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CH301 > Unit 4: IMFs & Thermodynamics > Flashcards

Unit 4: IMFs & Thermodynamics Flashcards

1
Q

forces between particles (atoms, molecules, or ions) of a substance are called ________________

A

intermolecular forces

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2
Q

bonds within molecules or formula units are called __________________

A

intramolecular forces

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3
Q

the dominant forces between molecules are _____________

A

electrostatic

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4
Q

dispersion forces are __________ and _____________ attractive forces between _____________ dipoles

A

very weak, very short range, temporary (induced)

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5
Q

dispersion forces are the only forces between ___________ molecules

A

nonpolar

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6
Q

dispersion forces are also called

A

London forces, van der Waals, or induced dipoles

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7
Q

dispersion forces are __________ rather than ______________ dipole-dipole interactions

A

temporary; permanent

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8
Q

polarizability ___________ with increasing numbers of electrons and, therefore, with increasing sizes of molecules

A

increases

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9
Q

London forces are generally ____________ for molecules that are larger or have more electrons

A

stronger

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10
Q

IMF result from attractive forces between regions of ____________ and ____________ charge density in neighboring molecules

A

positive, negative

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11
Q

_________ interactions are so strong, they can even be considered intermolecular forces as well as intramolecular forces

A

ionic

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12
Q

surface tension describes the inward forces that must be overcome in order to ________ the surface area of a liquid

A

expand

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13
Q

viscosity increases as IMFs __________ in strength and as the temperature __________

A

increase; decreases

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14
Q

the vapor pressure of all liquids ___________ with temperature

A

increases

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15
Q

at room temperature, a liquid with ______ vapor pressure is called volatile

A

high

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16
Q

diamond is a __________ crystal of carbon

A

covalent

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17
Q

diamond and graphite are two _____________ forms of carbon

A

crystalline

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18
Q

graphite forms __________ while diamond is ______________

A

flat sheets; tetrahedral

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19
Q

the electrons in metallic solids are _____________

A

delocalized to form a “sea of electrons” that allow electricity (the movement of electrons) to flow freely

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20
Q

First Law of Thermodynamics: During any physical or chemical change, the total amount of energy in the universe is __________

A

conserved (Law of Conservation of Energy)

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21
Q

Total energy = __________ + ____________

A

kinetic energy, potential energy

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22
Q

Total energy = __________ = ___________ + ___________

A

internal energy, heat energy, work energy

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23
Q

State functions are a property of the system whose value depends ONLY on the __________ and ___________ states of system

A

initial, current
(symbols are capital letters)

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24
Q

usually the reaction: the reactants and products

A

system

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25
Q

the rest: the beaker, the air in the room, etc

A

surroundings

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26
Q

system + surroundings

A

universe

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27
Q

open system

A

exchange energy & matter

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28
Q

closed system

A

exchange energy only

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29
Q

isolated system

A

no exchange of energy or matter

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30
Q

isothermal

A

constant temperature

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31
Q

adiabatic

A

constant heat

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32
Q

isobaric

A

constant pressure

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33
Q

Internal energy is the sum of the _________ and ___________ energy of all _________ in the system

A

kinetic
potential
particles

34
Q

endothermic reaction:
sign for q:

A

absorbing heat, q > 0

35
Q

exothermic reaction:
sign for q:

A

gives off heat, q < 0

36
Q

positive work is work done __ system __ surroundings
volume is __________

A

on, by, decreasing

37
Q

negative work is work done __ system __ surroundings
volume is ___________

A

by, on, increasing

38
Q

specific heat is how much _________ is required to heat ____________ of a substance by one degree

A

heat, one gram

39
Q

heat of fusion is how much heat is required ________ __________ of a substance without changing the ___________

A

to melt one gram, temperature

40
Q

heat of vaporization is how much heat is required to __________ ________ of a substance without changing the ____________

A

vaporize one gram, temperature

41
Q

sublimation

A

solid to gas

42
Q

deposition

A

gas to solid

43
Q

unit for heat of vaporization

A

J/g

44
Q

___________ is heat at constant pressure

A

enthalpy change (∆H)

45
Q

heat of combustion is the _________ change for the combustion reaction in which _____ mole of the fuel is reacted

A

enthalpy, one

46
Q

calorimetry

A

an experimental technique to measure the energy change associated with a chemical or a physical process

47
Q

bomb calorimeter = constant ___________

A

volume

48
Q

coffee cup calorimeter = constant _____________

A

pressure

49
Q

standard ________ enthalpies of formation is enthalpy for reaction in which ____________ of a substance in a specified state is formed from its constituent elements in their ___________

A

molar, one mole, standard states

50
Q

larger atoms and molecules are more __________ than smaller atoms and molecules

A

polarizable

51
Q

__________ IMFs = most ideal gas

A

weaker

52
Q

the stronger the IMFs, the ________ the vapor pressure

A

weaker

53
Q

_________ IMFs = more viscosity

A

stronger

54
Q

nonmetals that melt below 500K are __________ solids

A

molecular

55
Q

nonmetals that melt above 500K are _________ solids

A

covalent

56
Q

breaking bonds ______ energy

A

absorbs

57
Q

forming bonds _______ energy

A

gives off

58
Q

ion-ion forces have a full and __________ charge

A

permanent

59
Q

hydrogen bonding has a partial and __________ charge

A

permanent

60
Q

third law of thermodynamics: the entropy of a ____________, _________________ substance at ____________ is zero

A

pure, perfect crystalline, absolute zero

61
Q

Gibbs Free Energy will always be ________ for spontaneous processes

A

negative

62
Q

when free energy is greater than zero, it is ______ stable

A

less

63
Q

when free energy is less than zero, it is _______ stable

A

more

64
Q

in a combustion reaction, heat is always ___________

A

released

65
Q

condensation

A

gas to liquid

66
Q

vaporization

A

liquid or solid to gas

67
Q

evaporation

A

liquid to gas

68
Q

for a given reaction, if ∆H (enthalpy change of the reaction) is _____________ and ∆S (entropy change) is ___________, then the value of ∆G (free energy) will ALWAYS BE NEGATIVE

A

negative, positive

69
Q

_________ law of thermodynamics: all _____________ changes are accompanied by an ___________ in universal entropy

A

second, spontaneous, increase

70
Q

reactions that occur spontaneously in one direction cannot occur spontaneously in the ___________ direction

A

reverse

71
Q

non-spontaneous means that entropy change is __________

A

negative

72
Q

entropy is a _____________ function that is a measure of the ____________ of energy

A

state, dispersal

73
Q

elements in their ____________ states will have change of free energy (∆G) equal to ___________

A

standard, zero

74
Q

third law of thermodynamics

A

the entropy of a pure, perfect crystalline substance at absolute zero is zero

75
Q

first law of thermodynamics (law of conservation of energy)

A

during any physical or chemical change, the total amount of energy in the universe is conserved

76
Q

standard states

A

how elements exist when they are at 1 atm pressure and 25 degrees Celsius

77
Q

molar heat of formation

A

the enthalpy change for the formation of one mole of product from its elements in their standard states

78
Q

the change in internal energy, ∆U, for a process is equal to the amount of heat __________ at constant ____________

A

absorbed, volume

79
Q

the change in enthalpy, ∆H, for a process is equal to the amount of heat ____________ or _____________ at constant __________

A

absorbed, released, pressure

80
Q

for a _____________ change, a positive change in entropy for the system is matched by a negative entropy change for the surroundings

A

physical

CH301 (4 decks)

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