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Chemistry 1A > Week Ten > Flashcards

Week Ten Flashcards

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1
Q

Properties of liquids

A

strong inter molecular
free to move
cannot expand or contract significantly

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2
Q

Surface tension

A

measure of resistance of a liquid to an increase in its surface area

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3
Q

attraction of liquids on surface

A

net attractive forces that pulls them towards the interior of the liquid

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4
Q

middle of liquids - attraction

A

no net pull in any direction in the middle

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5
Q

Spherical shape of water

A

have less surface area so water is attracted to this shape

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6
Q

Forces that molecules in contact with surface have

A

adhesion

cohesion

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7
Q

adhesion forces

A

attract molecules in liquid to walls of container

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8
Q

cohesion forces

A

attract molecules in liquid to one another

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9
Q

Meniscus

A

curves surface of liquid, formed by adhesion and cohesion forces

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10
Q

strength of forces

A

adhesion forces are stronger than cohesive

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11
Q

Capillary action

A

upward movement of water against gravity

due to adhesion forces between water and oxygen

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12
Q

Viscosity

A

liquids resistance to flow

greater the viscosity, slower the liquid pours

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13
Q

What affects viscosity

A

combination of molecular shape and intermolecular forces

affected by temp

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14
Q

Viscosity vs temp

A

decreases as temp increase due to higher kinetic energy

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15
Q

Vapour pressure

A

the pressure that occurs when both the gas phase and liquid phase are happening at same time

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16
Q

vapour pressure in closed container

A

partial pressure increases as molecules enter gas phase

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17
Q

vapor pressure in open container

A

will continually lose molecules to gas phase until fully evaporated

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18
Q

Vapor pressure vs temp

A

at high temp, amount of molecules that can leave phases increases

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19
Q

liquid kinetic energy

A

have energy kinetic energy to move around within liquid phase

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20
Q

What affects vapour pressure

A

strength of intermolecular forces and temp

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21
Q

Vapor pressure - boiling liquid

A

when vapor pressure equals outside pressure, liquid will boil

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22
Q

Low pressure - vapor pressure - boiling

A

boiling point lower, pressure easily reached

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23
Q

high pressure - vapor pressure - boiling

A

boiling point increases,

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24
Q

Magnitude of forces in solids

A

forces range from large to small

can be bound by various attractive forces

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25
Q

intermolecular forces

A

molecular solids

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26
Q

covalent bonds

A

network solids

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27
Q

delocalised bonds

A

metallic solids

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28
Q

electrostatic bonds

A

ionic solids

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29
Q

Molecular solids

A

aggregates of molecules are bound by dispersion, dipolar, hydrogen bonding or combination

30
Q

Network solids

A

have high melting points
held by covalent bonds
bonding pattern determines properties

31
Q

Metallic solids

A

array of metal atoms embedded in mobile valence electrons
ductile and malleable
range of properties
properties determined by position on periodic table and number of valence electrons

32
Q

Ionic solids

A

contain cation and anions strongly attracted to each other by electrostatic forces
determined by charges

33
Q

temp during phase change

A

remains same

34
Q

what must happen for temp to change during phase change

A

substance must be completely changed

35
Q

phase changes - energy

A

require that energy is either supplied or removed from substance

36
Q

Phase change

A

transition of substance from one phase to other

depends on temp, pressure, magnitude of bonds and intermolecular forces

37
Q

molar enthalpy of melting

A

for solid to liquid

heat needed to melt 1 mole of substance at normal melting point

38
Q

Molar enthalpy of vaporisation

A

for liquid to gas

heat needed to vaporise 1 mole of substance at normal boiling point

39
Q

Molar enthalpy of sublimation

A

for solid to gas

heat needed to vaporise 1 mole of substance from solid phase

40
Q

vaporisation

A

liquid to gas

41
Q

condensation

A

gas to liquid

42
Q

fusion

A

freezing

43
Q

Sublimation

A

solid to gas

44
Q

Deposition

A

gas to solid

45
Q

Enthalpy of phase change

A

reverse processes have same magnitude but opposite signs

46
Q

Supercritical Fluids

A

form upon compression of gases at high temp or heating liquid to very high temp at high pressure

47
Q

Supercritical fluid properties

A

of both gas and liquid

48
Q

Critical point

A

density of gas and liquid phase are equal and no phase boundary
critical temp and pressure

49
Q

Phase diagrams

A

summarise phase behaviour of a substance

50
Q

Boundary lines

A

between phases that separates regions where each phase is stable

51
Q

triple point

A

where boundary lines meet at single point

52
Q

x ray diffraction

A

determines the arrangement of atoms in crystalline structure

53
Q

incoming x rays

A

atoms emit outgoing x rays

54
Q

in phase and outer phase - direction

A

in different directions

55
Q

constructive interference

A

cause diffracted beams in exposed crystals

56
Q

bragg equation

A

relates wavelength of x rays to the direction and distance between the atom planes
n(wavelength) = 2dhklsin0
where dhkl = distance between planes

57
Q

amorphous

A

when solids form rapidly and molecules are locked into irregular positions

58
Q

amorphous solids

A

dont diffract xrays

59
Q

defects in solids

A

alters properities of solid material

60
Q

ceramics

A

very hard and high melting point
dont conduct electricity
contain metals with high oxidation stat and non metals with high negative oxidation state

61
Q

hexagonal arrangment of spheres in solids

A

most dense packing

62
Q

second layer of solids

A

sit in the dimples of first layer

63
Q

third layer of solids

A

can be in same positions as first layer or in new positions

64
Q

hexagonal closed packing

A

when 3rd layer is a repeat of first layer

65
Q

cubic closed packing

A

when third layer is different to first 2 layers

66
Q

crsytal shape

A

lattice

pattern of point

67
Q

primitive cubic lattice

A

layers of atoms stacked directly above another so that all atoms lie along straight lines at right angles

68
Q

body centred cubic lattice

A

simple cube with one entire atom in the center of cube

69
Q

face centred cubic lattice

A

simple cube with atom in centre of each face of cube

70
Q

ionic crystals

A

ions of opposite charge alternate with one another to maximis attraction and minimise repulsion

71
Q

ionic solids - packing principle

A

closed packed structures formed by larger ions

smaller ions dill interstitial spaces

Chemistry 1A (12 decks)

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