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Chemistry 1110 > Lecture 7 - States of Matter: Gases, Liquids, Solids > Flashcards

Lecture 7 - States of Matter: Gases, Liquids, Solids Flashcards

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1
Q

solid has ______ shape/volume

A

definite

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2
Q

liquid has _______ shape/volume

A

indefinite

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3
Q

gas has ________ shape/volume

A

indefinite

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4
Q

solid has _____ density

A

high

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5
Q

liquid has _____ density

A

high

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6
Q

gas has _____ density

A

very low

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7
Q

solid has ______ compressibility

A

very low

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8
Q

liquid has _____ compressibility

A

very low

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9
Q

gas has _____ compressibility

A

very high

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10
Q

solid has _____ thermal expansion

A

very small

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11
Q

liquid has _____ thermal expansion

A

small

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12
Q

gas has _____ thermal expansion

A

moderate

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13
Q

particles are in constant random motion describes

A

kinetic energy

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14
Q

particles attract/repel each other describes

A

potential energy

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15
Q

particles motion ______ with temperature

A

increases

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16
Q

particles transfer energy through _____

A

collisions

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17
Q

kinetic energy = ________ = particles ______

A

disruptive force, far apart

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18
Q

potential energy = _____ = particles _____

A

cohesive, close together

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19
Q

formula to figure our how much pressure is exerted on a surface

A

P = (F/A)

p: pressure
f: force
a: area

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20
Q

Boyles Equation

A

P1V1 = P2V2

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21
Q

Boyles Law:

as pressure increases, volume _______

A

decreases

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22
Q

Charles Equation

A

V1/T1 = V2/T2

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23
Q

Charles Law:

as temperature increases, volume ______

A

increases

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24
Q

Gay-Lussac’s Equation

A

P1/T1 = P2/T2

25
Q

Gay Lussac’s Law:

as temperature increases, pressure _____

A

increases

26
Q

Combined Gas Equation

A

(P1V1)/T1 = (P2V2)/T2

27
Q

empirical gas law

A

1 mole gas = 22.4 L

28
Q

What is STP

A

Standard Temperature = 273 K

Standard Pressure = 1 atm

29
Q

Ideal Gas Equation

A

PV = nRT

30
Q

solid -> liquid

A

melting

31
Q

liquid -> gas

A

evaporation

32
Q

gas -> liquid

A

condensation

33
Q

liquid -> solid

A

freezing

34
Q

solid -> gas

A

sublimation

35
Q

gas -> solid

A

deposition

36
Q

heat is absorbed and the energy of the system increases

A

endothermic change of state

37
Q

heat energy is given off and the energy of the system decreases

A

exothermic change of state

38
Q

forces that exist between molecules

A

intermolecular forces

39
Q

forces within molecules

A

intramolecular

40
Q

which is stronger, intermolecular or intramolecular

A

intramolecular (made of covalent bonds)

41
Q

exist between polar molecules

A

dipole-dipole

42
Q

special type of extra strong dipole-dipole interaction between a hydrogen atom covalently bonded to a small, very electronegative atoms (F, O, or N) and an unshared pair of electrons on another small, very electronegative atom (F, O, N)

A

hydrogen bonding

43
Q

how to identify hydrogen bonding

A

H is bonded to N, O, or F

44
Q

the amount of heat energy required to convert the solid to liquid

A

heat of fusion

45
Q

the amount of heat energy required to convert the liquid to a gas

A

heat of vaporization

46
Q

molecules in nonpolar molecular liquids and solids are held together by weak electrostatic forces (larger molecule = stronger force)

A

London Forces

47
Q

a weak temporary intermolecular force that occurs between an atom or molecule (polar or nonpolar) and another atom or molecule (polar or nonpolar)

A

London Force

48
Q

They results from the temporary uneven e- distribution in molecules at any one moment, thus crating an instantaneous temporary dipole

A

London Force

49
Q

They are the weakest type of intermolecular force

A

London Force

50
Q

They are important because they occur between all molecules

A

London Force

51
Q

Comparing Intermolecular Forces:

  • add the the effect of London Forces and are found in polar molecules
A

Dipole-Dipole

52
Q

Comparing Intermolecular Forces:

  • the strongest intermolecular force and occurs in molecules which have H atoms bonded to F, O, or N atoms
A

Hydrogen Bonds

53
Q

Comparing Intermolecular Forces:

  • are found in all substances and are the weakest intermolecular force
A

London Force

54
Q

List the Intermolecular Forces from strongest to weakest

A

Hydrogen Bonding > Dipole-Dipole > London

55
Q

increasing the temperature of a liquid ________ its evaporation rate

A

increases

56
Q

molecules that escape (evaporate) from liquid water at room temperature

A

water vapor

57
Q

the pressure exerted by a vapor above a liquid when the liquid and vapor are in equilibrium

A

vapor pressure

58
Q

the temperature at which the vapor pressure equals the atmospheric pressure

A

boiling point

Chemistry 1110 (9 decks)

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