Chemistry ch. 11-13 Exam Study Flashcards


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Exam study for ch. 11-13, Dr. Wanda Jones CH-202.
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1

BEGINNING OF CH. 11

BEGINNING OF CH. 11 (back of card)

2

Crystalline solids ________.

have ordered structures

3

________ liquid crystals are colored because the molecular layers are arranged in slightly twisted planes with respect to one another.

Cholesteric

4

What are the common types of smectic liquid-crystalline phases?

A and C

5

There are ________ types of smectic liquid-crystalline phases.

3

6

For a given substance that exhibits liquid-crystalline properties, the transition from solid to liquid-crystal state occurs ________.

at the melting point of the solid

7

In liquids, the attractive intermolecular forces are ________.

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

8

As a gaseous element condenses, the atoms become ________ and they have ________ attraction for one another.

closer together, more

9

Together, liquids and solids constitute ________ phases of matter.

the condensed

10

The strongest interparticle attractions exist between particles of a ________, and the weakest interparticle attractions exist between particles of a ________.

solid, gas

11

________ are particularly polarizable.

Large molecules, regardless of their polarity,

12

The ease with which the charge distribution in a molecule can be distorted by an external electrical field is called the ________.

polarizability

13

Elemental iodine (I2) is a solid at room temperature. What is the major attractive force that exists among different I2 molecules in the solid?

London dispersion forces

14

Hydrogen bonding is a special case of ________.

dipole-dipole attractions

15

________ is the energy required to expand the surface area of a liquid by a unit amount of area.

Surface tension

16

Which statements about viscosity are true?

(i) Viscosity increases as temperature decreases.
(ii) Viscosity increases as molecular weight increases.
(iii) Viscosity increases as intermolecular forces increase.

All of the above.

17

The shape of a liquid's meniscus is determined by ________.

the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and its container

18

Viscosity is ________.

the resistance to flow

19

The property responsible for the "beading up" of water is ________.

surface tension

20

Heat of sublimation can be approximated by adding together ________ and ________.

heat of fusion, heat of vaporization

21
card image

A-B solid
B-C solid and liquid
C-D liquid
D-E liquid and gas
E-F gas

The ________ (is)are associated with the heat energy being used up to increase distances between molecules.

phase changes B → C and D → E

22

Large intermolecular forces in a substance are manifested by ________.

high heats of fusion and vaporization
high boiling point
low vapor pressure
high critical temperatures and pressures

23

Of the following, ________ is an exothermic process.

freezing
subliming
melting
boiling

freezing

24

A volatile liquid is one that ________.

readily evaporates

25

In general, the vapor pressure of a substance increases as ________ increases.

temperature

26

The vapor pressure of any substance at its normal boiling point is ________.

1 atm

27

Volatility and vapor pressure are ________.

directly proportional to one another

28

On a phase diagram, the critical pressure is ________.

the pressure required to liquefy a gas at its critical temperature

29

On a phase diagram, the critical temperature is ________.

the temperature above which a gas cannot be liquefied

30

On a phase diagram, the melting point is the same as ________.

the freezing point

31

BEGINNING OF CH. 12

BEGINNING OF CH. 12 (back of card)

32

A solid has a very high melting point, great hardness, and poor electrical conduction. This is a(n) ________ solid.

covalent network

33

Trends in melting points for metals can be explained with the ________.

electron-sea model

34

The ________ for Ge shows it to be a semiconductor, because the gap between the filled lower and empty higher energy bands is relatively small.

molecular-orbital model

35

All of the following are a type of solid except ________.

metallic
supercritical
ionic
covalent network
molecular

supercritical

36

Consider the following statements about crystalline solids:

(i) Molecules or atoms in molecular solids are held together via ionic bonds.
(ii) Metallic solids have atoms in the points of the crystal lattice.
(iii) Ionic solids have formula units in the point of the crystal lattice.
(iv) Molecules in covalent-network solids are connected via a network of covalent bonds.

Which of the statements is true?

(ii)

37

The ________ of light waves upon passing through a narrow slit is called diffraction.

scattering

38

What fraction of the volume of each corner atom is actually within the volume of a face-centered cubic unit cell?

1/8

39

What portion of the volume of each atom or ion on the face of a unit cell is actually within the unit cell?

1/2

40

________ have properties that depend on the manner in which the solid is formed.

Heterogeneous alloys

41

________ are examples of homogeneous alloys.

Intermetallic compounds

42

________ generally differ from compounds in that the atomic ratios of the constituent elements in the former are ________ and may vary over a wide range.

Alloys, not fixed

43

Of the following, ________ may be added to steel to modify its properties.

carbon and nickel

44

How many valence electrons do inorganic compounds contain if they are considered semiconductors?

4

45

All of the following are natural polymers except ________.

nylon

46

The empirical formula of an addition polymer ________.

is the same as that of the monomer from which it is formed

47

What happens to a polymer as it becomes more crystalline?

Its yield stress decreases.
Its density decreases.
Its melting point decreases.
Its stiffness decreases.

None of the above is correct.

48

Natural rubber is too soft and chemically reactive for practical applications. ________ of natural rubber entails crosslinking reactive polymer chains with sulfur atoms.

Vulcanization

49

The formation of a ________ polymer generally involves the elimination of a small molecule.

condensation

50

All of the following are classified as a nanomaterial except ________.

buckminsterfullerene
carbon nanotubes
isoprene
graphene

All of the above are classified as nanomaterials.

51

The properties of graphene include ________.

high strength
large thermal conductivity
a zero energy gap

All of the above.

52

BEGINNING OF CH. 13

BEGINNING OF CH. 13 (back of card)

53

Hydration is a specific example of the phenomenon known generally as ________.

solvation

54

Pressure has an appreciable effect on the solubility of ________ in liquids.

gases

55

The phrase "like dissolves like" refers to the fact that ________.

polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes

56

In a saturated solution of a salt in water, ________.

the rate of crystallization = the rate of dissolution

57

An unsaturated solution is one that ________.

has a concentration lower than the solubility limit

58

A solution with a concentration higher than the solubility allows is ________.

supersaturated

59

Molality is defined as the ________.

moles solute/kg solvent

60

Which one of the following concentration units varies with temperature?

Molality.
Mole fraction.
Mass percent.
Molarity.

Molarity.

61

The magnitudes of Kf and of Kb depend on the identity of the ________.

solvent

62

As the concentration of a solute in a solution increases, the freezing point of the solution ________ and the vapor pressure of the solution ________.

decreases, decreases

63

The ratio of the actual value of a colligative property to the value calculated, assuming the substance to be a nonelectrolyte, is referred to as ________.

the van't Hoff factor

64

Colligative properties of solutions include all of the following except ________.

an increase in the osmotic pressure of a solution upon the addition of more solute

the increase of reaction rates with increase in temperature

elevation of the boiling point of a solution upon addition of a solute to a solvent

depression of vapor pressure upon addition of a solute to a solvent

depression of the freezing point of a solution upon addition of a solute to a solvent

the increase of reaction rates with increase in temperature

65

The process of a substance sticking to the surface of another is called ________.

adsorption (not absorption)

66

All of the following are considered to be colloids except ________.

a foam
an emulsion
a homogeneous mixture
an aerosol
All of the above are colloids.

a homogeneous mixture

67

Hydrophobic colloids ________.

can be stabilized by adsorption of ions

68

END

Good luck on the exam!

END (back of card)