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Chemistry > module 11 to 13 > Flashcards

module 11 to 13 Flashcards

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1
Q

Describes the behavior of matter in terms of particles in motion.

A

Kinetic-molecular theory

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2
Q

A collision between gases in which no energy is lost

A

elastic collision

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3
Q

measure of the average kinetic energy of the particles in a sample of matter.

A

temperature

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4
Q

Movement of one material through another.

A

diffusion

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5
Q

states that the rate of effusion/diffusion for a gas is inversely proportional to the square root of its molar mass.

A

Graham’s law of effusion

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6
Q

Force per unit area

A

pressure

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7
Q

Used to measure atmospheric pressure.

A

barometer

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8
Q

SI unit of pressure; equal to one newton per square meter

A

pascal

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9
Q

Equal to 101.3 Kilopascal (kPa)

A

atmosphere

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10
Q

States that the total pressure of a mixture of gases is equal to the sum of pressures of all gases in the mixture.

A

Dalton’s law of partial pressures

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11
Q

Weak forces that result from temporary shifts in the density of the electrons in electron clouds.

A

dispersion force

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12
Q

Attractions between oppositely charged regions of polar molecules

A

dipole-dipole force

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13
Q

A dipole-dipole attraction that occurs between molecules containing a hydrogen atom bonded to a small, highly electronegative atom with at least one lone electron pair.

A

hydrogen bond

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14
Q

Measure of the resistance of a liquid to flow.

A

viscosity

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15
Q

The energy required to increase the surface area of a liquid by a given amount.

A

surface tension

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16
Q

Compounds that lower the surface tension of water

A

surfactant

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17
Q

solid whose atoms, ions, or molecules are arranged in an orderly, geometric structure

A

crystalline solid

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18
Q

The smallest arrangement of atoms in a crystal lattice

A

unit cell

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19
Q

Elements that exist in different forms at the same state.

A

allotrope

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20
Q

Solids not arranged in a regular, repeating pattern; the opposite of crystalline solids

A

amorphous solid

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21
Q

The temperature at which the forces that hold the crystal lattice of a solid together are broken and becomes a liquid.

A

melting point

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22
Q

Process by which a liquid changes to a gas or vapor.

A

vaporization

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23
Q

When vaporization only occurs only at the surface of a liquid.

A

evaporation

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24
Q

The pressure exerted by a vapor over a liquid is called

A

vapor pressure

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25
Q

The temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure

A

boiling point

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26
Q

The temperature at which a liquid is converted into a crystalline solid.

A

freezing point

27
Q

The process by which a gas or a vapor becomes a liquid.

A

condensation

28
Q

process by which a substance changes from a gas or vapor into a solid without becoming a liquid.

A

deposition

29
Q

A graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure.

A

phase diagram

30
Q

The point on a phase diagram that represents the temperature and pressure at which three phases of a substance can coexist.

A

triple point

31
Q

States that the volume of a fixed amount of a gas held at a constant temperature varies inversely with the pressure.

A

Boyle’s law

32
Q

Zero on the Kelvin scale; represents the lowest possible theoretical temperature.

A

absolute zero

33
Q

States that the volume of a given amount of gas is directly proportional to its Kelvin temperature at constant pressure.

A

Charles’s law

34
Q

States that the pressure of a fixed amount of gas varies directly with the Kelvin temperature when the volume remains constant.

A

Gay-Lussac’s law

35
Q

States that the relationships between pressure, temperature, and volume of a fixed amount of gas.

A

Combined Gas law

36
Q

States that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

A

Avogadro’s principle

37
Q

The volume that 1 mol occupies at 0.00 degrees Celsius and 1.00 atm.

A

molar volume

I mole has 22.4L

38
Q

The conditions of 0.00 degrees Celsius and 1.00 atm.

A

standard temperature and pressure (STP)

39
Q

Experiments using known values of P, V, T, and n have determined the value of this constant

A

Ideal gas constant

Represented by R

40
Q

Describes the physical behavior of an ideal gas in terms of the pressure, volume, temperature, and number of moles of gas present.

A

Ideal gas law

41
Q

A mixture containing particles that are large enough that, if left undisturbed, will settle out over time due to gravity.

A

Suspension

42
Q

Heterogenous mixture of intermediate size that cannot be separated by settling or filtration.

A

colloid

43
Q

The erratic movement of colloid particles

A

Brownian motion

44
Q

The scattered light by dispersed colloid particles.

A

Tyndall effect

45
Q

A substance that can dissolve in a solvent is…

A

soluble

46
Q

Two liquids that are soluble in each other in any proportion are…

A

miscible

47
Q

A substance that does not dissolve in a solvent is…

A

insoluble

48
Q

Two liquids that can be mixed but separate shortly after are…

A

immiscible

49
Q

A measure of how much solute is dissolved in a specific amount of solvent or solution.

A

concentration

50
Q

The number of moles of solute dissolved per liter of solution concentration

A

molarity (M)

51
Q

Describes solutions in terms of how many moles of solute are dissolved in a specific mass(kg) of solvent

A

molality

m

52
Q

The ratio of the number of moles of solute or solvent in solution to the total number of moles of solute and solvent

A

mole fraction

53
Q

The process of surrounding solute particles with solvent particles to form a solution

A

solvation

54
Q

The overall energy change that occurs during the solution formation process

A

heat of solution

55
Q

Occur when no more solute can be dissolved.

A

saturated solution

56
Q

Contain less dissolved solute for a given temperature and pressure than a saturated solution

A

unsaturated solution

57
Q

Contains more dissolved solute than a saturated solution at the same temperature.

A

supersaturated solution

58
Q

States that at a given temperature, the solubility of a gas in a liquid directly proportional to the pressure

A

Henry’s law

59
Q

Physical properties of solutions that are affected by the number of particles but not by the identity of dissolved particles

A

colligative property

60
Q

Due to the number of solute particles in solution and is colligative property of solutions

A

vapor pressure lowering

61
Q

The temperature difference between a solution’s boiling point and a pure solvent’s boiling point

A

boiling point elevation

62
Q

A solution’s difference in temperature between its freezing point and the freezing point of its pure solvent

A

freezing point depression

63
Q

The diffusion of a solvent through a semipermeable membrane

A

osmosis

64
Q

The amount of additional pressure cause by water molecules that moved into the concentrated solution

A

osmotic pressure

Chemistry (2 decks)

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