Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chem 151 > Unit 1 Review > Flashcards

Unit 1 Review Flashcards

1
Q

What are some properties used to differentiate substances?

A

density, solubility, and melting point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is viscosity?

A

The thickness of a substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are extensive properties?

A

Properties that depend on the amount of a substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are intensive properties?

A

Properties that do not depend on the amount of a substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Name some extensive properties

A

Mass, volume, concentration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Name some intensive properties

A

boiling point, density, viscosity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are system properties?

A

Properties that are not unique to each substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Name some system properties

A

Temperature and pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Good differentiating characteristics have values that:

A

do not depend on the amount of substance and are unique

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is melting point?

A

When a solid turns into a liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is boiling point?

A

When a liquid turns into a gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What does normal mean in chemistry?

A

The substance is at 1 atm pressure (sea level)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

How do you convert celcius to kelvin?

A

Add 273.15 units to the original temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What happens when a substance’s temperature is below the melting point?

A

The substance is a solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What happens when a substance’s temperature is above the melting point?

A

The substance is a liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What happens if the substance’s temperature is above the boiling point?

A

The substance is a gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What happens if the substance’s temperature is below the melting point?

A

The substance is a solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is the melting point of water?

A

0 degrees celsius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is the boiling point of water?

A

100 degrees celsius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What happens when energy is absorbed by the system?

A

The change in energy is greater than 0, heating up

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What happens when energy is released by the system?

A

The change in energy is less than 0, cooling down

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What happens to temperature during a phase change?

A

Nothing, it stays constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Can temperature increase or decrease without energy doing the same?

A

NO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the starting point on a change in energy vs temperature graph?

A

When the change in energy (delta E) is 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Is delta E postive or negative when cooling?
Negative
26
Is delta E positive or negative while heating?
Positive
27
What happens during the phase change condensing?
A gas becomes a liquid.
28
What happens during the phase change deposition?
A gas becomes a solid.
29
What happens during the phase change sublimation?
A solid becomes a gas.
30
What happens during the phase change vaporization?
A liquid becomes a gas.
31
What happens during the phase change freezing?
A liquid becomes a solid.
32
What happens during the phase change melting?
A solid becomes a liquid.
33
What is phase stability?
Different phases are stable at different values of temperature and pressure.
34
Does every liquid evaporate?
Yes, every liquid can evaporate at a certain temperature (depending on the substance)
35
When does boiling occur?
When vapor pressure equals to external pressure
36
What is vapor pressure?
the pressure exerted by the vaporized substance
37
How would you boil a substance without increasing the temperature?
Decreasing the pressure (which lowers the boiling point)
38
What does volatile mean?
When a substance can transition to the gas phase more easily than another
39
What happens if the vapor pressure is higher pertaining to volatility?
The substance is more volatile
40
What happens to the boiling point if the vapor pressure is high?
The boiling point is low
40
Do opposite processes occur at the same temperatures?
Yes, for example, condensing and boiling occurs at the same temperature
41
What is the particulate model of matter?
Matter is made of a large number of very small particles that move constantly in random directions
42
Can particles be made of anything?
Yes (atoms, ions, molecules, etc)
43
What is the difference between the states of matter?
The space between particles
44
What state do particles have the highest average kinetic energy?
It is the same level for all phases
45
What state do particles have the highest average speed
It is the same for all phases
45
What system property changes the average kinetic energy of particles?
Temperature
45
Does each particle move at the same speed?
NO, they move at varying speeds.
46
What is a measure of the average kinetic energy per particle?
temperature
47
Do particles with different masses have different average speeds?
Yes, higher mass=slower speed and vice versa
47
What increases pressure?
Increase in temperature and/or number of particles
47
What causes pressure?
The collisions of particles between the walls of their container
48
What decreases pressure?
Increase in volume
49
What is the formula for density?
(number of particles)/ (volume)
50
What is the ideal gas law formula(s)?
PV= NRT OR PV=KbNT
51
Do gas particles interact with each other?
No, regardless of temperature gas particles should be assumed to not interact with each other
51
What are intermolecular/attractive forces?
How much the particles interact with each other
52
What state has the highest intermolecular forces?
Solid
53
What state has the lowest intermolecular forces?
Gas
54
What happens to potential energy if the intermolecular forces are strong?
It decreases, for example solids have the lowest potential energy
55
Particles that attract each other are said to have...?
Negative potential energy and strong intermolecular forces (ex: solids)
56
What phase has the lowest potential energy?
Solids
57
What phase has the highest potential energy?
Gas
58
The stronger the attractive forces, the the potential energy
LOWER
59
Are temperature and kinetic energy proportional?
YES
60
How does potential energy increase?
With a phase change
61
What happens to temperature and the speed of particles at the triple point?
Temperature is the same, so the average speed of the particles is the same
62
Do you need more or less energy to perform a phase change on a substance with strong molecular forces?
MORE
62
What changes kinetic energy?
Temperature increase/decrease
63
The higher the boiling point the the IMFs
STRONGER
64
The stronger the IMFs, the LOWER the
Viscosity, volatility, and vapor pressure
65
The stronger the IMFs, the HIGHER THE
Boiling point, sublimation point, density, and viscosity
66
What is the number of configurations (entropy)?
The possible number of arrangements of something
67
Entropy from lowest to highest is
solid--->liquid--->gas
68
What state is favored at high temperatures?
gas
68
As potential energy increases, the number of configurations...
INCREASES
69
What temperatures are optimal for potential energy absorptions?
High temperatures
70
At low temperatures, can potential energy still be absorbed?
Yes
71
What amount of configuations does high pressure prefer?
LOW (solids can take more pressure, but have less configurations)
72
What amount of configurations does low pressure prefer
HIGH (gas cannot take large amounts of pressure, but have more configuations)
73
What element is represented by a blue molecule?
Nitrogen
74
What element is represented by a black molecule?
Carbon
75
What element is represented by a red molecule?
Oxygen
76
What are the categories of substances?
Pure and mixed
77
What are the categories of pure substances?
Elemental and chemical compound
78
What are the categories of chemical compounds?
Ionic and covalent (molecular)
79
What are elementary substances?
They are the simplest substances made of identical particles of the same type (either free or bonded)
80
What are chemical compounds?
They are made of identical particles of two or more of the same type (ONLY bonded)
81
Can liquids have multiple phases?
Yes, if they do not mix
82

Chem 151 (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions