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chemistry > chp 14 test > Flashcards

chp 14 test Flashcards

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1
Q

intermolecular forces vs intramolecular forces

A

intermolecular- between molecules, much weaker than intramolecular forces (dispersion, dipole-dipole, hydrogen bonds)

intramolecular- within a molecule (ionic, covalent, metallic)

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2
Q

intramolecular forces

A

forces that exist within a molecule

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3
Q

intermolecular forces

A

attractive forces between molecules

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4
Q

neutral atom

A

equal number of protons and electrons

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5
Q

how can an atom lose its symmetry?

A

electrons can randomly move to one side

a charged object near the atom can cause the electrons to shift

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6
Q

what is the result of lost symmetry in an atom?

A

a dipole

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7
Q

dipole

A

a mole in which the positive and negative charges are not evenly distributed

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8
Q

induced dipole

A

one dipole can cause a neighboring atom to turn into a dipole; a neighboring atom of a dipole that becomes a dipole because of the neighboring dipole

resulting dipoles attract to each other

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9
Q

(london) dispersion force

A

force of attraction between two neighboring temporary dipoles

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10
Q

partial charges on atom cause blank dipoles

A

permanent

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11
Q

dipole-dipole forces

A

attractions between neighboring permanent dipoles

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12
Q

why are dipole-dipole forces much stronger than dispersion forces?

A

because they result from permanent (not temporary) dipoles

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13
Q

hydrogen bond

A

a really strong dipole-dipole force

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14
Q

weakest to strongest IF

A

dispersion forces
dipole-dipole forces
hydrogen bonds

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15
Q

particles of a liquid

A 
are in constant random motion
are sliding past each other
are tightly packed
are able to change positions
are NOT able to separate from one another
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16
Q

what are properties of liquids determined by?

A

nature and strength of IF between the particles

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17
Q

properties of liquids

A

definite volume- due to strong IF preventing them from separating
are fluids- IF are weak enough to allow liquids to flow
high density- IF are strong and the particles are tightly packed
incompressible- IF forces are sting and the particles are tightly packed
ability to dissolve- many solid will disolve in many liquids; IF are weak enough to allow the particles to move past each other
ability to diffuse- IF are weak enough to allow the particles to move past each other
tendency to evaporate
tendency to solidify
surface tension
viscosity

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18
Q

surface tension

A

a force that pulls adjacent molecules on the surface of a liquid together

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19
Q

relationship between surface tension and IF (and temp)

A

the greater the strength of the IF, the higher the surface tension

if temp increases, IF are weakened, surface tension decreases

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20
Q

viscosity

A

the friction or resistance to motion, between particles of a liquid as they move past each other

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21
Q

relationship between viscosity and IF (and temp)

A

the greater the IF, the higher the viscosity

if temp increases, IF are weakened, viscosity decreases

22
Q

particles of a solid

A

can only vibrate in position

are not free to move around

have very strong IF

23
Q

properties of a solid

A

high density

nonfluidity

incompressible

definitive volume and shape

tendency to melt

solids have tightly packed particles

24
Q

types of solids

A

cristallin

amorphous

25
Q

cristallin solids

A

particles arranged in a highly ordered, geometric repaying pattern

26
Q

amorphous solids

A

no repeating pattern

particles are randomly arranged

when heated, solids softens and then melts

27
Q

electron sea model

A

fixed positive ions surrounddd by mobile electrons

28
Q

properties of metals

A

good conductors of heat and electricity

malleable- easily shaped

ductile- can be drawn into wires

29
Q

what are the six state changes

A

vaporization (l—>g)
melting (s—>l)
sublimation (s—>g)

condensation (g—>l)
freezing (l—>s)
deposition (g—>s)

30
Q

which state changes are endothermic? why?

A

vaporization, melting, sublimation

all require heat to weaken or break IF

31
Q

which state changes are exothermic? why?

A

heat is released when IF get stronger

32
Q

what happens to kinetic energy in state changes?

A

always remains constant because temp remains constant during state changes; if temp is constant, KE is constant

33
Q

what happens to potential energy in state changes?

A

will increase or decrease depending on the kind of state change; PE increases in endothermic reactions and decreases in exothermic reactions

34
Q

what does it mean to be in equilibrium?

A

equilibrium is reached when the rate of evaporation equals the rate of condensation (or any other state changes)

35
Q

equilibrium

A

a dynamic condition in which two opposing changes occur at equal rates

36
Q

what happens if the equilibrium is lost between condensation and evaporation is lost because the temp increases and evaporation increases

A

condensation increase to return the system to equilibrium

37
Q

le châtelier’s principle

A

when the equilibrium of a system is lost, the system will adjust to return to equilibrium

38
Q

equilibrium vapor pressure

A

pressure = equilibrium vapor pressure

the pressure of a gas at equilibrium with its pressure

(as temp increases, the vapor pressure increases; when vapor pressure equals atmospheric pressure, the liquid boils)

39
Q

boiling point

A

when a vapor pressure equals atmospheric pressure, the liquid boils

high altitude = lower atm pressure

(a lower arm pressure is needed to boil; lower boiling pts)

40
Q

phase diagram: triple point

A

all three states of matter are in equilibrium

41
Q

phase diagram: critical point

A

the temp above which a substance will always be a gas

42
Q

strong IF prevent liquid particles from separating; which property applies to this?

A

definite volume

43
Q

IF forces in liquid particles are weak enough to allow liquids to flow; which property applies to this?

A

are fluids

44
Q

IF in liquid particles are strong, which means the particles are tightly packed; which properties apply to this?

A

high density

incompressible

45
Q

IF in liquid particles are week enough to allow the particles to move past each other; which properties apply to this?

A

ability to dissolve- many solids will dissolve in many liquids

ability to diffuse

46
Q

solids have strong IF and tightly packed particles; which properties apply to this?

A

high density

nonfluidity

incompressible

definite volume and shape

47
Q

what is the state of matter of a substance determined by?

A

the strength of the forces (IF)

48
Q

liquids: definitive volume

A

due to strong IF preventing them from separating

49
Q

liquids: are fluids

A

IF are weak enough to allow liquids to flow

50
Q

liquids: high density, incompressible

A

IF are strong, which means particles are tightly packed

51
Q

liquids: ability to dissolve, ability to diffuse

A

IF are weak enough to allow the particles to move past each other

chemistry (16 decks)

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