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chemistry exam 1 Flashcards

1
Q

Which IM force is this? F2 boils at 85k, but Cl2 boils at 238k.

A

Dispersion

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2
Q

Which IM force is this? Xe is liquid at 120k, but Ar is gas.

A

Dispersion

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3
Q

Which IM force is this? Ch3OH boils at 65k but CH3SH boils at 6k.

A

H bond

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4
Q

Which IM force is this? Acetone boils at 65k, but 2-methylpropane boils at -12.

A

dipole dipole

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5
Q

What happens if gas is under high pressure?

A

Inc of IM forces, and molecules are closer together, so it can transform to liquid and even solid.

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6
Q

Why does increase in temp cause transformation of solid to liquid to gas?

A

By adding energy, endothermic reaction

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7
Q

Which IM force operates only with Hydrogen atom of a polar bond with a nearby small electronegative atom?

A

H bond.

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8
Q

Which type of IM force operates only with polar molecules?

A

Dipole Dipole

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9
Q

Which ion force operates between all molecules?

A

London dispersion

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10
Q

Acetones IM force is _________ bc of its _______

A

dipole dipole, permanent dipole

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11
Q

Larger the atom, the more polarizeable (t/f)

A

true

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12
Q

For molecules of same mass, dispersion force increases as polarizeability increases (t/f)

A

true

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13
Q

Dispersion factors between linear molecules are greater than dispersion forces between spherical molecules (t/f)

A

true

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14
Q

dipole dipole are always larger than dispersion (t/f)

A

false. sometimes w bigger molecule, its dispersion force is stronger.

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15
Q

For molecules w/ varying molecular weight, dispersion forces may not become stronger as molecules become more polarizable (t/f)

A

true. polarizability increases with size.

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16
Q

How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in solids?

A

The average kinetic energy of molecules is less than the average energy of attraction between molecules.

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17
Q

How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in liquids?

A

The average kinetic energy of molecules is approximately equal to the average energy of attraction between molecules.

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18
Q

How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in gases?

A

The average kinetic energy of molecules is greater than the average energy of attraction between molecules.

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19
Q

Which type of intermolecular attractive force operates between all molecules?

A

London dispersion forces

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20
Q

Which type of intermolecular attractive force operates only between polar molecules?

A

dipole-dipole forces

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21
Q

Dispersion force inc as ______ inc

A

mw

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22
Q

Surface tension and temperature are

A

inversely related

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23
Q

Viscosity and temperature are

A

inversely related

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24
Q

Substances with high surface tension also tend to have high viscosities since both are related to the

A

strength of IM forces

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25
Q

The weaker the intermolecular forces in a molecule, the greater its…

A

volatility

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26
Q

increasing molecular weight is the opposite of

A

increasing volatility

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27
Q

Covalent bonding occurs in both molecular and covalent-network solids. Which of the following statements best explains why these two kinds of solids differ so greatly in their hardness and melting points?

A

The molecules in molecular solids are held together by weak intermolecular interactions.

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28
Q

Is Si
a molecular, metallic, ionic, or covalent-network solid?

A

Si
is a covalent-network solid.

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29
Q

Silicon readily reacts to form silicon dioxide, SiO2
, which is quite hard and is insoluble in water. Is SiO2
most likely a molecular, metallic, ionic, or covalent-network solid?

A

SiO2
is a covalent-network solid.

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30
Q

Which element or elements are alloyed with gold to make white gold used in the jewelry industry?

A

Ni,Pd

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31
Q

Indicate what type of alloy is formed for white gold.

A

substitutional alloy

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32
Q

Which element or elements are alloyed with gold to make rose gold used in the jewelry industry?

A

Cu

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33
Q

Indicate what type of alloy is formed for rose gold.

A

substitutional alloy

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34
Q

Which element or elements are alloyed with gold to make blue gold used in the jewelry industry?

A

In

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35
Q

Indicate what type of alloy is formed for blue gold.

A

intermetallic compounds

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36
Q

Which element or elements are alloyed with gold to make green gold used in the jewelry industry?

A

Ag

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37
Q

Indicate what type of alloy is formed for green gold.

A

substitutional alloy

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38
Q

Intermetallic compounds have a fixed composition. (t/f)

A

true

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39
Q

Copper is the majority component in both brass and bronze. (t/f)

A

true

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40
Q

In stainless steel, the chromium atoms occupy interstitial positions. (t/f)

A

false

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41
Q

Substitutional alloys tend to be more ductile than interstitial alloys. (t/f)

A

true

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42
Q

Nonmetallic elements are never found in alloys.(t/f)

A

false

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43
Q

Interstitial alloys tend to form between elements with similar ionic radii. (t/f)

A

false

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44
Q

Substitutional alloys are solid solns, but interstitial alloys are heterogenous alloys (t/f)

A

false

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45
Q

The atomic radii of atoms in a substitutional alloy are similar to each other, but in an interstitial alloy, the interstitial atoms are a lot smaller than the host lattice atoms (t/f)

A

true

46
Q

Subs alloys have solute atoms that replace solvent atoms in a lattice but interstitial alloys have…

A

solute atoms that are in between the solvent atoms in a lattice

47
Q

Aluminum metal crystallizes in a face-centered cubic unit cell.
-How many Aluminum atoms are in a unit cell?
-What is the coordination number of each Aluminum atom?
-Calculate the density of Aluminum metal.

A

-4 atoms

-12

-2.71

48
Q

What type of IM Force is CCl4 in benzene C6H6?

A

dispersion

49
Q

What type of IM Force is CH3OH in water?

A

H bonding

50
Q

What type of IM Force is NaBr in water?

