2009-2010 Chemistry Kinetic Theory Of Matter

Front 1

what are the 3 assumptions of the kinetic theory?

Back 1

1. all matter is made up of tiny particles.
2. these particles are in Constant motion (theoretically molecular otion ceases at absolute zero).
3. the collisions that occur between the particles are elastic, meaning no net loss of energy

Front 2

it is very _____ to compress a liquid.

Back 2

hard

Front 3

The density of liquids is ______ than the densities of gases.

Back 3

greater

Front 4

the measure of disorder is called

Back 4

entropy

Front 5

As liquids are cooled, kinetic energy is ____.

Back 5

lowered

Front 6

in liquids, particles vibrate about ____ points

Back 6

moving

Front 7

solids vibrate about ____ points

Back 7

fixed

Front 8

____ are practically incompressible

Back 8

solids

Front 9

solids diffuse...

Back 9

very slowly

Front 10

the major factor that determines the physical state of a substance at room temp is

Back 10

intermolecular forces

Front 11

____ is useful in determining if a bond is to be classified as nonpolar covalent, polar covalent or ionic.

Back 11

electronegativity

Front 12

a bond between a metal and a nonmetal...

Back 12

ionic

Front 13

a bond between 2/more nonmetals

Back 13

covalent

Front 14

electronegativity difference of nonpolar covalent

Back 14

less than/equal to .3 (or .5)

Front 15

electronegativity difference of polar covalent

Back 15

greater than .3/.5 up to 1.6/1.7

Front 16

electronegativity difference of ionic

Back 16

equal or greater to 2.0

Front 17

3 types of intermolecular forces of attraction

Back 17

dipole-dipole
hydrogen bonding
london dispersion forces

Front 18

dipole-dipole forces

Back 18

strongest of the I.F./ between two polar molecules

Front 19

hydrogen bonding

Back 19

very stong dipole-dipole reaction/
occurs when H is bonded to a highly electronegative element/
causes a high boiling point

Front 20

London Dispersion Forces

Back 20

weakest of the IF/
induced (temporary dimples)/
found in NONPOLAR substances and noble gases/
Stronger for larger molecules (or ones that have more electrons)/ higher boiling point

Front 21

liquids with like polarities will _____

Back 21

dissolve

Front 22

the measure of how fluid a liquid is

Back 22

viscosity

Front 23

a low viscosity means that the liquid runs _____

Back 23

easily

Front 24

the higher IF the ______ the viscosity

Back 24

higher

Front 25

surface tension is the

Back 25

energy required to increase the surface area of a liquid by a given amount

Front 26

Ionic bonds have ____ melting points and ____ boiling points

Back 26

high/high

Front 27

ionic bonds conduct ___ only when melted or dissolved

Back 27

electricity

Front 28

Ionic bonds are ____ soluble

Back 28

water

Front 29

ionic bonds are insoluble in _____ solvents

Back 29

non-polar

Front 30

non-polar molecular bonds have _____ forces between units

Back 30

dispersion

Front 31

nonpolar molecular bonds have ___ melting points and boiling points

Back 31

low

Front 32

nonpolar molecular bonds are nonconducting and _____ in H20

Back 32

insoluble

Front 33

nonpolar molecular bonds are soluble in ____ substances

Back 33

nonpolar

Front 34

polar molecular bonds have all _ IF forces between units

Back 34

3

Front 35

polar molecular bonds have ____ melting point and boiling than non-polar covalent solids

Back 35

higher

Front 36

polar molecular bonds conducting or nonconducting?

Back 36

nonconducting

Front 37

polar molecular bonds are likely to be soluble in ____ solvents

Back 37

polar

Front 38

covalent network solids have ____ bonds between units

Back 38

covalent

Front 39

covalent network solids are ___ and solid

Back 39

hard

Front 40

covalent network solids have a very ____ melting point

Back 40

high

Front 41

covalent network solids are conductors or nonconductors?

Back 41

non-conductors

Front 42

covalent network solids are _______ in common solvents

Back 42

insoluble

Front 43

an example of covalent network solids are

Back 43

diamond/ quartz

Front 44

metallic substances have relatively ___ melting points

Back 44

high

Front 45

metallic substances are ____ in common solvents

Back 45

insoluble

Front 46

metallic substances are malleable and ___

Back 46

ductile

Front 47

metallic substances are ____ conductors of electricity

Back 47

good

Front 48

metallic substances ___ react with H20

Back 48

may

Front 49

list the bonds from weakest to strongest

Back 49

-dispersion
-dipole
-H bonding
-Metallic Ionic
-Covalent Bonds

Front 50

In melting, is NRG required or released?

Back 50

required

Front 51

in vaporization, is NRG required or released?

Back 51

required

Front 52

in sublimation, is NRG required or released?

Back 52

required

Front 53

in freezing, is NRG required or released?

Back 53

released

Front 54

in condensation, is NRG required or released?

Back 54

released

Front 55

in solidification, is NRG required or released?

Back 55

released

Front 56

What is the phase change of melting?

Back 56

solid-liquid

Front 57

What is the phase change of vaporization?

Back 57

liquid-gas

Front 58

What is the phase change of sublimation?

Back 58

solid-gas

Front 59

What is the phase change off freezing?

Back 59

liquid-solid

Front 60

What is the phase change of condensation?

Back 60

gas-liquid

Front 61

What is the phase change of solidification?

Back 61

gas-solid