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General Chemistry H > Chapter 2 Review > Flashcards

Chapter 2 Review Flashcards

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1
Q

Define diffusion:

A

The spread of particles from one area of high concentration to an area of low concentration.

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2
Q

What can happen in diffusion?

A

Particles can interact with each other which can affect their spread.

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3
Q

What are the 3 states of matter?

A

Solids, liquids, and gasses.

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4
Q

Why does matter never stop moving?

A

It keeps solids from falling apart because molecules attract and repel each other.

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5
Q

What do the molecules in liquids do?

A

They take the shape and form of the container that they are in because without this, they have no shape or form.

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6
Q

What does head do to molecules?

A

It makes them more excited and they begin to go free for all in dance analogy.

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7
Q

What is evaporation?

A

When molecules become so excited jarring each other, they fly out of the liquid.

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8
Q

What is condensation?

A

When molecules in the air come in contact with coldness, this turns them into liquid.

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9
Q

What is expansion?

A

When molecules are excited, they want to expand as the temperature rises.

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10
Q

What is contraction?

A

When a gas gets cold, the molecules move slower and want to contract.

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11
Q

Because of expansion and contraction, what do people have to do when designing infrastructure and certain products?

A

There is space at the top of a bottle of water and cracks in the sidewalk and in the road to allow for expansion and contraction to take place in the change of climate with seasonal change.

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12
Q

Why can you not measure temperature with your hand?

A

The human body measures temperature relative to itself.

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13
Q

What is temperature?

A

It measures the effect of the speed of molecules resulting in expansion and contraction.

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14
Q

Why is mercury used in thermometers?

A

It is very dense so it expands and contracts a lot.

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15
Q

What does a barometer measure?

A

Atmospheric pressure

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16
Q

What is atmospheric pressure?

A

The pressure of the air we are surrounded by which is a result of the atmosphere pressing down.

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17
Q

What was bad about the first barometer?

A

It was too big since it used water.

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18
Q

Why was a mercury barometer used?

A

Because it could be much smaller.

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19
Q

How did mercury barometers work?

A

Mercury would sit on a plate with a tube above with measurements written on it. The mercury would adjust itself to match the atmospheric pressure moving up the tube as pressure increased. This was a result of the atmosphere pressing down on the mercury in the plate. It forced the mercury up the tube.

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20
Q

What are the standard pressure measurements?

A

1 atm = 760 mmHg = 14.7 psi = 101.3 kPa

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21
Q

Define (scientific) law:

A

Statements of observed regularities that have value because of their predictive power.

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22
Q

What causes laws to be created?

A

Experiments done over and over yield the sam results every time.

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23
Q

What do laws allow us to do?

A

They allow us to make predictions, but not explain why things happen or behave the way they do.

24
Q

What do theories do?

A

They explain different behaviors and observations.

25
Q

What is the difference between a law and a theory?

A

Laws help make predictions, theories explain the behaviors.

26
Q

What is standard temperature for a gas?

A

0 °C = 273 K

27
Q

What is the Kinetic Molecular Theory?

A

Gases are composed of tiny particles which are very far apart and the size of which is negligible; molecules are in constant, rapid, straight-line motion (therefore storing thermal energy); particles are assumed to have no attraction or repulsion for one another (collisions are elastic and total thermal energy remains constant); and the average thermal energy of the gas particles is directly proportional to the kelvin temperature of the gas.

28
Q

Define negligible:

A

Zero

29
Q

What is the combined gas law?

A

(P1V1)/(T1n1) = (P2V2)/(T2n2)

30
Q

How did Anders Celsius devise the Celsius temperature scale?

A

He put mercury in a tube and put that in water. When the water was frozen, he marked the level of mercury as 0 °C. When the water was boiling, he marked the level of mercury as 100 °C.

31
Q

How do you solve manometer problems?

A

1) Subtract the values from each other. 2) Subtract of add to the Proom (If atmospheric side has more pressure, subtract)

32
Q

Is atmospheric pressure the same everywhere on the surface of the earth?

A

No, it can change because of differences in altitude and temperature.

33
Q

Why is the fluid in a barometer mercury, rather than water or another liquid?

A

Mercury is denser than water meaning that it can expand more.

34
Q

Why can you not use a pump like at SDC to lift water up to the 3rd floor of an apartment complex?

A

There is not enough gravity/atmospheric pressure to push the water up that high.

35
Q

Why does the alcohol level in a thermometer rise when it is placed in a warmer fluid? (3 steps)

A

1) The molecules become excited and move quicker, 2) to maintain the same pressure, the volume increases, 3) once the pressure returns to its original value, the volume remains the same.

36
Q

Why does the alcohol level in a thermometer falls when it is placed in a colder fluid? (3 steps)

A

1) The molecules move slower, 2) to maintain the same pressure, the volume decreases, 3) once the pressure returns to its original value, the volume remains the same.

37
Q

Why is the Celsius scale not appropriate to use when describing the behavior of gases?

A

It isn’t appropriate to use the Celsius scale when describing the behavior of gases because it can be negative and when talking about temperature, there can be no negative movement of particles as well as when solving for pressure, volume, or other quantities, they cannot be negative.

38
Q

What is Boyle’s law?

A

P1V1 = P2V2, as P goes up V goes down and vice versa

39
Q

What is Charles’ law?

A

V1/T1 = V2/T2, as T goes up V goes up

40
Q

Define elastic:

A

A collision in which the total Kinetic energy of the colliding bodies is equal to their total kinetic energy in other forms

41
Q

What is the Gay-Lussac law?

A

P/T = K, K is a constant

42
Q

Define observed regularity:

A

After many tests, the results are similar and can be predicted due to prior trials

43
Q

What is pressure caused by?

A

Molecules hitting the sides of a container or the objects

44
Q

How does pressure change?

A

How often or how hard molecules hit the sides of a container.

45
Q

What will happen if a non-flexible container is used?

A

The gas sample will have an internal pressure that is different from external pressure.

46
Q

What will happen if a flexible container is used?

A

The internal and external pressures will always be the same because they are both pushing on the sides of the container equally.

47
Q

What is the difference between direct and inverse proportion?

A

Direct is as one number increases, the other does as well; Inverse is as one number increases, the other decreases

48
Q

What is Avegadro’s law?

A

P/n = K, K is a constant; pressure is proportional to the number of “puffs” and as we add more “puffs”, pressure increases

49
Q

What do molecules never actually do, but always do?

A

Molecules never actually touch, but are always in motino

50
Q

The cooler the molecules:

A

the slower they move

51
Q

Define melting:

A

When solids lose their shape due to heat; the molecules move so quickly that they lose attraction to each other and go crazy

52
Q

How does a thermometer work?

A

Energy is transferred into the thermometer so the liquid expands because the bulb is thinner.

53
Q

As volume increases, what happens?

A

Pressure decreases

54
Q

As the temperature or number of particles increases, what happens?

A

Pressure increases

55
Q

Define diffusion:

A

The spreading of something to that there is an equal amount of that something everywhere possible

General Chemistry H (4 decks)

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