Physics Chap7

Question 1

Definite volume and definite shape

Answer 1

solids

Question 2

Attempts to describe all the states of matter and the conversion between states

Answer 2

Kinetic-molecular theory of matter

Question 3

Solids intermolecular forces are

Answer 3

strong enough to hold molecules rigidly in place with respect to each other

Question 4

definite volume but no definite shape

Answer 4

liquids

Question 5

strong enough to hold molecules in a condensed phase, not strong enough to prevent molecules from sliding past each other

Answer 5

intermolecular forces of liquids

Question 6

fluids have the ability to

Answer 6

flow (liquids and gases)

Question 7

Neither a definite shape nor volume

Answer 7

gases (will expand to fill the available space)

Question 8

are essentially zero between molecules

Answer 8

gas intermolecular forces (ideally independent molecules)

Question 9

what determines how molecules interact?

Answer 9

intermolecular forces (impact the macroscopic properties of a sample directly mostly)

Question 10

What determines intermolecular forces?

Answer 10

chemical bonding

Question 11

Molecules, atoms, and oppositely charged are _______ each other, but not to close. ________

Answer 11

attracted(Coulomb’s Law), REPULSION

Question 12

octet rule

Answer 12

atoms add, remove, or share electrons so as to wind up with 8 VALENCE electrons

Question 13

formed between metals and nonmetals. metals tend to form cations

Answer 13

ionic compounds

Question 14

nonmetals tend to form

Answer 14

anions

Question 15

which is stronger, ionic bonds or covalent bonds?

Answer 15

ionic bonds(almost always solids)

Question 16

ionic bond results from ________ attraction between _______ charged ions.

Answer 16

coulombic, oppositely

Question 17

on the periodic table the number of valence electrons is equal to

Answer 17

the group number

Question 18

covalent bonds result from

Answer 18

sharing of electrons

Question 19

The intermolecular forces that operate between the molecules in a sample, all of which are caused by how electrons are arranged in the molecule.

Answer 19

VSEPR Theory

Question 20

What is the most electronegative element?

Answer 20

flourine

Question 21

If two atoms of identical electronegativity are bonded together, the bond is

Answer 21

non-polar

Question 22

If two atoms of different electronegativity are bonded together, the bond is

Answer 22

polar, the electrons spend more time around the more electronegative atom (this creates partial charges)

Question 23

Three main IM forces

Answer 23

dipolar, hydrogen bonding, and London forces

Question 24

Attraction between the opposite(partial) charges of polar molecules

Answer 24

dipole-dipole attraction

Question 25

attraction between a hydrogen bonded directly to an O, N, and F and another electronegative atom

Answer 25

hydrogen bonding

Question 26

attraction between an ionic and a polar molecule

Answer 26

ion dipole attraction

Question 27

which attraction is important with how we give meds

Answer 27

ion dipole attraction (also with protein binding, albumin and alpha acidic glycoproteins)

Question 28

what is also known as Vander Waals forces

Answer 28

London forces

Question 29

result of an instantaneous dipole that is created whenever electrons in a molecule are unevenly distributed.

Answer 29

London Forces, all common matter experiences, larger molecules show more of it.

Question 30

More intermolecular forces mean what 4 things

Answer 30

-higher boiling and melting points, higher heats of fusion and vaporization, lower vapor pressure, more viscous liquids,

Question 31

IM forces also affect solubility, | "like dissolves....

Answer 31

"like"

Question 32

polar compounds dissolve more easily in other _______ compounds

Answer 32

polar. "like dissolves like"

Question 33

The ultimate in ______ species, are soluble in water, but are generally not soluble in _______ organic solvents such as ether.

Answer 33

polar, nonpolar

Question 34

what are some nonpolar species

Answer 34

nitrogen, oxygen, and CO2, (relatively insoluble in a polar solvent like water)

Question 35

Most organic compounds have backbones consisting of hydrogen and carbon. Hydrocarbons are essentially _________. Therefore, most organic compounds are not very soluble in ______.

Answer 35

nonpolar, water.

Question 36

Substances with ______ IM attractions have _______ surface tensions.

Answer 36

greater, greater

Question 37

does water have a high or low surface tension?

Answer 37

high

Question 38

laplaces law

Answer 38

wall surface tension is directly proportional to radius if pressure is the same. tension=radiusxpressure

Question 39

aneurysms are _______, and radius of aneurysm is divided by

Answer 39

spherical, 2,

Question 40

soaps are derived directly from fats or oils through a chemical process called

Answer 40

saponification

Question 41

what is a fatty acid?

Answer 41

a long-chained carboxylic acid having 12-18 carbon atoms.

Question 42

a soap is the salt of a

Answer 42

fatty acid

Question 43

when placed into water the surfactant molecule will strive to get the greasy, nonpolar ______ tail away from the ______ water molecules.

Answer 43

hydrocarbon, polar.

Question 44

what does surfactant disrupt to decrease the surface tension of the water? (monolayers)

Answer 44

disrupt the hydrogen bonding between water molecules

Question 45

the surfactant molecules stick their polar heads onto the water, while their greasy tails stick out of the surface of water

Answer 45

monolayers

Question 46

the tails of the surfactant molecules can dissolve in each other to form a double layer. the nonpolar tails interact with eachother, with the polar heads on the outside interacting with the water molecules

Answer 46

bilayers and basic structure of cell membranes

Question 47

tails can dissolve in each other forming a sphere, crating a non-polar microenvironment in the water is called

Answer 47

micelles

Question 48

Viscosity ______ with increasing intermolecular forces.

Answer 48

increases

Question 49

Substances having ______ IM forces have ______ vapor pressures

Answer 49

greater, lower

Question 50

The most energetic molecules in a liquid have sufficient kinetic energy to break IM forces and escape into the gas phase. Once the molecules are free as gases, they exert a pressure called

Answer 50

the vapor pressure

Question 51

vapor pressure is _______ proportional to temp

Answer 51

directly

Question 52

volatility of a liquid ______ with increasing temp

Answer 52

increases

Question 53

When there is a balance between vaporization and condensation, a state of ______ ________ exists

Answer 53

dynamic equilibrium

Question 54

Des has to be heated to ______ roughly to keep in _____ state

Answer 54

2atm, liquid

Question 55

Is a gas more volatile with a high or low vapor pressure?

Answer 55

high

Question 56

volatility is

Answer 56

nonquantaitative term that describes the tendency of a liquid to evaporate

Question 57

what describes the distribution of why vapor pressure increases with temp?

Answer 57

Boltzmann distribution

Question 58

states the total pressure of a gaseous mixture is the sum of the partial pressures of each of the component gases.

Answer 58

Dalton's Law of Partial Pressures

Question 59

vapor pressure is ______ dependent

Answer 59

temperature

Question 60

liquid to gas

Answer 60

vaporiztion

Question 61

gas to liquid

Answer 61

condensation

Question 62

solid to gas

Answer 62

sublimation

Question 63

gas to solid

Answer 63

deposition

Question 64

boiling point is _____ at higher elevation

Answer 64

lower, since less atm pressure to overcome

Question 65

temperature at which the vapor pressure of a liquid equals the ambient pressure

Answer 65

boiling point