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Chem two exam one

Total questions: 104

Worksheet time: 57mins

Name
Class
Date
1.

Indicate the strongest intermolecular force in each molecule

1.HCL

2.F2

3.CO

4.HF

a)

  1. 1. dispersion

  2. 2. hydrogen bonding

  3. 3. dipole-dipole

  4. 4. hydrogen bonding

b)

  1. 1. dipole-dipole

  2. 2. dipole-dipole

  3. 3. dispersion

  4. 4. dipole-dipole

c)

  1. 1. dipole-dipole

  2. 2. dispersion

  3. 3. dipole-dipole

  4. 4. hydrogen bonding

d)

  1. 1. dispersion

  2. 2. dipole-dipole

  3. 3. dispersion

  4. 4. dipole-dipole

2.


Choose the pair of substances most likely to form a
homogeneous mixture.

a)

KCl and Hg

b)

NaI and C6H14

c)

C3H8 and C2H5OH

d)

F2 and PF3

e)

NH3 and CH3OH

3.

How much energy in joules does it take to heat 50.0g of water
at 100 ºC to 120 ºC? Cs(liquid) = 4.18 j/g·ºC Cs(gas) = 2.01 j/g
ºC ∆Hvap = 40.7 kJ/mol

a)

115 kJ

b)

1150kJ

4.

What phase changes, if any, would occur in
Order if this substance was at 0 ºC and 300 atm
and then keeping the temperature constant
the pressure was dropped down to 2 atm?

a)

Evaporation

b)

Melting

c)

Evaporation followed by Melting

d)

Melting followed by Evaporation

5.

What is the edge length of a basic cubic lattice cell in relation to
the atomic radius?

(a)  

6.


Identify the network covalent solid

a)

Cl2(s)

b)

Rn(s)

c)

CH4(s)

d)

SiO2(s,quartz)

7.

Identify the metallic solid

a)

Xe(s)

b)

KBr(s)

c)

Zr(s)

d)

CO2(s)

8.


Which substance would have the lowest melting point?
• Cl2(s), Kr(s), C3H8(s), SiO2(s,quartz)

a)

Cl2(s)

b)

Kr(s)

c)

C3H8(s)

d)

SiO2(s,quartz)

9.

Place the following compounds in order of decreasing strength of intermolecular forces.

 

  1. CH3CH2CH2CH2CH2CH3          II.  (CH3)3CCH2CH3         III.  (CH3)2CHCH2CH2CH3

a)

I > III > II

b)

II > III > I

c)

III > II > I

d)

I > II > III

10.

Identify the term used to describe the resistance of liquid to flow.

a)

density

b)

viscosity

c)

surface tension

d)

capillary action

11.

How much energy is required to vaporize 45.4 g of ethanol (C2H5OH) at its boiling point, if its ΔHvap is 40.5 kJ/mol?

a)

27.8 kJ

b)

51.1 kJ

c)

39.9 kJ

d)

18.9 kJ

12.

What is the strongest intermolecular force present in CH3CH2CH2OH?

a)

hydrogen bonding

b)

dipole-dipole

c)

ion-dipole

d)

dispersion forces

13.

How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C?  The following physical data may be useful.

ΔHvap = 40.7 kJ/mol

Cliq = 4.18 J/g∘C

Cgas = 2.01 J/g∘C

Csol = 2.09 J/g∘C

Tmelting = 0∘C

Tboiling = 100∘C

a)

91.7 kJ

b)

87.7 kJ

c)

63.5 kJ

d)

52.7 kJ

14.

According to the phase diagram of CO2 below.  If we started at 4 atm and 190 K and kept the pressure constant but increased the temperature to 217K what process would occur?

a)

melting

b)

evaporation

c)

freezing

d)

sublimation

15.
a)

Triple Point

b)

Vapor Pressure Curve

c)

Sublimation Point

d)

Critical Point

16.

What type of cubic lattice cell has a coordination number of 8?

a)

face centered cubic

b)

basic cubic

c)

cubed cubic cube

d)

body centered cubic

17.

What is the volume of a single lattice cell in cubic centimeters for an atom with a radius of 151 pm that forms a face centered cubic cell. 

Because webcourses wont' let you put an exponent into the numerical answer put just the value for the blank portion (a)   x 10-23

18.

