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School > Unit 12 Chemistry: States of Matter > Flashcards

Unit 12 Chemistry: States of Matter Flashcards

1
Q

Solid: shape? volume? density? compressible?

A

Definite shape, definite volume, high density, not compressible.

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2
Q

Examples of solids at room temp.

A

Copper, diamond, wood, plastic.

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3
Q

Liquid: shape? volume? density? compressible?

A

Indefinite shape, definite volume, lower density than solids, not compressible.

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4
Q

Examples of liquids at room temp.

A

Water, gasoline.

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5
Q

Gas: shape? volume? density? compressible?

A

Indefinite shape, indefinite volume, very low density, compressible.

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6
Q

Examples of gas at room temp.

A

Oxygen, carbon dioxide.

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7
Q

What does kinetic mean?

A

It means motion.

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8
Q

What does the Kinetic theory of Matter state?

A

It states that all particles of matter are in constant motion.

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9
Q

Describe the motion of gases:

A

Gas particles move quickly but independently of each other. The move in a straight line until they collide with another particle, then they change direction.

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10
Q

What are gases made up of and what do they look like?

A

Made up of negligible volume. They are far apart from each other and they do not attract or repel. They expand to fill their container.

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11
Q

What does elastic collision mean?

A

Elastic collision means that when gas particles collide, they do not stick together.

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12
Q

What causes gas pressure?

A

It is caused by the collisions of gas particles with each other and the walls of their container.

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13
Q

More collisions result:

A

If there are more particles in a particular place and if the temperature increases, the pressure will increase.

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14
Q

A region of space where no gas pressure is exerted is called a:

A

Vacuum

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15
Q

The pressure caused by the air in our atmosphere is called:

A

Atmospheric pressure

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16
Q

What is the relationship between altitude and pressure?

A

As altitude increase, atmospheric pressure decrease.

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17
Q

What is used to measure atmospheric pressure?

A

The barometer

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18
Q

The average pressure as measured at sea level is called:

A

Standard pressure

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19
Q

Standard pressure quantities:

A

1 atm
760 mmHg
101.3 kPa

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20
Q

A measure of the amount of kinetic energy a sample of matter has is called:

A

Temperature

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21
Q

Not all particles have the same…

A

kinetic energy

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22
Q

What is the relationship between the average KE and kelvin temp?

A

The average KE is directly proportional to the kelvin temp.

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23
Q

Kelvin is never….

A

A negative number

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24
Q

As temperature decreases, what happens to the particles?

A

The particles move slower and slower.

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25
Q

What is the formula to calculate Kelvin?

A

degree celsius + 273

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26
Q

What does STP stand for and what does it equal?

A

Standard temperature and pressure and equals 0 degrees celsius and 273K

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27
Q

If the temperature goes from 200K to 400K, what happens to the KE?

A

The average KE will double.

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28
Q

If the temperature goes from 100K to 300K, what happens to the KE?

A

The average KE will triple.

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29
Q

If the temperature goes from 300K to 100K, what happens to the KE?

A

The average KE will be 1/3.

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30
Q

What is significant about the temperature absolute zero?

A

The particles stop moving. Nothing can be colder than absolute zero on the kelvin scale.

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31
Q

What happens to particle motion as the temperature of a substance increases?

A

The particles move faster.

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32
Q

Why do liquids move as a unit?

A

There is intermolecular forces of attraction between particles.

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33
Q

Are the forces of attraction greater or weaker in a liquid than in a gas?

A

Much greater

34
Q

Liquids have the ability to do what?

A

Slide past each other and have the ability to flow.

35
Q

Are liquids compressible?

A

Slightly

36
Q

Is a liquid’s kinetic energy more or less than a solid or gas?

A

Less than gas, but more than solid. Right in the middle.

37
Q

What happens to liquids if they are left out?

A

They evaporate and change from a liquid to a gas.

38
Q

The conversion of a liquid to gas below the substance’s boiling point is called:

A

Evaporation

39
Q

In order to evaporate, what must happen?

A

A particle must have enough KE to overcome the forces of attraction.

40
Q

When the particles with the highest KE evaporate away from liquids, what happens to the temp and KE?

