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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
What is the formula to calculate Kelvin?
degree celsius + 273
26
What does STP stand for and what does it equal?
Standard temperature and pressure and equals 0 degrees celsius and 273K
27
If the temperature goes from 200K to 400K, what happens to the KE?
The average KE will double.
28
If the temperature goes from 100K to 300K, what happens to the KE?
The average KE will triple.
29
If the temperature goes from 300K to 100K, what happens to the KE?
The average KE will be 1/3.
30
What is significant about the temperature absolute zero?
The particles stop moving. Nothing can be colder than absolute zero on the kelvin scale.
31
What happens to particle motion as the temperature of a substance increases?
The particles move faster.
32
Why do liquids move as a unit?
There is intermolecular forces of attraction between particles.
33
Are the forces of attraction greater or weaker in a liquid than in a gas?
Much greater
34
Liquids have the ability to do what?
Slide past each other and have the ability to flow.
35
Are liquids compressible?
Slightly
36
Is a liquid's kinetic energy more or less than a solid or gas?
Less than gas, but more than solid. Right in the middle.
37
What happens to liquids if they are left out?
They evaporate and change from a liquid to a gas.
38
The conversion of a liquid to gas below the substance's boiling point is called:
Evaporation
39
In order to evaporate, what must happen?
A particle must have enough KE to overcome the forces of attraction.
40
When the particles with the highest KE evaporate away from liquids, what happens to the temp and KE?
They both decrease.
41
How does heat flow?
It flows from warmer to cooler objects.
42
What kind of process is evaporation?
It is a cooling process. The particles that move the fastest leave and lowers KE.
43
What happens to particles in a closed container?
They still evaporate, but the particles are trapped. They will build up in concentration, making them more likely to collide with each other.
44
A dynamic process where two reactions occur at the same rate is called:
Equilibrium
45
Where are particles with the most KE found?
The surface of a liquid.
46
The pressure caused by the evaporated particles in a closed container is called:
Vapor pressure
47
What is the relationship between vapor pressure and temp?
As temperature increases, vapor pressure will increase (direct relationship).
48
What is the relationship between IM forces and vapor pressure?
As IM forces increase, vapor pressure decreases (indirect relationship).
49
The temperature at which a substance will boil is called:
Boiling point
50
Conversion from liquid to gas throughout the entire substance is called:
Boiling
51
In order to boil:
Vapor pressure=atm pressure
52
The boiling point at standard pressure is called:
Normal boiling point
53
What does boiling point depend on?
It depends on atm pressure
54
What is the relationship between atmospheric pressure and boiling point?
High AP: BP increase Low AP: BP decrease
55
Boiling can also occur by....
Lowering atm pressure until it equals vapor pressure
56
Below sea level...
It takes more VP=atm, so a higher BP is observed here (high pressure).
57
Above sea level...
It takes less energy to have VP=atm pressure (low pressure).
58
What is the normal boiling point for water?
100 degrees celsius or 373K
59
In the solid state, particles have the lowest amount of.....
KE
60
Are the IM forces higher or lower in the solid state than the other states?
Higher
61
How do the particles in the solid state move?
They vibrate and place and they do not flow because they are in fixed positions.
62
Solids contain particles that are arranged in an orderly, repeating pattern called...
Crystalline solids
63
Example of Crystalline solids:
Table salt, NaCl
64
Lack order among the particles that it makes up is called...
Amorphous solids
65
Example of an Amorphous solid:
Glass, SiO2
66
The attraction of positive and negative increases the likelihood to stay in the solid state. Has strong IM forces.
Ionic Crystalline solids
67
Held together by covalent bonds and have much weaker IM forces.
Covalent Crystalline or Amorphous solids.
68
When will solids melt?
When the particles in the solid state have enough KE to break free from their free positions.
69
What temperature does melting occur?
The temperature at which this occurs is called the melting point.
70
Since IM forces are stronger in ionic solids, will they have higher or lower m.p.s than molecular solids?
Higher m.p.s.
71
The conversion of a solid to a gas without going through the liquid state is called...
Sublimation
72
What is the reverse process of sublimation?
Deposition
73
When does sublimation occur?
it occurs when the vapor pressure of a solid is greater than or equal to the surrounding atm pressure.
74
Is the vapor pressure of solids higher or lower than the vp of liquids?
Much lower but it will increase if the solid is heated.
75
Why is sublimation difficult?
Most substances will melt before VP = ATM pressure
76
How is it easier to get a solid to sublime?
Lower ATM pressure
77
Why does dry ice sublimate at room temp?
it has a high VP due to its weaker IM forces.
78
Shows the conditions of temperature and pressure that are necessary for a substance to exist as a solid, liquid, or gas is called...
A phase diagram
79
The conditions of temperature and pressure at which all three states of matter are in equilibrium with each other is called...
Triple point
80
What are the two types of phase diagrams?
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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