What type of solid is palladium?

a)

ionic solid

b)

metallic atomic solid

c)

network covalent solid

d)

nonbonding atomic solid

19.

  1. Which of these forms hydrogen bonds?

a)

  1. HF

b)

  1. CH3CO2H

c)

  1. Br

d)

  1. CH3OH

e)

  1. CH3OCH3

20.

  1. Ethanol, CH3CHOH, has a vapor pressure of 59mmHg at 25 degrees C. What quantity of energy as heat is required to evaporate 125mL of the alcohol heat at 25 degrees C? The enthalpy of vaporization of the alcohol at 25 degrees C is 42.32kJ/mol. The density of the liquid is 0.7849g/mL

  2. Answer in kJ



(a)  

21.

  1. Higher boiling point?

  2. O2 or N2

a)

O2

b)

N2

22.

  1. Higher boiling point?

  2. SO2 or CO2

a)

SO2

b)

CO2

23.

  1. Higher boiling point?

  2. HF or HI

a)

HF

b)

HI

24.

  1. Higher boiling point?

  2. SiH4 or GeH4

a)

SiH4

b)

GeH4

25.

  1. Rank in order of increasing enthalpy of vaporization

  2. a. CH3OH

  3. b. C2H6

  4. c. HCl

a)

  1. C2H6 < HCl < CH3OH

b)

HCl<CH3OH<C2H6

c)

CH3OH<C2H6<HCL

26.

  1. Rank the following in order of increasing boiling point:

  2. a. CH3CH2CH2CH2CH3

    b. CH3F

    c. CH3Cl

a)

CH3CI<CH3F<CH3CH2CH2CH2CH3

b)

CH3CH2CH2CH2CH3 < CH3Cl < CH3F

27.

  1. Calcium metal crystallizes in a face-centered cubic unit cell. The density of the solid is 1.54 g/cm3. What is the radius of the calcium atom?



(a)  

28.

Which statement is true?

a)

Ideal gases mix because mixing decreases their potential energy

b)

Ideal gases mix because mixing increases their potential energy

c)

Ideal gases mix because mixing decreases their entropy

d)

Ideal gases mix because mixing increases their entropy

29.

If the solvent-solute interactions in a mixture are comparable in strength to the solvent-solvent interactions and the solute solute interactions, what can you conclude about solution formation in this mixture?

a)

  1. A homogeneous solution forms.

b)

  1. A homogeneous solution does not form.

c)

  1. The formation of a homogeneous solution is uncertain.

30.

The forces between ionic compounds and polar compounds are known as __________ forces.

a)


dispersion

b)


dipole-dipole

c)

hydrogen bonding

d)

ion-dipole

e)

ionic

31.

In a liquid the tendence of liquids to minimize their surface area is calle

a)

Viscosity

b)

Surface Tension

c)

Vapor Pressure

d)

Capillary Action

e)

Hydrogen Bonding

32.

Which of the following has the smallest dipole-dipole forces (having none would also be considered
the smallest)?

a)


HI

b)


CH3CH2Cl

c)

F2

d)

CO

e)

all are the same

33.

Identify the compound that does NOT have hydrogen bonding

a)


NH3

b)

HF

c)

H2O

d)

CH3(CH2)3NH2

e)


CH3CH2F

34.

Ammonia (NH3) has a higher normal boiling point than its heavier congener PH3. Which is the best
explanation for this difference

a)


NH3 is trigonal pyramidal and polar while PH3 is trigonal planar and nonpolar

b)

NH3 is more acidic than PH3

c)


NH3 experiences stronger dispersion forces than PH3

d)


NH3 has extensive hydrogen bonding while PH3 does not.

35.

Choose the substance with the HIGHEST vapor pressure at a given temperature

a)

AsH3

b)

CH3OCH2CH3

c)


RbBr

d)

SiO2

e)

BH3

36.

Determine the vapor pressure (in mm Hg) of a substance at 29°C, whose normal boiling point is 76°C
and has a ΔHvap of 38.7 kJ/mol.

a)

48 mm Hg

b)

21 mm Hg

c)


13 mm Hg

d)

96 mm Hg

e)

80 mm Hg

37.

