Chapter 11 key terms Flashcards

1
Q

As temperature decreases, what happens to particles?

A

they get closer together

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2
Q

What 5 physical properties reflect intermolecular forces?

A

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

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3
Q

Types of intermolecular bonds from weakest to strongest?

A

Dispersion forces, dipole-dipole forces, hydrogen bonding, ion dipole

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4
Q

How is a dispersion force created?

A

a nonpolar particle can be temporarily polarized to create a dispersion force

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5
Q

What 3 factors determine how strong the dispersion force is?

A
  1. number of electrons(more electrons, more dispersion force)
  2. size of atom or molecule/molecular weight(more compact, more dispersion force)
  3. shape of molecules with similar masses(more compact, less dispersion force)
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6
Q

Do molecules with lower boiling points have weaker or stronger intermolecular forces?

A

weaker

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7
Q

When do dipole-dipole interactions occur?

A

in polar molecules

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8
Q

For molecules of approximately equal mass and size, the more polar the molecule, the higher or lower its boiling point?

A

higher

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9
Q

Which has a greater effect: Dipole-dipole interactions or dispersion forces?

A

-if two molecules are of similar size and shape, dipole-dipole will most likely be the dominating force
-if one molecule is significantly larger than another, dispersion forces will likely determine its physical properties

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10
Q

What are ion-dipole forces?

A

found in solutions of ions
-strength of these forces is what makes it possible for ionic substances to dissolve in polar solvents, like water

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11
Q

What is viscosity?

A

resistance of a liquid to flow

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12
Q

What 8 liquid properties are affected by intermolecular forces?

A

boiling point, melting point, viscosity, surface tension, capillary action, heats of vaporization, heats of fusion

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13
Q

When does viscosity increase?

A

with stronger intermolecular forces

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14
Q

When does viscosity decrease?

A

with higher temperature

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15
Q

What is a phase change?

A

conversion from one state of matter to another

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16
Q

What happens to energy in a phase change?

A

Its either added(endothermic) or released(exothermic)

17
Q

What are the 3 pairs of phase changes?

A

melting/freezing, vaporizing/condensing, subliming/depositing

18
Q

What phase changes are endothermic?

A

melting/fusion, vaporization, sublimation

19
Q

What phase changes are exothermic?

A

condensation, freezing, deposition

20
Q

What is the heat of fusion?

A

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

21
Q

What is the heat of vaporization?

A

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

22
Q

What is the heat of sublimation?

A

the energy required to change a solid directly to a gas

23
Q

During a phase change does temperature of the substance change?

A

NO, which means melting point and boiling point also don’t change

24
Q

In a heating curve, what is the enthalpy change (heat, q) the product of?

A

its the product of the mass or moles and the heat of fusion or vapoization

25
Q

What is a heating curve?

A

a graph of temperature versus heat

26
Q

What do the horizontal lines of a heating curve represent?

A

one for melting and one for vaporization
-horizontal because temp doesn’t change

27
Q

What is a supercritical fluid?

A

the state of a gas beyond the critical temperature

28
Q

What is critical temperature?

A

the temperature beyond which a gas cannot be compressed

29
Q

What happens to most gases when pressure is applied?

A

they liquify

30
Q

What is critical pressure?

A

the pressure needed to compress the liquid at a critical temperature

31
Q

What is vapor pressure?

A

the state of dynamic equilibrium between liquid molecules evaporating and vapor molecules condensing

32
Q

When does the boiling point of a liquid occur?

A

its the temperature at which the vapor pressure equals the atmospheric pressure

33
Q

What is the relationship between pressure and temperature?

A

inverse

34
Q

What is a phase diagram?

A

graph showing states of matter under conditions of temperature and pressure

35
Q

What happens at the triple point?

A

all phases are present

36
Q

What happens at the critical point?

A

supercritical fluid