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Chemistry > 13.2, 15.1, 15.2, 16.1 > Flashcards

13.2, 15.1, 15.2, 16.1 Flashcards

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1
Q

evaporation

A

vaporization that occurs at the surface of a liquid that is not boiling

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2
Q

boiling

A

vaporization throughout the liquid when vapor pressure is equal to the outside pressure

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3
Q

boiling point

A

the temperature at which the vapor pressure of a liquid is just equal to the external pressure on the liquid

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4
Q

normal boiling point

A

the boiling point of a liquid at a pressure of 101.3 kPa or 1atm

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5
Q

solvation

A

a process that occurs when an ionic solute dissolves

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6
Q

what happens when things dissolve in a solution

A

solvent molecules surround the positive and negative ions

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7
Q

vapor pressure

A

a measure of the force exerted by a gas above a liquid in a sealed container
a dynamic equilibrium exists between the vapor and the liquid

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8
Q

surface tension

A

an inward force that tends to minimize the surface area of a liquid
it causes the surface to behave as if it were a thin skin

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9
Q

solution

A

a homogeneous mixture, consists of solutes dissolved in a solvent

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10
Q

solvent

A

the dissolving medium in a solution

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11
Q

solute

A

dissolved particles in a solution

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12
Q

soluble

A

tendency to dissolve in a specific amount of solvent at a specified temperature and presssure

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13
Q

insoluble

A

tendency not to dissolve

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14
Q

diple

A

a molecule that has two poles, or regions, with opposite charges

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15
Q

miscible

A

describes liquids that dissolve in one another in all proportions

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16
Q

immiscible

A

describes liquids that are insoluble in one another

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17
Q

example of immiscible

A

oil and water

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18
Q

saturated

A

maximum amount of solution

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19
Q

unsaturated

A

less than maximum amount of solution

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20
Q

supersaturated

A

more solute than it can hold at a given temperature

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21
Q

two biggest differences between a liquid and a gas

A

the particles are farther apart in a liquid

intermolecular forces important in a liquid, negligible in a gas

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22
Q

what happens to a liquid as it evaporates

A

average kinetic energy goes up, intermolecular forces are broken from the surface and some particles turn into a gas

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23
Q

what happens to the temperature of a liquid as it evaporates

A

it goes down

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24
Q

what affects the rate of evaporation? How and why?

A

heating speeds it up because the kinetic energy of the particles increases

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25
Q

in a closed container, what is going on between the liquid and the vapor?

A

vapor pressure increases until it reaches dynamic equilibrium
rate of evaporation = rate of condensation
the liquid partices at the surface vaporize and produce increased vapor pressure, so then they later condense and return to liquid state

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26
Q

how does an increase in the temperature of a contained liquid affect the kinetic energy? Vapor pressure?

A

it increases them both

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27
Q

can a boiling liquid ever be increased above the boiling point by adding more energy

A

no

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28
Q

how can water be made to boil above the normal boiling point

A

higher external pressure

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29
Q

what are the six phase changes and what phases do they convert between

A 
sublimation - solid to gas
deposition - gas to solid
evaporation - liquid to gas
condensation - gas to liquid
freezing - liquid to solid
melting - solid to liquid
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30
Q

what are the conditions of a polar bond

A

two different atoms

asymmetrical

31
Q

what are the conditions for a non-polar molecule

A

2 same atoms

symmetry

32
Q

how many bonding pairs of electrons are there in water

A

2

33
Q

how many non-bonding pairs are there

A

2

34
Q

what is the shape of water

A

bent

35
Q

what is electronegativity

A

the ability of an atom to attract electrons when the atom is in a compound

36
Q

which part of the periodic table are elements with the greatest electronegativities found?

A

top right

37
Q

which elements do not have electronegativity values and why

A

noble gases
full
don’t bond

38
Q

which element in water has the highest electronegativity

A

oxygen

39
Q

which element in water has the lowest electronegativity

A

hydrogen

40
Q

Which element in water pulls the electrons closer to it

A

oxygen

41
Q

what is the charge on oxygen in water

A

slightly negative

42
Q

what is the charge of hydrogen in water

A

slightly positive

43
Q

Is water a polar molecule

A

yes

44
Q

what is hydrogen bonding

A

positive attracts to negative of another

attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom

45
Q

what are two consequences of hydrogen bonding in water

A

high surface tension

low vapor pressure

46
Q

what does a surfactant do

A

interferes with hydrogen bonding and reduces surface tension

47
Q

example of surfactant

A

detergent

48
Q

bonds between water molecules are

A

hydrogen bonds

49
Q

bonds between the H and O within a water molecule are

A

polar covalent bonds

50
Q

Why does water have such a high boiling point compared to other compounds

A

hydrogen bonding causes high surface tension, particles can’t break up as easily

51
Q

why does it take so much energy to melt ice

A

hydrogen bonding

52
Q

how can the boiling point be adjusted or changed

A

increased pressure will increase boiling point

increased altitude will lower boiling point

53
Q

why is ice less dense than water

A

hydrogen bonds hold water in open framework

54
Q

what is a homogeneous solution

A

solution that is uniform in composition

55
Q

can the solute be filtered out from the solvent in a homogeneous solution

A

no

56
Q

what types of substances can be dissolved in each other

A

like
polar in polar
nonpolar in nonpolar

57
Q

what solutes form an electrolyte when dissolved in water

A

ionic compounds

58
Q

under what other conditions do ionic compounds conduct electricity

A

when they are molten and soluble

59
Q

what solutes are most likely to dissolve in water

A

ionic and polar

60
Q

what solutes form non-electrolytes when dissolved in water

A

molecular compounds

61
Q

what type of solution can conduct electricity

A

electrolytes

62
Q

what types of elements for electrolytes

A

ionic

63
Q

are all molecular compounds non-electrolytes

A

no

64
Q

what molecular compounds are electrolytes

A

acids

NH3

65
Q

What is the difference between weak and strong electrolytes

A

strong electrolyte - strong electric current, dissociate into ions completely
weak electrolyte - weak electric current, few ions dissociate

66
Q

vaporization

A

the conversion of a liquid to a gas or vapor

67
Q

Why might an ionic compound not dissolve in water

A

not soluble - attractions are stronger

68
Q

how could you tell whether a compound would dissolve in water or not

A

solubility table

69
Q

what affects the rate of dissolving

A

stirring
temperature
surface area

70
Q

what is the expression for solubility

A

the number of grams of solute per 100g of solvent at a certain temperature

71
Q

what affects the solubility of a solute and how?

A

temperature, pressure, nature of solvent (polar, nonpolar)

temp goes up, solubility goes up

72
Q

what affects the solubility of a gas

A

temperature and pressure

73
Q

how could you tell whether a solution was supersaturated

A

drop solute in and if it crystallizes is supersaturated

Chemistry (12 decks)

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