A student collected multiple data points relating the temperature and pressure of a substance. She then
plotted 1/T vs. ln P and obtained a straight-line plot with a slope of -3101. What is the ∆Hvap of the
substance?

a)


4.78 kJ

b)

3000 kJ

c)

8.314 kJ

d)

25.78 kJ

e)


not enough information

38.
a)


I only

b)

II only

c)

both I and II

d)


neither I or II

39.

Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4 from 35.0°C to gaseous
CCl4 at 76.8°C (the normal boiling point for CCl4). The specific heat of CCl4(l) is 0.857 J/(g ∙ °C) its heat
of fusion is 3.27 kJ/mol and its heat of vaporization is 29.82 kJ/mol.

a)

0.896 kJ

b)

5.74 kJ

c)

6.28 kJ

d)

1.43 kJ

e)

7.45 kJ

40.

Identify the characteristics of a body-centered cubic cell

a)

1 atom inside, coordination # of 6

b)

1 atom inside, coordination # of 8

c)


2 atom inside, coordination # of 6

d)

4 atom inside, coordination # of 12

e)

2 atom inside, coordination # of 8

41.

A metal crystallizes in a face centered cubic structure and has a density of 8.90 g/cm3. If the radius
of the metal atom is 125 pm, what is the identity of the metal?

a)

At

b)

Fe

c)

Pd

d)

Cr

e)

Co

42.

Which of the following forms a molecular solid?

a)

C10H22

b)

Silver

c)


NH4NO3

d)


C, diamond

e)

all of the above

43.
a)

b)

c)

d)

44.
a)

-650 kJ/mol

b)


+650 kJ/mol

c)


+690 kJ/mol

d)

-690 kJ/mol

e)

-710 kJ/mol

45.
a)


AA

b)


AB

c)

ABC

d)

all of the above

e)


none of the above

46.

Which of the following compounds will be MOST soluble in nonane (C9H20)?

a)


CH3CH2OH

b)

CH3(CH2)3CH2OH

c)


CH3COCH2CH3

d)


CH3COOH

e)

C6H6

47.

Which of the following elements would you add to germanium to make an n-type semiconductor?

a)

phosphorous

b)

silicon

c)


gallium

d)

arsenic

e)

both A and D

48.

Choose the correct order of increasing band gaps

a)

Conductor < Insulator < Semiconductor

b)


Insulator < Conductor < Semiconductor

c)

Semiconductor < Conductor < Insulator

d)

Conductor < Semiconductor < Insulator

49.

Dynamic equilibrium can be defined as ___________

a)


rate of dissolution > rate of recrystallization

b)


rate of concensing > rate of bubbling

c)


rate of dissolution < rate of recrystallization

d)

rate of dissolution = rate of recrystallization

e)


rate of bubbling > rate of dissolving

50.

Determine the IMF in this element or compound

Xe

a)

dispersion

dipole-dipole

H-bonding

ion-dipole

b)

dispersion

dipole-dipole

c)

dispersion

d)

dispersion

dipole-dipole

H-bonding

51.

what IMF does HF have increasing strength

(all lowercase)

(a)  

52.

what IMF does NF3 have increasing strength

(all lowercase)

(a)  

53.

what IMF does SiBr4 have increasing strength

(all lowercase)

(a)  

54.

what IMF does Cl2 have increasing strength

(all lowercase)

(a)  

55.

what IMF does PCl3 have increasing strength

(all lowercase)

(a)  

56.

what IMF does HI have increasing strength

(all lowercase)

(a)  

57.

Arrange these compounds in order of increasing boiling point.

a.CH4

b.CH3CH3

c.CH3CH2Cl

d.CH3CH2OH

a)

b,d,a,c

b)

a,b,c,d

c)

d,c,b,a

d)

d,a,c,b

58.

Which one has the higher boiling point?

a)

NH3

b)

CH4

59.

Which one has the higher boiling point?

a)

CH3OCH3

b)

CH3CH2OH

60.

Which one has the higher boiling point?

a)

CO2

b)

NO2

61.

At the same temperature, which has the higher vapor pressure?

a)

Br2

b)

I2

62.

At the same temperature, which has the higher vapor pressure?

a)

H2S

b)

H2O

63.

At the same temperature, which has the higher vapor pressure?

a)

NH3

b)

PH3

64.

Does this pair of compounds form a homogeneous solution when combined?

CCl4 and H20

a)

homogeneous

b)

not homogeneous

65.

