strong base is titrated with a weak acid is the starting pH high or low?

A

High, strong base has high pH

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43
Q

If a strong acid is titrated with a weak base does the eq point occur just below or just above a pH of 7

A

below, start with a low pH

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44
Q

Does the presence of commmon ions increase or decrease the solubility

A

decrease because the ion will dissolve less than it normally would with a common ion

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45
Q

Do the formation of complex ions increase or decrease solubility?

A

Increase by forming metal ion + lewis base

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46
Q

Metal oxides and hydroxides that are relatively insoluble in water but are soluble in strongly acidic and strongly basic solutions are said to be—

A

Amphoteric

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47
Q

If Q>ksp the solution is —

A

super saturated

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48
Q

If Q<Ksp the solution is—

A

unsaturated

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49
Q

If Q=Ksp the solution is —

A

saturated

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50
Q

Change in Free energy equation

concerning standard gibbs free E

A

standard gibbs free E +RTln(Q)

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51
Q

Change in free energy

enthalpy and entropy

A

Change in H-Tchange in S

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52
Q

transition metal complexes

A

transition metal + ligand

charged = complex ion

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53
Q

ligands

concerning metal complexes

A

bonding molecule to the metal ion
- usually polar or an anion
- must have one pair of unpaired electrons

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54
Q

werners theory

A

every transition metal has a primary valence and a secondary valence

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55
Q

primary valence

A

oxidation state

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56
Q

secondary valence

A

coordination number

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57
Q

why do the transition metals after 6B start to increase in size

A

metallic bonding strength decreases as anitbonding orbitals are filled so it cancels out effective nuclear charge and size increases

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58
Q

Lanthanide contraction

periods 5 and 6

A

this is why we dont see the expected increase in radius size in the second half of the transition metals, the filling of the 4f orbitals decrease radius size

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59
Q

Transition metals lose their — orbitals first

A

S orbitals

then d orbitals

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60
Q

all spins are paired, weakly repulsed in a magnetic field, generally not considerd magnetic

A

diamagnetic

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61
Q

unpaired electrons where the spins are not affected by surrounding atoms, weakly attracted in a magnetic field

A

paramagnetic

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62
Q

ferromagnetism

A
  • stronger than paramagnetism
  • all spins align parallel to the magnetic field
  • create permenant magnet
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63
Q

antiferromagnetism

A
  • unpaired electrons align their spins opposite to adjacent atoms but the magnetic charges cancel out
64
Q

ferrimagnetism

A

unpaired electrons have opposite spins to adjacent ones but the magnetic charge does not cancel out

happens in atoms that have diff number of electrons

65
Q

ferro, ferri, and antiferrimagnetic substances become — when heated above a certain temperature

A

paramagnetic

thermo E cancels out magnetic forces

66
Q

The metal ligand bond happens as a result of —

A

Lewis acid and Lewis base interaction

67
Q

is the ligand the lewis acid or base?

A

lewis base

electron donor

68
Q

is the transition metal the lewis acid or base?

A

lewis acid

electron acceptor

69
Q

Complex formation can change—

A
  • tendency of redution and oxidation
  • color
70
Q

If the coordination number if 4 what is the likely geometry?

A

tetrahedral or square planar

71
Q

if the coordination number is 6 what is the likely geometry?

A

Octahedral

72
Q

anions from strong bases are—

halides

A

neutral

73
Q

cations from strong bases are—

grp I and II

A

neutral

74
Q

anions from weak bases are—

A

basic

75
Q

Transition metals are usually —

A

acidic

76
Q

Spontaneous processes

A

Processes that proceed with no outside assistance

S is positive for spontaneous process

77
Q

Nonspontaneous procsses

A

Processes that require outside assistance to proceed

S is negative for nonspon processes

78
Q

State functions

A

T, H, S, E and G

not q and w

79
Q

Entropy

A

the randomness of a system

80
Q

Entropy =

S

A

qrev/ T

qrev= Enthalpy

81
Q

2nd law of thermodynamics

A

the entropy of the univ increases for any spontaneous process

82
Q

1st law of thermodynamics

A

energy can not be created or destroyed only converted

83
Q

3rd law of thermodynamics

A

Entropy of a substance that is perfectly crystalline (1 m.s.) is 0

84
Q

Entropy =

with microstates

A

k*ln(wfinal/winitial)

k= boltzmans constant 1.38*10^-23

85
Q

Gibbs free E =

standard gibbs value

A

Standard G+RT*ln(Q)

86
Q

gibbs free E =

enthalpy and entropy

A

Change in H - T*Change in S

87
Q

If a reaction is spontaneous should G be negative or positive

A

negative = spon process for G

if G = 0 the system is at eq

88
Q

Donor atom

A

the atom in a ligand that bonds to the metal ion

89
Q

Monodentate

A

has one donor atom, can bind to one coordination site

H20, NH3, CN-, Cl-

90
Q

Bidentate

A

Has two donor atoms, can bind to two donor sites

Carbonate ion, Oxalate, (en) ethylinediamine

91
Q

Polydentate

A

More than two donor atoms, can bind to more than two donor sites

EDTA, Triphosphate ion

92
Q

Prevents reactions with metal atoms by forming a ‘claw’ over them

A

Chelating agents

93
Q

examples of porphyrins

A

Heme, Chlorophyll

94
Q

made of porphine molecules and found in biological systems

A

Porphyrins

95
Q

Heme

A

Porphyrine with Fe (II) as the metal ion

96
Q

Chlorophyll

A

Porphyrin with Mg(II) as the metal ion

97
Q

isomer

A

same chemical formula, different bonds and structures

98
Q

Structural isomer

A

different connections/ bonds of atoms

linkage isomers and coordination sphere isomers

99
Q

linkage isomer

A

the ligand is bound to the metal by different atoms

Ex: NO2 can choose to bond by N or by O

100
Q

Coordination sphere isomer

A

differing atoms within the coordination sphere and outside of it

101
Q

Stereoisomers

A

same bonds but different geometric arragnment

Geometric isomers and enantiomers

102
Q

geometric isomers

cis/trans isomers

A

Bonds on different or same sides of molecule

cis= same side trans= diff side

103
Q

Are geometric isomers found in all geometric arrangments?

