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misc > Physics Chap7 > Flashcards

Physics Chap7 Flashcards

1
Q

Definite volume and definite shape

A

solids

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2
Q

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

A

Kinetic-molecular theory of matter

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3
Q

Solids intermolecular forces are

A

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

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4
Q

definite volume but no definite shape

A

liquids

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5
Q

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

A

intermolecular forces of liquids

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6
Q

fluids have the ability to

A

flow (liquids and gases)

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7
Q

Neither a definite shape nor volume

A

gases (will expand to fill the available space)

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8
Q

are essentially zero between molecules

A

gas intermolecular forces (ideally independent molecules)

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9
Q

what determines how molecules interact?

A

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

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10
Q

What determines intermolecular forces?

A

chemical bonding

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11
Q

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

A

attracted(Coulomb’s Law), REPULSION

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12
Q

octet rule

A

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

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13
Q

formed between metals and nonmetals. metals tend to form cations

A

ionic compounds

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14
Q

nonmetals tend to form

A

anions

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15
Q

which is stronger, ionic bonds or covalent bonds?

A

ionic bonds(almost always solids)

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16
Q

ionic bond results from ________ attraction between _______ charged ions.

A

coulombic, oppositely

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17
Q

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

A

the group number

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18
Q

covalent bonds result from

A

sharing of electrons

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19
Q

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

A

VSEPR Theory

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20
Q

What is the most electronegative element?

A

flourine

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21
Q

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

A

non-polar

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22
Q

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

A

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

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23
Q

Three main IM forces

A

dipolar, hydrogen bonding, and London forces

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24
Q

Attraction between the opposite(partial) charges of polar molecules

A

dipole-dipole attraction

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25
Q

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

A

hydrogen bonding

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26
Q

attraction between an ionic and a polar molecule

A

ion dipole attraction

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27
Q

which attraction is important with how we give meds

A

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

28
Q

what is also known as Vander Waals forces

A

London forces

29
Q

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

A

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

30
Q

More intermolecular forces mean what 4 things

A

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

31
Q

IM forces also affect solubility,

“like dissolves….

A

“like”

32
Q

polar compounds dissolve more easily in other _______ compounds

A

polar. “like dissolves like”

33
Q

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

A

polar, nonpolar

34
Q

what are some nonpolar species

A

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

35
Q

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

A

nonpolar, water.

36
Q

Substances with ______ IM attractions have _______ surface tensions.

A

greater, greater

37
Q

does water have a high or low surface tension?

A

high

38
Q

laplaces law

A

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

39
Q

aneurysms are _______, and radius of aneurysm is divided by

A

spherical, 2,

40
Q

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

A

saponification

41
Q

what is a fatty acid?

A

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

42
Q

a soap is the salt of a

A

fatty acid

43
Q

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

A

hydrocarbon, polar.

44
Q

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

A

disrupt the hydrogen bonding between water molecules

45
Q

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

A

monolayers

46
Q

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

A

bilayers and basic structure of cell membranes

47
Q

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

A

micelles

48
Q

Viscosity ______ with increasing intermolecular forces.

A

increases

49
Q

Substances having ______ IM forces have ______ vapor pressures

A

greater, lower

50
Q

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

A

the vapor pressure

51
Q

vapor pressure is _______ proportional to temp

A

directly

52
Q

volatility of a liquid ______ with increasing temp

A

increases

53
Q

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

A

dynamic equilibrium

54
Q

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

A

2atm, liquid

55
Q

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

A

high

56
Q

volatility is

A

nonquantaitative term that describes the tendency of a liquid to evaporate

57
Q

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

A

Boltzmann distribution

58
Q

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

A

Dalton’s Law of Partial Pressures

59
Q

vapor pressure is ______ dependent

A

temperature

60
Q

liquid to gas

A

vaporiztion

61
Q

gas to liquid

A

condensation

62
Q

solid to gas

A

sublimation

63
Q

gas to solid

A

deposition

64
Q

boiling point is _____ at higher elevation

A

lower, since less atm pressure to overcome

65
Q

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

A

boiling point

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