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Grade 11 Chemistry > Solids Liquids And Gases > Flashcards

Solids Liquids And Gases Flashcards

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1
Q

KMT

A

Kinetic molecular theory

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2
Q

What does the KMT say about gases?

A
  • Molecules are far apart with empty space between them
  • Lots of energy
  • no attractive forces between molecules
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3
Q

Because Gas molecules have lots of energy what occurs between them?

A

Motion of molecules are rapid and constant causing collisions. These Collisions are perfectly elastic.

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4
Q

Describe gas pressure using KMT

A

Results of simultaneous Collisions of billions of gas

Particles on an object.

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5
Q

What is atmospheric pressure (think KMT)

Can this vary between locations?

A

Collisions of air molecules.

Varies based on elevation. (Less air higher up= lower pressure)

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6
Q

What does a barometer measure?

A

Atmospheric pressure in Kpa

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7
Q

Describe Charles law

A

-Relates temperature and volume
-As the temperature of an enclosed gas increases, the volume increases.
V/T=V2/T2

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8
Q

Describe Boyle’s law

A

Relates volume and pressure

As the pressure of an enclosed gas increases the volume of the gas decreases. (Inverse=curbed graph)

P1V1=P2V2

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9
Q

Describe Gay-Lussac’s law

A

Relates pressure and temperature

As the temperature of an enclosed gas increases, the pressure increases. (With constant volume)
P1/T1=P2/T2

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10
Q

What is the combined gas law formula

A

P1V1/T1=P2V2/T2

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11
Q

What is Avogadros law formula

A

V1/N1=V2/N2

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12
Q

What’s the Ideal gas law

A

PV=nRT

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13
Q

What are the only two elements that are liquids at room temperature?

A

Mercury and Bromine

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14
Q

IMF

A

Inter molecular forces

Attractive forces between separate molecules

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15
Q

What does the KMT have to say about liquids

A
  1. Molecules have space between them, but are close enough to have some attractive forces.
  2. Molecules have some kinetic energy
  3. Molecules experience attractive forces that allow them to keep a definite volume.
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16
Q

When will liquids evaporate or vaporize?

A

When the molecules at the surface gain enough kinetic energy to overcome IMF’s

17
Q

When will gases condense back to a liquid?

A

When the molecules loose energy and the IMF’s become stronger

18
Q

Write a dynamic equilibrium for liquids and gases

A

Condensation (Liquid —->

19
Q

Use the KMT to describe solids

A
  1. Particles have very little space between them, with high IMF’s
  2. Particles have very little kinetic energy
  3. High IMF’s allow solids to retain a definite shape
20
Q

Malleable?

Ductile?

A

Malleable- can be formed or molded

Ductile- can be pulled and drawn out into wire

21
Q

Whats an equilibrium for solids and liquids

A

Freezing (Solid——>

22
Q

What’s an equilibrium for gases and solids

A

Deposition (Solid——>

23
Q

What’s a vacuum?

A

Space where no particles of matter exist

24
Q

Define Evaporation and vaporization

A

Vaporization- conversion of liquid to gas

Evaporation- vaporization on surface of a liquid

25
Q

Boiling point?

A

Temperature at which the vapor pressure of a liquid is equal to the external pressure on the liquid

26
Q

Describe the melting points of ionic and molecular solids?

A

Ionic- high melting point (strong IMF’s)

Molecular- low melting points

27
Q

What are some uses for sublimation?

A
  • freeze dry things
  • dry ice
  • Solid air fresheners
28
Q

What does a phase diagram show?

A

Graph showing the condition at which a substance exists at all stares.

Triple point= substance exists at all stares equally

(Based on temperature and pressure)

29
Q

Describe the compressibility or the three states…

A

Gases- compressible
Liquids-not compressible
Solids- not compressible

30
Q

On a heating curve, what does a flat slope indicate?

What does a steep slope indicate?

A

Flat line= more energy needed to increase temperature(change of state)

Steep line=less energy needed to raise temperature

31
Q

When reading a Manometer, if the gas pressure is bigger than the atmospheric pressure, How is the pressure calculated?

A

Add the atmospheric pressure and height of mercury

32
Q

If the gas pressure is lower than the atmospheric pressure, How is pressure calculated?

A

Subtract mercury height from atmospheric pressure

Grade 11 Chemistry (6 decks)

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