Does this pair of compounds form a homogeneous solution when combined?

KCl and H20

a)

not homogenous

b)

homogenous

66.

Does this pair of compounds form a homogeneous solution when combined?

Br2 and CCl4

a)

homogenous

b)

not homogenous

67.

Does this pair of compounds form a homogeneous solution when combined?

CH3CH2OH and H2O

a)

homogenous

b)

not homogenous

68.

Which compound would you expect to have greater surface tension?

a)

acetone

(CH3)2CO

b)

Water

H20

69.

Which compound would be expected to have the greater viscosity?

a)

Compound A

b)

Compound B

70.

Identify each solid as molecular, ionic, or atomic

Br2 (s), CO2 (s), Cu (s), CaBr2 (s)

a)

ionic, covalent, molecular, atomic

b)

molecular, molecular, atomic, ionic

c)

atomic, ionic, molecular molecular

d)

molecular, atomic, molecular, covalent

71.

Which solid has the highest melting point?

a)

Ar (s)

b)

CCl4 (s)

c)

LiCl (S)

d)

CH3OH (s)

72.

Which solid has a higher melting point?

a)

TiO2 (s)

b)

HOOH (s)

73.

Which solid has a higher melting point?

a)

CCl4 (s)

b)

SiCL4 (s)

74.

Which solid has a higher melting point?

a)

Kr (s)

b)

Xe (s)

75.

Which solid has a higher melting point?

a)

NaCl (s)

b)

CaO (s)

76.

  1. list melting points in decreasing order: (C(s diamond), Kr (s), Nacl (s), H20 (s))

a)

C(s diamond)>H20 (s)>Nacl (s)>Kr (s)

b)

Kr (s)>C(s diamond)>H20 >Nacl (s)

c)

C(s diamond)>Nacl (s)>H20 (s)>Kr (s)

d)

Nacl (s)>H20 (s)>Kr (s)> C(s diamond)

77.

Categorize the crystalline solid

SiC

a)

Nonbonding

b)

Network Covalent

c)

Metallic

d)

Ionic solids

e)

Molecular solids

78.

Categorize the crystalline solid

HBr

a)

Nonbonding

b)

Molecular

c)

Metallic

d)

Network Covalent

e)

Ionic

79.

Categorize the crystalline solid

Cu

a)

Molecular

b)

Metallic

c)

Ionic

d)

Network covalent

e)

nonbonding

80.

Categorize the crystalline solid

Br2

a)

ionic

b)

molecular

c)

nonbonding

d)

covalent

81.

NH4ClO3

a)

molecular

b)

metallic

c)

Ionic

d)

covalent

82.

How many moles of iron are in one face centered cubic lattice cell?

a)

6.642x10^-24 mol

b)

7.542x10^-38 mol

c)

6.642x10^-22 mol

d)

7.54x10^-36 mol

83.

Find the Delta H of Hydration

Delta H of solution= -50.5 kJ

Delta H of solute= +510 kJ

a)

560.5 kJ

b)

675.5 kJ

c)

-560.5 kJ

d)

-675.5 kJ

84.

A solution is saturated in both nitrogen gas and potassium bromide at 75 degrees celsius. When the solution is cooled to room temperature, what is most likely to happen?

a)

Some nitrogen gas bubbles out of the solution

b)

Some potassium bromide precipitates out of the solution

c)

Some nitrogen gas bubbles out of the solution, and some potassium bromide precipitates out of the solution

d)

Nothing happens

85.

On a Phase diagram, the vaporization curve is between

a)

a solid and a gas

b)

a solid and a liquid

c)

a liquid and a gas

d)

two solids

86.

A student collected multiple data points relating the temperature and pressure of a substance. She then plotted 1/T vs. ln P and obtained a straight-line plot with a slope of -6101. What is the delta H of vaporization. of the substance?

a)

4.78 kJ

b)

67.35 kJ

c)

8.314 kJ

d)

25.78 kJ

e)

50.72 kJ

87.

Identify the element with the largest band gap

a)

lead

b)

silicon

c)

germanium

d)

carbon

e)

tin

88.

Identify the characteristics of a basic cubic cell

a)

1 atom inside, coordination number of 6

b)

2 atom inside, coordination number of 8

c)

2 atom inside, coordination number of 6

d)

1 atom inside, coordination number of 8

e)

1 atom inside, coordination number of 12

89.

