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Chemistry 1040 - NSULA Fall 2016 > Chapter 11 - Liquids and Intermolecular Forces > Flashcards

Chapter 11 - Liquids and Intermolecular Forces Flashcards

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1
Q

Define condensed phases.

A

solid and liquid states of matter

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2
Q

What is the fundamental difference between states of matter?

A

the strength of the intermolecular forces of attraction

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3
Q

List five characteristics of gas.

A
  • assumes both volume and shape of its container
  • expands to fill its container
  • is compressible
  • flows readily
  • diffusion within a gas occurs rapidly
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4
Q

List five characteristics of liquid.

A
  • assumes shape of portion of container it occupies
  • does not expand to fill its container
  • is virtually incompressible
  • flows readily
  • diffusion within a liquid occurs slowly
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5
Q

List five characteristics of solids.

A
  • retains own shape and volume
  • does not expand to fill its container
  • is virtually incompressable
  • does not flow
  • diffusion within a solid occurs extremly slowly
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6
Q

How does kinetic energy compare to the energy of attraction for gas?

A

kinetic energies&raquo_space; energies of attraction

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7
Q

How does kinetic energy compare to the energy of attraction for liquids?

A

comparable kinetic energies and energy of attraction

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8
Q

How does kinetic energy compare to the energy of attraction for solids?

A

energies of attraction&raquo_space; kinetic energies

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9
Q

List five physical properties that reflect intermolecular forces.

A

boiling point, melting point, viscosity, surface tension, capillary action

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10
Q

The attractions between molecules are (stronger/weaker) then the intermolecular attractions that hold compounds together.

A

weaker

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11
Q

List the four types of molecular forces from strongest to weakest.

A
  • dispersion forces
  • dipole-dipole forces
  • hydrogen bonding
  • ion-dipole forces
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12
Q

What two types of intermolecular forces are referred to collectively as van der Waals forces?

A

dispersion forces, dipole-dipole forces

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13
Q

Which type of intermolecular force is a special type of dipole-dipole force?

A

hydrogen bonding

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14
Q

Define polarizability.

A

the tendency of an electron cloud to distort

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15
Q

What three factors affect the amount of dispersion force in a molecule?

A
  • the number of electrons in an atom
  • the size of the atom or molecule (molecular weight)
  • shape of molecules with similar masses
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16
Q

How does the number of electrons in an atom affect the amount of dispersion force in a molecule?

A

more electrons = more dispersion force

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17
Q

How does the shape of molecules with similar masses affect the amount of dispersion force in a molecule?

A

more compact = less dispersion force

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18
Q

What is the relationship between polarizability and boiling point?

A

If something is easier to polarize, it has a lower boiling point. This means less intermolecular force.

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19
Q

Explain dipole-dipole interactions.

A

Polar molecules have a more positively charged end and a more negatively charged end, collectively referred to as a dipole. The oppositely charged ends attract each other.

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20
Q

On what molecules do dipole-dipole interactions have a greater effect then dispersion forces?

A

molecules of comparable side and shape

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21
Q

On what molecules do dispersion forces have a greater effect then dipole-dipole interactions?

A

molecules with significant differences in size

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22
Q

Define hydrogen bonds.

A

an attraction between a hydrogen atom attached to a highly electronegative atom and a nearby small electronegative atom in another molecule or chemical group

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23
Q

What is unusual about the dipole-dipole interactions when H is bonded to N, O, or F?

A

they are unusually stong

24
Q

What forms hydrogen bonds?

A

Hydrogen bonding arises in part from the high electronegativity of nitrogen, oxygen, and flourine. These atoms interact with a nearly bare nucleus (which contains one proton).

25
Q

Where are ion-dipole interactions found?

A

in solutions of ions

26
Q

What makes it possible for ionic substances to dissolve in polar solvents?

A

the strength of ion-dipole interactions

27
Q

Define viscosity.

A

the resistance of a liquid to flow

28
Q

How is viscosity affected by intermolecular forces?

A

Viscosity increases with stronger intermolecular forces and decreases with higher temperature.

29
Q

Define surface tension.

A

extra inward forces on the surface of a liquid

30
Q

Define cohesive forces.

A

intermolecular forces that bind similar molecules to one another

31
Q

Define adhesive forces.

A

intermolecular forces that bind a substance to a surface

32
Q

Define capillary action.

A

the rise of liquids up narrow tubes due to adhesive and cohesive forces

33
Q

Define phase change.

A

conversion from one state of matter to another

34
Q

List three phase changes.

A
  • melting/freezing
  • vaporizing/condensing
  • subliming/depositing
35
Q

Define heat of fusion.

A

the energy required to change a solid at its melting point to a liquid

36
Q

Define heat of vaporization.

A

the energy required to change a liquid at its boiling point to a gas

37
Q

Define heat of sublimation.

A

the energy required to change a solid directly to a gas

38
Q

Define heating curve.

A

a plot of temperature verses heat added

39
Q

Define heat within a phase.

A

the produt of specific heat, sample mass and temperature change

40
Q

The temperature of the substance (does/does not) rise during a phase change.

A

does not

41
Q

Define heat during phase changes.

A

the product of mass and the heat of fusion of vaporization

42
Q

Define critical temperature.

A

the temperature beyond which a gas cannot be compressed

43
Q

Define critical pressure.

A

the pressure needed to compress the liquid at critical temperature

44
Q

Define supercritical fluid.

A

the state beyond critical temperature

45
Q

What does gas do when pressure is applied?

A

it liquefies

46
Q

Define boiling point.

A

the temperature at which a liquid’s vapor pressure equals its atmospheric pressure

47
Q

Define normal boiling point.

A

the temperature at which a liquid’s vapor pressure is 760 torr

48
Q

Define vapor pressure.

A

the pressure of a vapor in contact with its liquid or solid form

49
Q

What relationship does the Clausius-Clapeyron equation quantify?

A

the natural log of the vapor pressure of a liquid is inversely proportional to its temperature

50
Q

Define phase diagram.

A

a graph of pressure verses temperature for a substance

51
Q

What information does a phase diagram convey?

A

melting, boiling, and sublimation points at different pressures, the triple point and the critical point

52
Q

Define liquid crystals.

A

the intermediate state that some substances experience between solid and liquid state that has some traits of solids and some of liquids

53
Q

Define nematic liquid crystals.

A

liquid crystal in which the molecules are only ordered in one dimension along the long axis

54
Q

Define smetic liquid crystals.

A

liquid crystal in which molecules are ordered in two dimensions, along the long axis and in layers

55
Q

Define cholesteryic liquid crystals.

A

liquid crystals in which nematic-like crystals are layered at angles to each other

Chemistry 1040 - NSULA Fall 2016 (8 decks)

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