S.1.1.2 and S.1.1.3 Kinetic Molecular Theory Flashcards

1
Q

What do states of matter depend on?

A

Temperature and pressure, as well as inter-particle forces and energy, determine the state of matter.

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2
Q

What is temperature?

A

Average kinetic energy of molecules

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3
Q

What are the properties of a solid?

A

Particles: closely packed together
Inter-particle forces: strong, particles vibrate in position
Shape: fixed
Volume: fixed

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4
Q

What are the properties of a liquid?

A

Particles: more spaced
Inter-particle forces: weaker, particles vibrate, rotate, and slide over each other
Shape: not fixed
Volume: fixed

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5
Q

What are the properties of a gas?

A

Particles: fully spread out
Inter-particle forces: negligible, particles vibrate, rotate, and move freely
Shape: not fixed
Volume: not fixed

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6
Q

How do the particles of solids, liquids, and gases differ?

A

Closely packed in solids; more spaced in liquids; fully spaced out in gases

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7
Q

How do the inter-particle forces in solids, liquids, and gases differ?

A

Strong, particles vibrate in position in solids; weaker, particles vibrate, rotate, and slide over each other in liquids; negligible, particles vibrate, rotate, and move freely in gases

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8
Q

Fluid

A

Substance with no fixed shape and yields easily to external pressure

Liquids and gases

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9
Q

Diffusion

A

Particles of a substance spread out evenly

Mostly in fluids

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10
Q

How do the rates of diffusion of different particles compare?

A

Smaller particles diffuse faster than larger particles.

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11
Q

Aqueous solution

A

Solute (less abundant) dissolved in solvent (more abundant)

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12
Q

Changes of state

A

The absorption or release of energy in substances

Freezing, melting, condensation, vaporization, deposition, sublimation

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13
Q

Endothermic process

A

Substance changes from more condensed to less condensed state; energy is absorbed by the particles from the surroundings

Solid to liquid/gas; liquid to gas

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14
Q

Exothermic process

A

Substance changes from less condensed to more condensed state; particles lose energy to surroundings; intermolecular forces become stronger

Gas to liquid/solid; liquid to solid

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15
Q

What is 0 K?

A

Absolute zero: the lowest temperature possible

No motion and no heat; no transfer of kinetic energy on collisions

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16
Q

Why is there no temperature change during a change in state of matter?

A

All added energy is used to overcome the intermolecular forces between particles in the substance

17
Q

Kelvin temperature

A

Proportional to the average kinetic energy of particles and considered an absolute scale

18
Q

Relationship between the Kelvin and Celsius scales

A

Increase of 1°C is equivalent to an increase of 1K

0°C is equivalent to 273.15K; absolute zero is -273.15°C