Chapter 11 Intermolecular Forces and the Liquid State Flashcards

1
Q

Fusion (Melting)

A

solid to liquid; endothermic

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2
Q

Vaporization

A

liquid to gas; endothermic

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3
Q

Sublimation

A

solid to gas; endothermic

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4
Q

Freezing

A

liquid to solid; exothermic

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5
Q

Condensation

A

gas to liquid; exothermic

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6
Q

Deposition

A

gas to solid; exothermic

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7
Q

Enthalpy of Vaporization

A

energy required to convert 1 mole or 1 gram of a liquid to vapor at a given temperature

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8
Q

When the strength of the IMFs in a series of liquids increase, will the enthalpy of vaporization increase or decrease?

A

increase because it will require more energy to break the bonds

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9
Q

Dynamic Equilibrium

A

state in which the rates of vaporization and condensation are equal

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10
Q

What happens to temperature when vapor pressure increases?

A

as temperature increases, vapor pressure increases too

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11
Q

When the strength of the IMFs in a series of liquids increase, will the vapor pressure increase or decrease?

A

decrease because molecules with weaker IMFs are held less tightly to one another in the liquid phase so more of them can escape into the vapor phase

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12
Q

Surface Force

A

measure of force required to break the surface of the liquid

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13
Q

Do liquids with strong IMFs have high or low surface tension?

A

high surface tension

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14
Q

Viscosity

A

measure of a liquid’s resistance to flow

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15
Q

What does viscosity depend on?

A

IMF strength and length of the molecules in the liquid

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16
Q

Capillary Action

A

the result of the cohesive forces within a bulk sample of a liquid being overcome by adhesive forces

17
Q

Dipole-dipole IMF

A

attractive forces that occur between two polar molecules

18
Q

What do polar molecules have?

A

a permanent dipole; there is a partial positive charge at one end and a partial negative charge at the other end

19
Q

Hydrogen Bonding

A

strong type of dipole-dipole IMF that occurs between NOF

20
Q

Why are hydrogen bonds so strong?

A
  1. the elements bonded to H are very electronegative whereas H has a low electronegativity, resulting in a ver polar bonds
  2. H has a very small size, allowing hydrogen-bonding molecules to approach very closely and the smaller distance results in a stronger force of attraction
21
Q

Which is stronger? Hydrogen bonds or dipole-dipole IMFs?

A

hydrogen bonds

22
Q

Dipole-Induced Dipole Forces

A

attractive forces that occur between polar and nonpolar molecules; nonpolar molecules do not have permanent dipoles but it is possible to induce a temporary dipole in a nonpolar molecule

23
Q

Are dipole-dipole forces always stronger than dipole-induced dipole forces?

A

not always because the magnitude of the dipole-induced dipole can result in a force stronger than dipole-dipole forces

24
Q

Polarizibility

A

the extent to which the electron cloud of an atom or molecule can be distorted by an external electric charge

25
Q

As the number of electrons in a molecule increase, does the polarizibility increase or decrease?

A

it increases; therefore, it increases with increasing molar mass and molecular size

26
Q

Induced Dipole-Induced Dipole Forces/London Dispersion Forces/Dispersion Forces

A

attractive forces that occur between nonpolar molecules; there is no preferred directionality

27
Q

Are dispersion forces always weaker than dipole-dipole forces?

A

no, they can be stronger than dipole-dipole forces when they occur between highly polarizable molecules

28
Q

Dispersion forces are important in all liquids, even those consisting of polar molecules, why?

A

because any electron cloud can be distorted by the partial changes in surrounding molecules

29
Q

What happens to the boiling point as molar mass decreases?

A

boiling point decreases too

30
Q

Are Group 6A hydrides polar or nonpolar?

A

polar; therefore, there are dipole-dipole IMFs in pure liquids

31
Q

Why is the boiling point for water so high?

A

because there is extensive hydrogen bonding in water

32
Q

Besides high boiling point, what other properties do hydrogen bonds in water molecules influence?

A
  1. high enthalpy of vaporization
  2. high surface tension
  3. high heat capacity