A

No they are only found in octahedral or square planar, not tetrahedral

104
Q

enantiomers

optical isomers

A

isomers that are mirror reflections of each other but cannot be superimposed on each other

105
Q

rotates plane of light to the right

A

dextratory enantiomer

106
Q

rotates the plane of light to the left

A

levrortory enantiomer

107
Q

Does not rotate plane of light/ cancels out

A

racemic mixture

108
Q

Electrons flow spontaneously from the — to the —

A

anode to the cathode

109
Q

where oxidation occurs, negative value, loses mass over time

A

anode

110
Q

where reduction occurs, positive value, gains mass over time

A

cathode

111
Q

the more — the emf value is the more likely it is for — to occur

A

positive, reduction or negative, oxidation

112
Q

For a reaction to be spontaneous Ecell needs to be — and G needs to be —

A

positive, negative

113
Q

primary cell

A

cannot be recharged

alkaline (AA AAA)

114
Q

secondary cell

A

can be recharged

Lead acid, Ni-Cd, Li batteries

115
Q

Q=

colombs

A

It=nf

I = amperes t =time n= number of moles of e- f= faradays

116
Q

the color of a transition metal complex depends on — and —

A

the identity of the ligand and identity of the metal ion

117
Q

If an object is perceived as blue what is its wavelength? and what colors of light is it absorbing?

A

wavelength: about 450 nm
absorbed light: orange

118
Q

If an object is perceived as yellow what is its wavelength? and what colors of light is it absorbing?

A

wavelength: 570
absorbed light: purple

119
Q

Magnetic properites of complexes depend on —

A

the number of unpaired electrons in the d orbital

120
Q

the electrostatic field of the ligands interacts with the d orbitals in the metal ion

A

crystal field theory

121
Q

the orbitals that point towards the ligands are the — E orbitals

A

High

122
Q

the orbitals that do not point towards ligands are the— E orbitals

A

Low

123
Q

Ranks a ligands ability to increase crystal splitting E

A

Spectrochemical series

124
Q

The Spectrochemical series

A
  1. Cl-
  2. F-
  3. H2O
  4. NH3
  5. en
  6. NO2-
  7. CN-
125
Q

ligands on the left end/ low end of the spectrochemical series

A

weak field ligands

dont easily increase E (high spin)

126
Q

ligands on the right/ high end of the spectrochemical series

A

strong field ligands

easily increase E between orbitals (low spin)

127
Q

In an octahedral arrangement — is the low E orbitals

A

t2

6 electrons

128
Q

In a octahedral arragnment — is the high E orbtials

A

e

4 electrons

129
Q

in tetrahedrals — is the high E orbitals

A

t2

130
Q

In tetrahedrals — is the low E orbitals

A

e

131
Q

Almost all square planars are — spin

A

low spin

132
Q

Almost all tetrahedrals are — spin

A

high spin

133
Q

High spin complex

A

low field ligand, not a big different in E when placing electrons in orbitals

all orbitals filled then start pairing

134
Q

Low spin comlex

A

high field ligands, big diff in E when placing electrons in orbitals

all in low and then can add to high E orbital

135
Q

Alpha decay

A

emission of 4/2He nucleus

136
Q

Beta decay

A

emission of a High E electron

written 0/-1 e

137
Q

Gamma Decay

A

emits High E photons, does not change proton or neutron value

138
Q

positron emission

A

opposite of beta decay, emitts anti electron

written 0/+1e or +Beta

139
Q

electron capture

A

capture of an electron from the electron field by the nucleus

140
Q

What kind of radiation does an element under go if it is above the belt of stability

A

Beta decay

increase protons, decrease neutrons

141
Q

What kind of radiation does an element under go if it is below the belt of stability?

A

Positron emission or electron capture

increase neutrons

142
Q

Radioactive decay is a — order process

A

first order

143
Q

first order half life

A

t1/2= .693/k

144
Q

ln(Nt/N0)=

Nt= current number of nuclei N0= initial number

A

-kt

145
Q

Change in E=

A

Change in M *c^2

c= speed of light 2.9979*10^8

146
Q

Change in E=

A

Change in M*c^2

c= speed of light 2.9979*10^8

147
Q

Nuclear binding E

A

The amount of E it takes to separate the nucleons of an atom

148
Q

separating heavy nuclei into smaller more stable molecules

A

Fission

our current source of nuclear E

149
Q

Bringing together light/small nuclei into larger more stable ones

A

Fusion

better for E but no materials to withstand rxns

150
Q

Fuel elements

A

fissonable materials

151
Q

Moderator

A

Slow down nuclei so they can actually hit each other

152
Q

control rods

A

absorb nuclei. to keep rxn from over heating

153
Q

primary coolant

A

takes heat away from rxn

154
Q

secondary coolant

A

takes heat from primary coolant away to generate E

155
Q

Is ionized or non ionized radiation more harmful?

A

Ionized radiation is more harmful bc/ it forms free radicals

CHM 142 +145 (6 decks)

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