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Chemistry S2 > Chapter 10- States Of Matter > Flashcards

Chapter 10- States Of Matter Flashcards

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0
Q

Particles of matter are

A

Always in motion

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1
Q

Kinetic molecular theory

A

Explains the behavior of atoms/ molecules in different states of matter

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2
Q

Particles exhibit what type of motion

A

Vibrational, rotational, translational

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3
Q

All movement stops only at

A

Absolute zero

K = -273 C

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4
Q

Kinetic energy

A

Measures the amount of energy contained by a moving object

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5
Q

Temperature

A

Measure of the average kinetic energy of a substance

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6
Q

Kinetic energy equation

A

KE = 1/2mv^2

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7
Q

At the same temperature, particles of a lower max have a

A

Higher velocity

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8
Q

STP

A

Standard temperature
0 degrees C
-273 degrees K
1 ATM

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9
Q

Solids

A

Typically most dense
Particles are close together
Lowest temperature
Lowest average KE of particles

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10
Q

Liquids

A

Particles still relatively close together

Temperature and average KE increase from solid state

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11
Q

Gasses

A

Particles extremely far apart
Lowest density
Highest temperature and average KE

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12
Q

Intramolecular forces

A

Chemical bonds

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13
Q

Intermolecular forces

A

Attractions between molecules, strongest in solids

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14
Q

Strength of intermolecular forces

A
  1. Hydrogen bonds
  2. Dipole - dipole attraction
  3. Dipole induced dipole attraction
  4. London dispersion forces
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15
Q

Cohesive

A

Attractive force between two like molecules

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16
Q

Adhesive

A

Attractive force between two different molecules

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17
Q

Gasses are

A

Fluids

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18
Q

Fluid

A

A non solid state of matter in which particles are free to move or flow past each other

19
Q

gases have

A

low density and high compressibility

20
Q

gases readily

A

diffuse

21
Q

effusion

A

process by which gas particles pass through a tiny opening when pressure is exerted on them

22
Q

the rate of effusion of a gas is directly proportional to

A

the gas velocity

23
Q

crystalline solids

A

particles arranged in ordered, geometric pattern
definite melting point
ionic compounds

24
Q

amorphous solids

A

particles arranged randomly

can flow over a wide range of temperatures

25
Q

4 types of crystalline solids

A

ionic crystals
covalent network crystals
covalent molecular crystals
metallic crystals

26
Q

liquids have

A

surface tension

27
Q

surface tension

A

force that tends to pull adjacent parts of a liquids surface together, thereby decreasing surface area to the smallest possible size

28
Q

capillary action

A

the attraction of the surface of a liquid to the surface of a solid

29
Q

volatile

A

readily vaporizes

30
Q

melting

A

solid to liquid

31
Q

sublimation

A

solid to gas

32
Q

freezing

A

liquid to solid

33
Q

vaporization

A

liquid to gas

34
Q

condensation

A

gas to liquid

35
Q

deposition

A

gas to solid

36
Q

phase

A

any part of a system with uniform composition and properties

37
Q

vapor

A

a gas in contact with its liquid or solid phase

38
Q

vapor pressure

A

the pressure exerted on the surface of the liquid phase by its corresponding vapor

39
Q

liquid vapor equillibrium

A

state where the rate of evaporation is equal to the rate of condensation

40
Q

boiling point

A

the temperature at which the equilibrium vapor pressure of the liquid equals the atmosphere pressure

41
Q

normal boiling point

A

boiling point at 1 atm of pressure

42
Q

enthalpy

A

a measure of the total energy of a system

43
Q

molar enthalpy of vaporization

A

amount of heat energy needed to vaporize one mole of liquid at the liquids boiling point under constant pressure

44
Q

molar enthalpy of fusion

A

the amount of heat energy that must be added to melt one mole of solid at the solids melting point

Chemistry S2 (6 decks)

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