Define solubility

a)

A solid that does not dissolve in a gas

b)

the amount of a substance that will dissolve in a given amount of solvent

c)

the amount of a substance that will dissolve in a given amount of solute

d)

a solid mixed with another solid

e)

a liquid that does not dissolve in another liquid

90.

Which of the following statements is TRUE

a)

Intermolecular forces are generally stronger than bonding forces

b)

The potential energy of molecules decreases as they get closer to one another

c)

Energy is given off when the attraction between two molecules is broken

d)

Increasing the pressure of a solid usually causes it to become a liquid

e)

None of the above is true

91.

For Benzene (C6H6) the normal boiling point is 80.1 degrees Celsius and the enthalpy of vaporization is 30.8 kJ/mol. What is the boiling point of benzene at Mt Whitney where atmospheric pressure is 456 torr?

a)

337 K

b)

347 K

c)

4.20 K

d)

353 K

e)

371 K

92.

Arrange the following in order of decreasing melting point

CH3OCH3, CH3CH2CH3, CH3CH2OH

a)

CH3OCH3>CH3CH2CH3>CH3CH2OH

b)

CH3OCH3>CH3CH2OH>CH3CH2OH

c)

CH3CH2OH>CH3CH2CH3>CH3OCH3

d)

CH3CH2OH>CH3OCH3>CH3CH2CH3

93.

A portion of the phase diagram for UF6 is shown. Which statements are correct?

a)

UF6 evaporates at atmospheric pressure.

b)

At 40 degrees celsius and 2 atm, UF6 (g) is the predominant phase.

c)

both of the statements

d)

neither of the statements

94.

How much energy must be removed from a 125g sample of benzene (molar mass= 78.11g/mol) at 425.0 K to liquify the sample and lower the temperature to 335 K? The following physical data may be useful.

T melting= 279 K, T boiling= 353 K

a)

38.9 kJ

b)

95.4 kJ

c)

67.7 kJ

d)

74.4 kJ

95.

Place the following substances in order of decreasing vapor pressure at a given temperature.

NaCl CH3OH OF2

a)

CH3OH>OF2>NaCl

b)

NaCl>OF2>CH3OH

c)

OF2>CH3OH>NaCl

d)

OF2>NaCl>CH3OH

e)

NaCl>CH3OH>OF2

96.

A metal crystallizes in a body centered cubic structure and has a density of 7.87 g/cm^3. If the radius of the metal atom is 124 pm, what is the identity of the metal?

a)

At

b)

Fe

c)

Pd

d)

Cr

e)

Co

97.

Which of the following forms a molecular solid?

a)

CaCl2

b)

Au

c)

C (s graphite)

d)

HCl

e)

Fe

98.

Define sublimation

a)

the phase transition from solid to gas

b)

the phase transition from gas to solid

c)

the phase transition from gas to liquid

d)

the phase transition from liquid to gas

e)

the phase transition from liquid to solid

99.

Naval brass is 60.5% copper, 37.5% zinc, 1.8% tin and 0.7% lead. Identify the solute(s) in this alloy

a)

copper

b)

tin

c)

zinc

d)

lead

e)

tin, zinc, and lead

100.

Arrange the following in order of increasing boiling point (lowest to highest)

Ne,Xe,Kr

a)

Xe<Kr<Ne

b)

Ne<Kr<Xe

c)

Ne<Xe<Kr

d)

Kr<Ne<Xe

e)

Kr<Xe<Ne

101.

Identify the type of interaction between atoms in a nonbonding atomic solid

a)

polar bonding

b)

ionic bonding

c)

covalent bonding

d)

hydrogen bonding

e)

weak dispersion forces

102.

Which of the following elements would you add to germanium to make an n-type semiconductor

a)

indium

b)

silicon

c)

gallium

d)

arsenic

e)

both indium and arsenic

103.

Choose the pair of substances most likely to form a homogenous mixture

a)

KCl and Hg

b)

NaI and C6H14

c)

NH3 and CH3OH

d)

C3H8 and C2H5OH

104.

Which solid would you expect to have the highest melting point?

a)

H2O

b)

Li (s)

c)

CH3CH2OH (s)

d)

Ar (s)

e)

Ne (s)

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