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Flashcardlet > Phy Sci chapter eight > Flashcards

Phy Sci chapter eight Flashcards

0
Q

What determined whether a mixture is a suspension or a colloid

A

The size of the particles

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1
Q

An oatmeal raisin cookie is an example of a what

A

Heterogenous mixture

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2
Q

Chlorine, which is used in swimming pools to kill bacteria, is a what

A

Solute

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3
Q 
Which of the following is a solution 
A. Air 
B. Wood
C. Snow 
D. Orange juice
A

Air

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4
Q

Pennies minted after 1984 contain 97.5% zinc and 2.5% copper
These coins are examples of what

A

Alloys

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5
Q

Two liquids that form a heterogenous mixture are said to be

A

Immiscible

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6
Q

What is a method for separating a solution of miscible liquids

A

Distilling

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7
Q 
Which of the following is an example of a homogenous mixture 
A. Fog 
B. Gasoline 
C. Paint 
D. Grapefruit juice
A

Gasoline

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8
Q

Particles in a what can be separated by filtration

A

Suspension

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9
Q

The Tyndall effect in observed in

A

Colloids

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10
Q

What is a heterogenous mixture

A

It doesn’t have a fixed composition

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11
Q

What do particles in a suspension do

What size are they

A

Settle out

Large

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12
Q

A mixture in which particles of a material are more or less evenly dispersed throughout a liquid or gas

A

Suspension

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13
Q

What may particles in a suspension do

A

Settle over time

Be filtered out

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14
Q

Liquids that do not mix with each other

A

Immiscible

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15
Q

Process of luring a less dense liquid off a denser liquid

A

Decanting

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16
Q

What is declaring used for

A

To separate two immiscible liquids

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17
Q

What are the size of particles in a colloid

What does this mean

A

Too small

They can’t settle out

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18
Q

A mixture consisting of tiny particles that are intermediate in size between those in solutions and those in suspensions and that are suspended in a liquid, solid, or gas

A

Colloid

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19
Q

What are particles in a colloid large enough for

A

To scatter light that passes through

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20
Q

What does the Tyndall Effect state

A

That particles in a colloid are large enough to scatter light that passes through

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21
Q

What can some immiscible liquids form

A

Colloids

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22
Q

Any mixture of two or more immiscible liquids in which one liquid is dispersed in the other

A

Emulsion

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23
Q

What is a homogenous mixture

A

It looks uniform even when you examine it under a microscope because the individual complements of the mixture are too small to be seen

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24
Q

What is special about the ions in salt water

A

The number of ions is the same everywhere

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25
Q

Are homogenous mixtures solutions

A

Yes

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26
Q

A homogenous throughout which two or more substances are uniformly dispersed

A

Solution

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27
Q

In a solution, the substance that dissolves in the solvent

A

Solute

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28
Q

In a solution, the substance in which the solute dissolves

A

Solvent

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29
Q

What is not a homogenous mixture

A

Milk

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30
Q

What do miscible liquids mix to from

A

Solutions

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31
Q

Liquids that form a single layer when mixed

A

Miscible

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32
Q

A method used to separate miscible liquids that have different boiling points

A

Distillation

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33
Q

What do liquid solutions sometimes contain none of

A

Water

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34
Q

A liquid solution of gasoline, diesel fuel, and kerosene

A

Petroleum

35
Q

Other states of matter can also form what

A

Solutions

36
Q

What is the air a solution of

A

Nitrogen
Oxygen
Argon
Other gases

37
Q

A solution of mercury dissolved in silver

A

Amalgam

38
Q

The substance that there is the most amount of

A

Solvent

39
Q

The substance that there is the least amount of

A

Solute

40
Q

Solids can dissolve in what

A

Other solids

41
Q

A solid or liquid mixture of two or more metals

A

Alloy

42
Q

Why is water called the universal solvent

A

Because many substances can dissolve in water

43
Q

Water can dissolve what

A

Ionic compounds

44
Q

What is water

A

A polar compound

45
Q

Describes a molecule in which the positive and negative charges are separated

A

Polar

46
Q

What do water molecules attract

A

Both positive ions and negative ions

47
Q

What do polar water molecules pull apart

A

Ionic crystals

48
Q

The partially negative oxygen atoms of water molecules attract what

A

The positively charged sodium ions

49
Q

What does dissolving depend on

A

The forces between particles

50
Q

What must be forces between the solvent molecules and the particles of the substance be grape after than