A

They both decrease.

41
Q

How does heat flow?

A

It flows from warmer to cooler objects.

42
Q

What kind of process is evaporation?

A

It is a cooling process. The particles that move the fastest leave and lowers KE.

43
Q

What happens to particles in a closed container?

A

They still evaporate, but the particles are trapped. They will build up in concentration, making them more likely to collide with each other.

44
Q

A dynamic process where two reactions occur at the same rate is called:

A

Equilibrium

45
Q

Where are particles with the most KE found?

A

The surface of a liquid.

46
Q

The pressure caused by the evaporated particles in a closed container is called:

A

Vapor pressure

47
Q

What is the relationship between vapor pressure and temp?

A

As temperature increases, vapor pressure will increase (direct relationship).

48
Q

What is the relationship between IM forces and vapor pressure?

A

As IM forces increase, vapor pressure decreases (indirect relationship).

49
Q

The temperature at which a substance will boil is called:

A

Boiling point

50
Q

Conversion from liquid to gas throughout the entire substance is called:

A

Boiling

51
Q

In order to boil:

A

Vapor pressure=atm pressure

52
Q

The boiling point at standard pressure is called:

A

Normal boiling point

53
Q

What does boiling point depend on?

A

It depends on atm pressure

54
Q

What is the relationship between atmospheric pressure and boiling point?

A

High AP: BP increase
Low AP: BP decrease

55
Q

Boiling can also occur by….

A

Lowering atm pressure until it equals vapor pressure

56
Q

Below sea level…

A

It takes more VP=atm, so a higher BP is observed here (high pressure).

57
Q

Above sea level…

A

It takes less energy to have VP=atm pressure (low pressure).

58
Q

What is the normal boiling point for water?

A

100 degrees celsius or 373K

59
Q

In the solid state, particles have the lowest amount of…..

A

KE

60
Q

Are the IM forces higher or lower in the solid state than the other states?

A

Higher

61
Q

How do the particles in the solid state move?

A

They vibrate and place and they do not flow because they are in fixed positions.

62
Q

Solids contain particles that are arranged in an orderly, repeating pattern called…

A

Crystalline solids

63
Q

Example of Crystalline solids:

A

Table salt, NaCl

64
Q

Lack order among the particles that it makes up is called…

A

Amorphous solids

65
Q

Example of an Amorphous solid:

A

Glass, SiO2

66
Q

The attraction of positive and negative increases the likelihood to stay in the solid state. Has strong IM forces.

A

Ionic Crystalline solids

67
Q

Held together by covalent bonds and have much weaker IM forces.

A

Covalent Crystalline or Amorphous solids.

68
Q

When will solids melt?

A

When the particles in the solid state have enough KE to break free from their free positions.

69
Q

What temperature does melting occur?

A

The temperature at which this occurs is called the melting point.

70
Q

Since IM forces are stronger in ionic solids, will they have higher or lower m.p.s than molecular solids?

A

Higher m.p.s.

71
Q

The conversion of a solid to a gas without going through the liquid state is called…

A

Sublimation

72
Q

What is the reverse process of sublimation?

A

Deposition

73
Q

When does sublimation occur?

A

it occurs when the vapor pressure of a solid is greater than or equal to the surrounding atm pressure.

74
Q

Is the vapor pressure of solids higher or lower than the vp of liquids?

A

Much lower but it will increase if the solid is heated.

75
Q

Why is sublimation difficult?

A

Most substances will melt before VP = ATM pressure

76
Q

How is it easier to get a solid to sublime?

A

Lower ATM pressure

77
Q

Why does dry ice sublimate at room temp?

A

it has a high VP due to its weaker IM forces.

78
Q

Shows the conditions of temperature and pressure that are necessary for a substance to exist as a solid, liquid, or gas is called…

A

A phase diagram

79
Q

The conditions of temperature and pressure at which all three states of matter are in equilibrium with each other is called…

A

Triple point

80
Q

What are the two types of phase diagrams?

A
  1. Liquid state is more dense than the solid state (line to the left).
  2. Solid state is more dense than the liquid state (line to the right).

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