Chemistryii

Front 1

A liguid forms when a gas________

Back 1

condenses

Front 2

A liquid forms at a very _____ _____ and/or ____ _____
Avg. intermolecular attraction> average kinetic energy.
molecules are ________
and are in constant motion. some molecules have enough energy to slide past each other.

Back 2

low temperature or high pressure

Front 3

Liquid properties:
1.
2.
3.
4

Back 3

compressibility
viscosity
surface tension
capillary action

Front 4

Liquids are hard to compress. they are ____
and resist moving closer

Back 4

close together

Front 5

High viscosity=
low viscosity ex
high viscosity ex

Back 5

low flow
water
honey

Front 6

____ viscosity is caused by:
• Large intermolecular attractions.
• Large entanglement of molecules

Back 6

high

Front 7

higher T=

Back 7

lower viscosity

Front 8

• It takes energy to move past another molecule.
• Increase in T = increase in average Ek.
• Greater fraction of the molecules have enough Ek to slide
past each other (overcome intermolecular forces).

Back 8

low viscosity

Front 9

Liquid molecules attract each other.
Molecules at a surface experience
unbalanced forces. They are not as
well stabilized;
energy required to form a surface

Back 9

surface tension

Front 10

smaller surface area=
large intermolecular forces=

Back 10

higher stability
high surface tension

Front 11

The object with the smallest surface/volume ratio is a

Back 11

sphere

Front 12

___ forces between a surface and a liquid.

Front 13

____forces between liquid molecules.

Front 14

The shape of the ___tells us the relative
strength of the adhesive and cohesive forces

Back 14

meniscus

Front 15

The tendency to vaporize is a liquid’s ____.
as temperature ___, a liquid becomes more volatile

Back 15

volatility
increases

Front 16

at some time evaporation rate= __ rate

Back 16

condensation

Front 17

Equilibrium vapor pressure depends upon:

Back 17

1. intermolecular forces in the liquid
2. temperature

Front 18

it is independent of the:
1
2

Back 18

v of the liquid or vapor
surface area of the liquid

Front 19

a liquid boils when the vapor P= ____ P

Back 19

atmospheric pressure

Front 20

Evaporation is ___

Back 20

endothermic

Front 21

condensation is__

Back 21

exothermic

Front 22

the heat required to completely vaporize one mole of a substance at its boiling point

Back 22

molar heat of vaporization

Front 23

the heat released when one mole of a substance condenses at its boiling point

Back 23

molar heat of condensation

Front 24

in a solid:
molecules are ___
and in constant motion

donot have enough energy to slide past each other

Back 24

close

Front 25

melting is

Back 25

endothermic

Front 26

freezing is

Back 26

exothermic

Front 27

the heat required to melt one mole of a substance at its melting point

Back 27

molar heat of fusion

Front 28

the heat released when one mole of a substance cystallizes at its melting point

Back 28

molar heat of crystallization

Front 29

three phases in equilibrium

Back 29

triple point

Front 30

the end of the liquid/gas equilibrium line. It occurs at the critical temperature and critical pressure

Back 30

critical point

Front 31

above the critical temperature the substance is neither a liquid nor a gas.

Back 31

it is a supercritical fluid

Front 32

has a density similar to a liquid and a viscosity similar to a gas

Back 32

supercritical fluid

Front 33

can absorb/release large amounts of heat-moderates temperature

Back 33

specific heat capacity

Front 34

heat release on freezing protects crops

Back 34

heat of fusion

Front 35

water vapor contains large amounts of energy; heat release on condensation fuels storms

Back 35

heat of vaporization

Front 36

helps capillary action in plants

Back 36

surface tension

Front 37

fast energy transfer, rapid cooling of organisms

Back 37

thermal conductivity

Front 38

long-range order; sharp melting points; they relfect on the shape of the lattice
examples: ice,table salt, gems

Back 38

crystalline solid

Front 39

no regular repeating units; melt over a range of temperature; examples: glass,plastics,ceramics

Back 39

amorphous solid

Front 40

ionic forces hold positive and negative ions together. hard, brittle, high mp, often water soluble

Back 40

ionic solids

Front 41

metallic bonding; electrostatic attraction between metal ions and electrons. Malleable, ductile, good heat/electrical conduction, wide range of hardness and mp

Back 41

metallic solids

Front 42

london forces, dipole/dipole attraction, and hydrogen bonding. low to moderate, soft, poor conductors

Back 42

molecular solids

Front 43

covalent bonds hold atoms in infinite arrays, wide range of properties; diamonds; graphite

Back 43

network

Front 44

the smallest part of a lattice that can be used to construct the full lattice is the

Back 44

unit cell

Front 45

the atoms in a layer sit at the corners of the squares

8*1/8

Back 45

simple cubic

Front 46

an extra atom sits in the center of the cell(unshared)
8*1/8 +1=2 68% of the space is occupied

Back 46

cubic cells

Front 47

each face has 1 atom in the center

6*1/2+8*1/8=4

74% of the space is filled by atoms

Back 47

face-centered cubic

Front 48

have one valence electron, in s orbital

Back 48

alkali metals

Front 49

formed by the interaction of low-lying, empty atomic orbitals

Back 49

conduction band

Front 50

valence and conduction bands overlap. lots of open levels. electrons can move freely

Back 50

metal

Front 51

filled valence band;large band gap, electrons cannot jump the gap no conduction

Back 51

insulator

Front 52

filled valence band. narrow band gap. some electrons can jump the gap.. higher temperature= more energetic electrons=better conductor

Back 52

semiconductor

Front 53

Metals are better conductors at low T. superconductors have zero resistance at some temperatures

Back 53

bla

Front 54

exs of amorphous solids

Back 54

cement, concrete,cermaics,silicate ceramics,