A

The force between the particles in the crystal

51
Q

What kind of compound does water dissolve many of

A

Covalent (molecular)

52
Q

Water forms hydrogen bonds with what

A

Molecular compounds such as sugar

53
Q

The intermolecular force occurring when a hydrogen atom that is bonded to a highly electronegative atom of one molecule is attracted to two unshared electrons of another molecule

A

Hydrogen bond

54
Q

What does “like dissolves like” mean

A

A solvent will dissolve substances that have molecular structures that are like the solvent’s structure

55
Q

What will usually not dissolve in water

A

Nonpolar compounds

56
Q

Describes a molecule in which the centers of positive and negative charge are not separated

A

Nonpolar

57
Q

Nonpolar solvents are used to dissolve what

A

Nonpolar materials

58
Q

Why do substances dissolve

A

The energy transferred from the solvent to the solute, as well as the attractive forces between the solvent and solute molecules, causes molecules at the surface of the crystal to dissolve

59
Q

What kind of solutes dissolve faster

A

Solutes with a large surface area

60
Q

What helps the solute dissolve faster

A

Stirring of shaking a solution

61
Q

What particles diffuse throughout the solution faster

A

Dissolved solute particles

62
Q

More what particles can dissolve

A

Solute

63
Q

When do solutes dissolve faster

A

When the solvent is hot

64
Q

What affects the physical properties of a solution

A

Solutes

65
Q

What increases the boiling point of a solution

A

Solutes

66
Q

What lowers the freezing point of a solution

A

Solutes

67
Q

What is solubility

A

The maximum mass of a solute that can dissolve in 100g of a solvent at a certain temperature and standard atmospheric pressure

68
Q

The ability of a substance to dissolve in another at a given temperature and pressure

A

Solubility

69
Q

Different substances have different what

A

Solubilities

70
Q

How much of a substance is in a solution

A

To express how much of a substance can dissolve in a solvent, you need to use the concentration

71
Q

The amount of a particular substance in a given volume of a mixture, solution, or ore

A

Concentration

72
Q

What kind of solution has a large amount of solute

A

Concentrated

73
Q

What kind of solution has only a small amount of solute

A

Dilute

74
Q

What happens when you add more solute to a saturated solution

A

In a saturated solution, the dissolved solute is in equilibrium with undissolved solute
If you add more solute, it just settles to the bottom of the container

75
Q

A solution that cannot dissolve any more solute under the given conditions

A

Saturated solution

76
Q

Unsaturated solutions can become what

A

Saturated

77
Q

A solution that contains less solute than a standard solution does and that is able to dissolve additional solute

A

Unsaturated solution

78
Q

Doing what to a saturated solution can dissolve more solid

A

Heating

79
Q

The solubility of most solutes increases with what

A

Temperature

80
Q

A solution that holds more dissolved solute than is required to reach equilibrium at a given temperature

A

Supersaturated solution

81
Q

How do you make a supersaturated solution

A

You raise the temperature of a solution, dissolve more solute, then let the solution cool again

82
Q

What affects the solubility of gases

A

Temperature and pressure

83
Q

Gaseous solutes are what in warmer water

A

Less soluble

84
Q

Gases are more soluble under what

A

High pressure

85
Q

How do you describe how much of a solute is in a solution

A

One of the most common ways of expressing the concentration of a solution is molarity

86
Q

A concentration unit of a solution expressed in moles of solute dissolved per liter of solution

A

Molarity

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