A

Ion dipole

51
Q

What type of IM Force is NF3 in CH3CN?

A

dipole dipole

52
Q

An ionic compound has a very negative ΔHsoln
in water.
-Would you expect it to be very soluble or nearly insoluble in water?
-Which term would you expect to be the largest negative number: ΔHsolvent, ΔHsolute, or ΔHmix
-

A

-very soluble
-h mix

53
Q

Glycerol and water have which IM Forces

A

dip dip, h bond, dispersion

54
Q

N2O4 (g) –> 2NO2 (g)
what is the rate law for forward and reverse rxns?
what is k eq?

A

forward: kf[N2O4]
reverse: kf[NO2]^2
keq: [NO2]^2 / [N2O4]

55
Q

kp=…

A

Kp = Kc (RT) ^delta n (change in mols)

56
Q

If K»1, ______
If K «1, ______

A

-rxn favors products
-rxn favors reactants

57
Q

Rxn quotients of heterogenous eq do not include conc of…

A

pure liquids or pure solids

58
Q

Which compound has highest bp?
H2O, H2S, H2Se, H2Te

A

H2O

59
Q

In liquids, the attractive IM Forces are…

A

strong enough to hold molecules close together, but not strong enough to keep molecules from moving past each other

60
Q

As gas elements condense, the atoms become_____ and they have _____ attraction for one another

A

closer together, more

61
Q

Which combination of KE and IM forces result in a formation of a solid?

A

KE is much less than IF

62
Q

Which property is not effected by IM Forces?
bp, color, mp, viscosity

A

color

63
Q

Which has lowest bp?
CH3OH , H2S. , NH3, HCl , CH4

A

CH4

64
Q

Which interaction must be overcome for water to evaporate?

A

H bonding

65
Q

To form hydrogen bond, what must the non hydrogen atom possess?

A

must have a non bonding electron pair

66
Q

How is energy involved in deposition related to those for condensation and freezing?

A

its magnitude is equal to the sum of condensation and freezing

67
Q

The difference between amorphous solids and crystalline solids is that…

A

crystalline solids have repeating lattice patterns

68
Q

which of these is not a type of cubic unit cell?
primitive, corner centered, body centered, face centered

A

corner centered.

69
Q

the type of element whose properties are explained by band theory

A

metalloids

70
Q

which of these substances has the weakest IM force
sucrose (table sugar),, NaCl, diamond, Iron

A

sucrose

71
Q

Ionic solids have _____ attractions

A

electrostatic

72
Q

metallic solids have _______

A

delocalized electrons

73
Q

molecular solids have ______

A

dispersion , dip dip, ion dip, h bond

74
Q

metals are….

A

malleable, ductile, good conductors

75
Q

Computers are made from…

A

semi conductors

76
Q

Nanotubes can be made from …

A

Carbon

77
Q

n type has :
p type has :

A

more ve-
less ve-

78
Q

a material is super conducting if…

A

it conducts with no resistance

79
Q

is deltaHmix bigger or smaller than deltaHsolute+solvent when its an exothermic soln?

A

deltaHmix is smaller , heat is being given out in products

80
Q

if an aq soln is dilute….

A

its molality will be same as molarity

81
Q

molality formula

A

mol solute / kg of solvent

82
Q

rate of rxn can inc by..

A

add heat, add catalyst, inc conc

83
Q

If we know that a rxn is elementary…

A

then we know its rate law

84
Q

in a rxn, species produced in early step and consumed in later step is

A

intermediate

85
Q

in a rxn, species on the reactant side initially that is consumed in an early step and regenerated later is a

A

catalyst

86
Q

if the value of equilibrium constant is large then ______ will mostly be present at eq

A

products

87
Q

if the value of eq constant is small than ______ will mostly be present at eq

A

reactants

88
Q

the eq constant expression depends on the _______ of the rxn

A

stoichiometry

89
Q

CO2 + H2 <—-> CO + H2O if all are gases and CO2 is removed, the CO at equilibrium will…

A

decrease

90
Q

CO2 + H2 <—–> CO + H2O inc temp of this endo rxn will _______ CO at equilibrium

A

increase

91
Q

reaction rate is the change in the amount of __________ over time

A

products or reactants

92
Q

3 factors effecting rate of rxn

A

physical state of reactants
conc of reactants
presence of a catalyst

93
Q

for reaction A + B —->C and Rate = k[B]^2…
if A is doubled, will the rate constant change?
what is the order of A and B?

A

no
0, 2

94
Q

what are units for rate constant

A

M^-1s^-1

95
Q

K = C + ___

A

273

96
Q

E on calc is

A

x 10^flip sign

97
Q

mass %

A

mass / total mass *100

98
Q

mole fraction

A

mol / total mol

99
Q

grams to kg

A

divide grams by 1000

100
Q

mL to L

A

divide mL by 1000

101
Q

1/2 life =

A

ln(2) / K

102
Q

density of water

A

1 gram / mL !!!

103
Q

collision formula

A

K = A * e ^ -Ea/ RT. (a=collison)

104
Q

x % by mass …

A

means x grams in 100g soln

105
Q

ln K2/ K1 ….

A

ln K2 / K1 = Ea/R * 1/T1 - 1/T2

106
Q

n t equation….

A

nt = n0 e ^ -kt. (nt is final mol n0 is initial mol)

107
Q

how to solve rate of combustion

A

look at coefficents, base on that . water vapor is H value

108
Q

ppb

A

-conc of x*10^-9
-mult by mass of soln, to get mass of element.

109
Q

% by mass

A

mass / total mass *100
** assume 1 L of soln

110
Q

quadratic

A

-b +/- sqrt of b^2-4ac all over 2a

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