Chem 2 Exam 1

Front 1

solids can be changed to gases by adding energy

Back 1

sublimation

Front 2

solids can be changed to liquids by adding energy

Back 2

melting

Front 3

liquids can be changed to gases by adding energy

Back 3

vaporization

Front 4

liquids can be frozen to solids by removing energy

Back 4

freezing

Front 5

gases can be condensed to liquids by removing energy

Back 5

condensation

Front 6

gases can be condensed to solids by removing energy

Back 6

deposition

Front 7

pressure and volume are inversely proportional

Back 7

boyles law

Front 8

volume and temperature are directly proportional

Back 8

charles law

Front 9

as the number of moles increases, the volume will increase as well

Back 9

avogadros law

Front 10

temperature and pressure are directly proportional

Back 10

gay-lussac law

Front 11

when do gases deviate from ideal behavior?

Back 11

low temperature and high pressure

Front 12

the mvmt of a gas into a vacuum

Back 12

effusion

Front 13

the gradual mixing of two or more gases

Back 13

diffusion

Front 14

short-range attractive forces operating between the particles that make up the units of a liquid or solid substance

Back 14

intermolecular forces

Front 15

attractive forces between two oppositely charged ions

Back 15

ion-ion

Front 16

attractive forces between an ion and a permanent dipole in a polar compound

Back 16

ion-dipole

Front 17

attractive interactions between polar molecules

Back 17

dipole-dipole

Front 18

very weak and very short-range attractive forces between temp dipoles

Back 18

london dispersion

Front 19

a dipole-dipole interaction between molecules containing hydrogen directly bonded to N, O, or F

Back 19

hydrogen bonding

Front 20

what intermolecular forces does HF have?

Back 20

dipole-dipole, dispersion, and hydrogen bonding

Front 21

what intermolecular forces does HCl have?

Back 21

dispersion and dipole-dipole

Front 22

diffuse freely into one another and form a homogenous solution (alcohol and water)

Back 22

miscible

Front 23

do not diffuse freely into one another and do not form a homogenous solution (oil and water)

Back 23

immiscible

Front 24

a measure of the ability of a liquid to evaporate quickly

Back 24

volatility

Front 25

the stronger the intermolecular forces, the ______ the viscosity

Back 25

higher

Front 26

forces that bind molecules to each other

Back 26

cohesive forces

Front 27

forces that bind molecules to a surface

Back 27

adhesive forces

Front 28

adesive forces > cohesive forces

Back 28

U-shaped (concave)

Front 29

cohesive forces > adhesive forces

Back 29

curved downwords (convex)

Front 30

capillary rise implies that…..

Back 30

adhesive forces are greater than cohesive forces

Front 31

capillary fall implies that

Back 31

cohesive forces are greater than adhesive forces

Front 32

the pressure exerted by a vapor in equilibrium with its liquid or solid phase

Back 32

vapor pressure

Front 33

temp at which the vapor pressure of the liquid equals the applied pressure

Back 33

boiling point

Front 34

what are the ways to get a liquid to boil?

Back 34

increase temp and decrease pressure

Front 35

solids composed of structural units bounded by specific (regular) geometric patterns; characterized by sharp melting points

Back 35

crystalline solid

Front 36

substances that do not display geometric regularity in the solid; do not have sharp melting points, but melt over a wide range of temps

Back 36

amorphous solids

Front 37

atoms at the corners of a simple cube

Back 37

primitive cubic

Front 38

atoms at the corners of a cube plus one in the center of the body of the cube

Back 38

body-centered cubic

Front 39

atoms at the corners of a cube plus one atom in the center of each face of the cube

Back 39

face-centered cubic

Front 40

discrete molecules that occupy positions in unit cells; attraction forces weak; usually soft and low melting points

Back 40

molecular solids

Front 41

positive and negative ions arranged in a definite crystal structure; strong attraction; hard; high melting points

Back 41

ionic solids

Front 42

individual atoms are covalently bonded to several other atoms; usually hard and high melting point

Back 42

covalent solids

Front 43

positively charged nuclei imbedded in a sea of electrons; hardness varies but usually have high melting points

Back 43

metallic solids

Front 44

what type of solid is CO2?

Back 44

molecular

Front 45

what type of solid is ice?

Back 45

molecular

Front 46

what type of solid is NaCl?

Back 46

ionic

Front 47

what type of solid is a diamond?

Back 47

covalent

Front 48

what type of solid is sand?

Back 48

covalent

Front 49

what type of solid is potassium?

Back 49

metallic

Front 50

what type of solid is aluminum?

Back 50

metallic