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Principles of Chemistry 1 > U1- Module 2: Modeling of Matter > Flashcards

U1- Module 2: Modeling of Matter Flashcards

(58 cards)

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1
Q

When does pressure become present?

A

When a collision occurs between molecules

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2
Q

What effect does increasing the temperature have on the pressure?

A

Increases pressure

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3
Q

What effect does increasing the number of molecules have on the pressure?

A

Increases pressure

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4
Q

What effect does increasing the volume have on the pressure?

A

Decreases pressure

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5
Q

What effect does the mass of particles have on pressure?

A

No effect

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6
Q

Particulate Model of Matter

A

Explains and predicts the physical properties and behavior of substances.

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7
Q

What are the 2 assumptions of the particulate model of matter?

A
  1. Any large sample of a substance is made of a larger number of very small particles.
  2. Particles are constantly moving in random directions through empty space.
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8
Q

How many particles are in 1 mL of water?

A

3.34 x 10^22

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9
Q

How big is a particle of water?

A

Nanometer size (1 x 10^-9)

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10
Q

Pressure

A

The force of the particle collisions on the walls

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11
Q

Pressure Formula

A

Pressure = force/area

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12
Q

How is macroscopic energy measured?

A

Due to microscopic collisions

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13
Q

Temperature

A

A measure of the average kinetic energy per particle.

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14
Q

What increases temperature?

A

Addition of energy

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15
Q

What effect does mass have?

A

Inversely effects velocity
- increase; decrease volume
etc.

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16
Q

Does mass effect the energy levels?

A

No

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17
Q

The lower the mass…

A

The higher the velocity (speed)

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18
Q

Volume and amount of particles are…

A

Directly proportional

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19
Q

Temperature and volume are…

A

Directly proportional

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20
Q

What are the only 2 variables that are inversely proportional?

A

Pressure and volume

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21
Q

What happens to potential energy when you strengthen intramolecular forces?

A

Potential energy decreases

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22
Q

How does temperature and pressure affect intramolecular forces?

A
  • Increasing pressure increases the forces
  • Increasing temperature decreases the forces (more likely to move apart)
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23
Q

What happens to the average kinetic energy when water evaporates?

A

It doesn’t change

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24
Q

What are the ideal gas law conditions?

Study These Flashcards
A

High temperature and low pressures

25
What is true of the quantities in the ideal gas law?
None of them depend on the chemical composition of the actual system.
26
What happens when there are intramolecular forces when the temperature is low?
The particles begin to cluster/stick together
27
What is the 3rd basic assumption of the particulate model of matter?
Particles interact with each other. The strength of the interactions depends on the distance between particles.
28
What happens to interactions and physical states at different distances?
Low: Repel; solid Medium: Strong attraction; liquid High: Small/no attraction; gas
29
What happens to the average kinetic energy when temperature decreases?
It decreases
30
What does a phase change always involve?
A change in how matter and energy are distributed in a system.
31
Kinetic Energy
Due to particle motion
32
Potential Energy
Due to particle interactions (energy stored)
33
What value does potential energy start at?
0
34
As particles become closer, what happens to the level of the potential energy?
It decreases (becomes negative)
35
Why does potential energy have a negative value?
The attractive forces (kinetic energy) are doing the work of bringing the particles together = lower potential for particles to come together now (already happened)
36
Do larger or smaller particles have a stronger attraction?
Larger
37
What does lower potential energy levels mean?
A more stable configuration; stronger bond
38
What does a phase change always involve?
A transition in how matter and energy are distributed in a system.
39
What is the formula for kinetic energy?
KE = 1/2 mv^2
40
How do you get rid of attractive forces?
Add energy to overcome the phase change
41
How do you convert from a gas to. a liquid?
Remove energy to move the particles closer together.
42
What happens to the average KE of a particle during a phase change?
It stays constant (no change) - same pattern as temperature
43
What are the 2 competing phenomena in the environment?
1. Particles constantly move in random directions. 2. There are attractive interactions between particles.
44
What are the 2 critical elements that must be analyzed to understand system changes?
1. Potential energy of its particles 2. Number of configurations particles can adopt.
45
What is the outcome of the competition of a system dependent on?
1. Strength of interactions 2. Factors that impact movement of particles.
46
What is the relationship between relative potential energy and particle distance?
The farther apart particles are, the higher potential energy they have.
47
What phase is the potential energy highest?
Solid - repulsive attractions
48
What phase is the potential energy lowest?
Liquid - most stable phase
49
What is the relationship between distance and potential enegry?
The greater the distance between particles, the higher the potential energy level.
50
What phase has the most number of particle configurations?
Gases; more distance between particles
51
What factor is likely to induce a phase change to the gaseous state?
Random motion
52
What are the characteristics of liquids in PEC diagrams?
- Low potential energy - Low number of configurations
53
What are the characteristics of gases in PEC diagrams?
- High potential energy - High number of configurations
54
What are the phase changes in PEC diagrams dependent on?
- Temperature - Pressure
55
What phase state is favored at high temperatures?
Gas - The higher the temp, the higher the Pe - Allows the system to absorb the energy needed to change to the gaseous phase
56
What phase state is favored at lower pressures?
Gas - Higher pressure favors higher number of particle configurations - Particles have more freedom to adopt configurations
57
What phase is favored at higher pressures and lower temperatures in PEC diagrams?
Liquids
58
What phase is favored at lower pressures and higher temperatures in PEC diagrams?
Gases

Principles of Chemistry 1 (16 decks)

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