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Ingram Chemistry > Kinetic Molecular Theory > Flashcards

Kinetic Molecular Theory Flashcards

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1
Q

What is the Kinetic Molecular Theory

A

An idea that is based on the idea that particles of matter are always in motion

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2
Q

What does the Kinetic Molecular Theory Explain?

A

The properties of solids, liquids, and gases

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3
Q

Gas particles are ___ apart

A

Far

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4
Q

What are Elastic Collisions?

A

collisions between gas particles and the container walls

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5
Q

What is the movement of Gas particles

A

Continuous, Rapid, and Random

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6
Q

Does gas particles have Potential or Kinetic energy

A

Kinetic Energy

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7
Q

Yes or No - Are there any forces of attraction between gas particles?

A

No

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8
Q

What does the temperature depend on in a Gas

A

Amount of Kinetic Energy

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9
Q

What are the 2 types of Ideal Gases

A

Hypothetical and Nonpolar

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10
Q

What is an Ideal Gas?

A

A gas that fits all assumptions of the KMT

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11
Q

What characteristics of Gases make it Ideal?

A

Pressure is not very high and Temperature is not very low

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12
Q

True or False - Lighter gas particles have higher speeds than heavier gases.

A

True

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13
Q

What are the 6 characteristics of Gases

A

1) Expandable
2) Fluid
3) Low Density
4) Compressible
5) Diffusion
6) Effusion

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14
Q

Gases have a ____ shape and a ____ volume

A

indefinite; indefinite

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15
Q

What does it mean for gases to be fluid?

A

The gas particles are bale to glide past one another.

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16
Q

Do gases have a high or low density? Why?

A

Low; the particles are far apart from each other.

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17
Q

Why are gases compressible?

A

The particles can crowd close together.

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18
Q

What happens to the volume of a gas if it compresses?

A

the volume decreases

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19
Q

What does diffusion mean?

A

The particles are able to spread out and fill up a lot of space. (Think of a diffuser)

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20
Q

What is a Real Gas?

A

A gas that does NOT behave according to the KMT

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21
Q

What are some characteristics of a Real Gas?

A

very high pressure; low temperature; polar molecules

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22
Q

What can happen to a gas if you raise the pressure, bit lower the temperature?

A

the particles will move closer, the Kinetic Energy will decrease, and the particles will condense and now form a liquid.

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23
Q

What is a Liquid?

A

A substance that can flow and takes the shape of its’ container

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24
Q

A liquid has a ____ volume and _____ shape

A

definite; indefinite

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25
Q

Does a liquid have a lower or higher density that a Gas? Why?

A

Higher density than gas due to the close arrangement of particles

26
Q

Can you compress a liquid?

A

No (Think bellyflop)

27
Q

Is a liquids ability to diffuse faster or slower than a gas?

A

Slower

28
Q

How can you speed up the process of Diffusion in a liquid?

A

increase the temperature

29
Q

What isu Tension?

A

a force that pulls the sides of the liquid together to create a “barrier”

30
Q

The higher the force of attraction, the higher the ___ in a Liquid.

A

Surface Tension

31
Q

What is Evaporation?

A

when particles from the top layer of a liquid becomes gas; this has NO BUBBLES

32
Q

What is Boiling?

A

The change of a liquid to a gas through high heat and it DOES have BUBBLES

33
Q

Solids have a ____ volume, ____ shape, and a ___ melting point

A

Definite; Definite; Definite

34
Q

What are some characteristics of a Solid?

A

High density; incompressibility, low rate of Diffusion

35
Q

What are the two types of Solids?

A

Crystalline and Amorphous

36
Q

What consists of a Crystalline Solid?

A

Crystals; an orderly arrangement of atoms; geometric repeating patterns

37
Q

What is a Amorphous Solid?

A

A solid of which the patterns are arranged randomly, and has a definite shape, but doesn’t have a geometric shape

38
Q

What is a Super Cooled Liquid?

A

substances that retain certain liquid properties even at temperatures at which they appear to be solid

39
Q

What is an example of a Super Cooled Liquid?

A

Real Glass

40
Q

What are the 4 Binding Forces in a Crystal?

A

1) Ionic Crystals
2) Covalent Network Crystals
3) Metallic Crystals
4) Covalent Molecular Crystals

41
Q

What are the characteristics of Ionic Crystals?

A
  • Positive + negative ions
  • Hard and Brittle
  • High melting points
  • good Insulators
42
Q

What are the characteristics of a Covalent Network Crystal?

A
  • high melting point
  • nonconductors or semiconductors
43
Q

What makes up a Metallic Crystal?

A

metal cations surrounded by valence electrons

44
Q

What are the characteristics of a Covalent Molecular Crystal?

A
  • Covalent bonds held together by IMF’s
  • soft
  • easily vaporized
  • good insulators
45
Q

What is a phase?

A

A uniform state of matter.

46
Q

What is an Equilibrium?

A

When 2 opposite changes occur at equal times

47
Q

Substances change back and forth between states at ___ speeds.

A

Equal

48
Q

What does Endothermic mean?

A

The particles take IN energy
- the particles move faster

49
Q

What does Exothermic mean?

A

The energy in the particles are EXiting
- the particles move slower

50
Q

What is freezing?

A

Liquid to a Solid; Exothermic

51
Q

What is Melting?

A

Solid to Liquid; Endothermic

52
Q

What is Condensation?

A

Gas to Liquid; Exothermic

53
Q

What is Vaporization?

A

Liquid to Gas; Endothermic

54
Q

What is Deposition?

A

Gas to Solid; Exothermic

55
Q

What is Sublimation?

A

Solid to Gas; Endothermic

(Think of sublimation starts with an “s” so it starts as a solid)

56
Q

What is vapor?

A

A gas in contact with a liquid or solid phase

(like Fog)

57
Q

What is Volatile?

A

Liquids that evaporate readily, have weak IMF’s

EX. Alcohol - it dries quickly

58
Q

What is the “Latent Heat of Fusion”?

A

The Equilibrium between a Solid and Liquid

59
Q

What is the “Latent Heat of Vaporization”?

A

The equilibrium between a liquid and gas

60
Q

What is the Triple Point?

A

the point at which a solid, liquid, and gas all coexist

61
Q

What is the Critical Point?

A

the highest point of pressure and temperature on the graph

Ingram Chemistry (7 decks)

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