Chapter 16 Flashcards

1
Q

Particles are very close together in an orderly, fixed and usually crystalline arrangement.

A

Solid

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2
Q

An endothermic change of state in which a solid becomes a liquid

A

Melting

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3
Q

The temperature and pressure at which a solid becomes a liquid

A

Melting point

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4
Q

Have enough kinetic energy to be able to move past each other easily, take the shape of their container.

A

Liquid

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5
Q

Resistant flowing liquids

A

Viscous

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6
Q

When liquids have attraction for each other

A

Cohesion

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7
Q

Attraction for particles of solid surfaces

A

Adhesions

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8
Q

Tendency to decrease their surface area to the smallest size possible, thereby decreasing their energy.

A

Surface tension

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9
Q

Attractive forces do not have a great effect on particles, which makes the particles independent.

A

Gas

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10
Q

The temperature and pressure at which the number of liquid particles becoming gas particles is the same as the number of gas particles returning to the liquid phase

A

Boiling point

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11
Q

The temperature and pressure at which a liquid becomes a solid

A

Freezing point

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12
Q

Solid to gas

A

Sublimation

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13
Q

A gas becomes a solid without first becoming a liquid

A

Deposition

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14
Q

A region that has the same composition and properties throughout

A

Phase

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15
Q

When particles are constantly moving between two or more phases, yet no net change in the amount of the substance in either phase occurs

A

Equilibrium

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16
Q

The pressure exerted by the molecules of a gas, or vapor, in equilibrium with a liquid

A

Vapor pressure

17
Q

A graph of the relationship between the physical state of a substance and the temperature and of the substance

A

Phase diagram

18
Q

The temperature and pressure conditions at which the solid, liquid, and gas phases of a substance coexist at equilibrium

A

Triple point

19
Q

Temperature and pressure at which the gas and liquid states of a substance become identical and form one phase

A

Supercritical fluid

20
Q

Liquid and vapor phrases are indistinguishable

A

Critical point

21
Q

Why do ionic compounds tend to have higher boiling and melting points?

A

They’re stronger bonds so they need more heat to break bonds

22
Q

Why do molecular substances with weak intermolecular forces have low melting points?

A

Need less energy because they’re weak bonds

23
Q

Why do molecular substances with strong intermolecular forces have high melting points?

A

Takes more energy to break bonds

24
Q

How do dipole-dipole forces affect the melting and boiling points of substances?

A

Takes more energy to break bonds

25
What forces are involved in hydrogen bonding?
F,O, N
26
What affect does hydrogen bonding have on physical properties of water?
Have a higher boiling point and crystals expand when freezing occurs
27
How can a molecule have a mom entry dipole?
When nonpolar molecules have dipoles that cancel each other out
28
Force of attraction between molecules with momentary dipoles
LDF
29
Explain the role of particle size and shape on the strength of attractive forces
Bigger size = stronger attractive force