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Chemistry > Unit Six > Flashcards

Unit Six Flashcards

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1
Q

Liquid

A

Medium packed particles, medium motion

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2
Q

Gas

A

Loosely packed particles, high motion

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3
Q

Temperature

A

A measure of the average kinetic energy particles of a substance have

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4
Q

Heat

A

Transfer of kinetic energy from a hotter object to a cooler one

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5
Q

Melting

A

Solid to liquid

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6
Q

Freezing

A

Liquid to solid

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7
Q

Vaporization

A

Liquid to gas

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8
Q

Condensation

A

Gas to liquid

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9
Q

Sublimation

A

Gas to solid

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10
Q

Deposition

A

Solid to gas

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11
Q

Fahrenheit to Celsius

A

F = 1.8 C + 32

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12
Q

Celsius to Fahrenheit

A

C = (F - 32)/1.8

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13
Q

Celsius and Kelvin

A

K = C + 273

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14
Q

Pressure conversions

A

1 atm = 14.7 psi = 101 kPa = 7.60x10^2 mm Hg (torr)

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15
Q

STP

A

Standard temperature and pressure, 1 atm and 273 K

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16
Q

Intramolecular forces

A

Hold the atoms of a molecule together

Ex. Ionic bonds, polar covalent bonds, nonpolar covalent bonds

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17
Q

Intermolecular forces

A

Hold molecules of a substance together

Ex. Dipole-dipole, hydrogen bonding, dispersion forces

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18
Q

Dispersion forces

A

Weak forces resulting from temporary shifts in electron densities, stronger for larger particles
In nonpolar molecules, bigger molecules = bigger force
Weakest type of intermolecular bonds

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19
Q

Dipole-dipole forces

A

Attraction between oppositely charged region of polar molecules
Polar covalent
Middle strength

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20
Q

Hydrogen bonds

A

Dipole-dipole attraction occurring between molecules containing hydrogen boned to fluorine, oxygen, or nitrogen
Strongest because greatest difference in electronegativity
Polar covalent
Strongest type

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21
Q

Are hydrogen bonds or ionic bonds stronger

A

Ionic because hydrogen is partial charges and ionic is full charges

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22
Q

Liquid density

A

Denser than gases

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23
Q

Liquid compression

A

Cannot compress a liquid (definite volume)

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24
Q

Liquid fluidity

A

Particles in a liquid do not have fixed locations

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25
Q

Liquid viscosity

A

A measure of resistance of a liquid to flow

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26
Q

Factors affecting viscosity

A

Stronger intermolecular forces mean greater viscosity
Larger and longer molecules will form more viscous solutions
Viscosity decreases with temperature

27
Q

Surface tension

A

Energy required to increase the surface area of a liquid
Because intermolecular forces at the center of the liquid experience balanced attractions on all sides while molecules at the surface are only pulled inward, thus creating a taught surface

28
Q

Cohesion

A

Attraction between identical molecules

29
Q

Adhesion

A

Attraction between different molecules

30
Q

Capillary action

A

What happens when the adhesion forces overcome the cohesion forces

31
Q

Solid

A

Closely packed particles, low motion

32
Q

Special properties of water due to hydrogen bonding

A

High melting and boiling point (takes more energy to line up or separate hydrogen bonds)
Surface tension and capillary action (strength of hydrogen bonds pulls them to the center of the liquid and towards one another and their container)
Solid water is less dense than liquid water (when cooled hydrogen bonds align in a spacious crystal pattern that makes the ice less dense than the water bc of liquid molecules)
Universal solvent (neutral, no net charge, can dissolve most things)

33
Q

Crystalline solids

A

Atoms, ions, or molecules in an orderly, geometric structure

34
Q

Molecular solid

A

Covalent substance, break down easily, soft, low melting points, water, sugar, dry ice

35
Q

Covalent network solid

A

Crystal structure, carbon, silica

36
Q

Ionic solid

A

Soluble, high melting points, salts

37
Q

Metallic solid

A

Orderly atoms, ductile, malleable, any metal

38
Q

Allotropes

A 
Multiple different forms of the same state
Ex carbon (diamond, graphite, etc)
39
Q

Amorphous solids

A

Solid where particles are not arranged in a repeating pattern
Ex obsidian, glass rubber

40
Q

Properties of gases

A

Gases are fluids
Gases are highly compressible
Gases completely fill containers
Gases have lower densities than liquid and solids

41
Q

KMT

A

Kinetic molecular theory, describes the motion of particles
Gas molecules are in constant, random motion
Gas molecules are separated by huge distance relative to the size of the molecules themselves
Gas molecules have no attractive/repulsive forces
Gases are made of molecules that have mass
Molecules undergo elastic collisions

42
Q

Relationship between temperature and kinetic energy

A

Temperature and energy of molecules are directly proportional
If temperature increases the kinetic energy increases

43
Q

Boyle’s law

A

P1V1 = P2V2, inverse relationship

44
Q

Charles law

A

V1/T1 = V2/T2, direct relationship

45
Q

Gay-Lussac law

A

P1/T1 = P2/T2, direct relationship

46
Q

Avogadro law

A

22.4 L = 1 mole gas

47
Q

Combined gas law

A

P1V1/T1 = P2V2/T2

48
Q

Ideal gas law

A 
PV = nRT
P = pressure in atm
V = volume in liters
n = moles
R = 0.08205 if atm, 8.31 if kPa
T = temperature in kelvin
49
Q

Ideal gas

A

Gases that behave according to the assumptions of kinetic molecular theory

50
Q

Assumptions made for ideal gases

A

No intermolecular forces

Individual molecules have no volume

51
Q

Conditions where real gases behave ideally

A

High temperature and low pressure

52
Q

Diffusion

A

Gas particles will travel from an area of high concentration to an area of low concentration until they are evenly distributed

53
Q

Effusion

A

Passage of a gas through a small hole/opening in a barrier

54
Q

Graham’s law of effusion

A

Gases that have larger molar masses move more slowly than lighter gases

55
Q

Avogadro’s hypothesis

A

Equal volumes of gases at the same temperature and pressure contain equal number of particles

56
Q

Other things about Avogadro’s hypothesis

A

Due mainly to the large amount of empty space between particles
From this, scientists have determined that one mole of gas = 22.4 L at STP

57
Q

Dalton’s law of partial pressure

A

The total pressure for a mixture of gases is equal to the sum of the pressures of the individual gases in the mixture
Ptotal = P1 + P2 + Px

58
Q

On a phase diagram, the top third is

A

Solid

59
Q

On a phase diagram, the middle third is

A

Liquid

60
Q

On a phase diagram, the bottom third is

A

Gas

61
Q

Triple point

A

The temperature and pressure where all three phases of matter could exist
Where the three lines converge and meet at a single point

62
Q

Critical point

A

Pressure and temperature above which distinct gas and liquid phases don’t exist

63
Q

Density formula

A

D = m/v

Chemistry (12 decks)

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