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Chemistry > Chapter 6- Liquids And Solids > Flashcards

Chapter 6- Liquids And Solids Flashcards

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0
Q

Large enough attractive forces to keep the molecules ___

A

Together

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1
Q

Molecules in the liquid state are ___

A

Close together

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2
Q

Attractive forces not strong enough to ___

A

Restrict movement

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3
Q

Liquids are practically incompressible

A

Compressibility

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4
Q

Measure of a liquid’s resistance to flow

A

Viscosity

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5
Q

Measure of the attractive forces exerted among molecules at the surface of the liquid.

A

Surface tension

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6
Q

Substances that are added to a liquid to decrease surface tension

A

Surfactants

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7
Q

The process of conversion of liquid to gas, at a temperature too low to boil.

A

Evaporation

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8
Q

Conversion of gas to the liquid state (reverse of evaporation)

A

Condensation

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9
Q

The temperature at which the vapor pressure of the liquid becomes equal to the atmospheric pressure.

A

Boiling point

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10
Q

Temperature at which the vapor pressure of the liquid is equal to 1 atm

A

Normal boiling point

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11
Q

Is a special type of dipole-dipole attraction

A

Hydrogen bonding

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12
Q

Is a very strong intermolecular attraction causing higher than expected b.p. and m.p.

A

Hydrogen bonding

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13
Q

What is necessary for Hydrogen Bonding?

A

Molecules have hydrogen directly bonded to O,N, or F.

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14
Q

Particles highly organized in a defined fashion

A

The solid state

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15
Q

Fixed shape and volume

A

The solid state

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16
Q

Incompressible

A

Properties of Solids

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17
Q

m.p. depends on strength of attractive forces between particles

A

Properties of solids

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18
Q

Can be crystalline solid- regular repeating structure

A

Properties of solids

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19
Q

Can be amorphous solid- no organized structure

A

Properties of solids

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20
Q

Process of conversion of molecules in the solid state directly to molecules in the gaseous state.

A

Sublimation of solids

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21
Q

Dry ice is solid carbon dioxide. It will convert directly to a gas at atmospheric pressure.

A

Sublimation of solids

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22
Q

Homogeneous mixture of two or more substances

A

Solution

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23
Q

What is an example of a solution?

A

Salt water

Contact solution

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24
Q

The component of the solution that is present in the lesser quantity than the solvent

A

Solute

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25
Q

The solution component present in the largest quantity

A

Solvent

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26
Q

A solution in which water is the solvent

A

Aqueous solution

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27
Q

Air is a solution composed of oxygen and several trace gases that are dissolved in the gaseous solvent, nitrogen

A

Gaseous solution

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28
Q

Homogeneous mixtures of metals in the solid state (brass, a solution of zinc in copper, gold jewelry)

A

Solid solution

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29
Q

Emphasis on the chapter

A

Liquid solution

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30
Q

Clear and transparent with no visible particles of solute

A

Property of liquid solutions

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31
Q

May be either colored or colorless

A

Property of liquid solutions

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32
Q

May be either a solution of electrolytes or nonelectrolytes

A

Property of a liquid solution

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33
Q

A homogeneous mixture with uniform properties throughout

A

True solution

Property of liquid solution

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34
Q

Volume of solutes and solvents are not___

A

Additive

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35
Q

Formed from solutes that are soluble ionic compounds

A

Electrolytes

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36
Q

Some ions dissociate in solution to produce ions that behave as charge carriers

A

Electrolytes

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37
Q

Good conductors of electricity

A

Electrolyte solutions

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38
Q

Formed from dissociating molecular solutes (covalent bonds)

A

Nonelectrolytes

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39
Q

Solutions are nonconducting

A

Nonelectrolytes

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40
Q

Glucose is a good example

A

Nonelectrolytes

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41
Q

Has only one component (water)

A

Pure substance

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42
Q

Contains more than one substance, with tiny particles (salt water) homogeneously intermingled.

A

True solution

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43
Q

Consists of solute parties dispersed through the dispersing medium. The distribution is not completely homogeneous because of the size of the colloidal particles (milk)

A

Colloidal suspension

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44
Q

Smaller than 1nm

A

Solution particles

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45
Q

1nm - 200nm

A

Colloidal particles

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46
Q

Larger than 200 nm

A

Precipitates

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47
Q

The light scattering ability of colloidal suspensions (headlights hitting the fog)

A

Tyndall effect

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48
Q

Do not scatter light

A

True solutions

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49
Q

Have particles that are large enough to scatter light causing the liquid to appear hazy

A

Colloidal suspensions

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50
Q

Like dissolves like

A

Solubility rule of thumb

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51
Q

Quantity of solute that can dissolve in a given number of solvent

A

Degree of solubility

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52
Q

Polar-

A

Polar solvent

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53
Q

Nonpolar-

A

Nonpolar solvent

54
Q

The magnitude of difference between polarity of solute and solvent- the more different they are, the ___

A

Lower the solubility

55
Q

Increase in temperature usually causes an___

A

Increase in solubility

56
Q

Not much effect on liquids and solids in solution. Solubility of gas is directly proportional to the applied pressure (Henry’s Law)

A

Pressure

57
Q

Contains all of the solute that can be dissolved at a certain temperature

A

Saturated solution

58
Q

If a saturated solution is cooled down, the amount of solute that the solution can hold___

A

Decreases

59
Q

The excess solute comes out of solution as a

A

Precipitate

60
Q

Sometimes, supersaturated solution occurs upon cooling. This is when after cooling, excess solute remains in solution for a time. This is ___ and eventually the excess solute will precipitate out of the solution

A

Unstable

61
Q

When a solute is added to a solvent, it will begin to dissolve and continued to dissolve until a ____ ___ is established between the dissolved and undos solved solute.

A

Dynamic equilibrium

62
Q

When a solution is saturated, the solution is in equilibrium with ___ solute

A

Undissolved

63
Q

States that the number of moles of a gas dissolved in a liquid at a given temperature is proportional to the pressure of that gas in the atmosphere that is in contact with the liquid

A

Henry’s law

64
Q

Gases are most soluble at ___ temperatures

A

Low

65
Q

Is the amount of solute dissolved in a given amount of solution

A

Concentration

66
Q

Concentration has impact on ____ properties - melting and boiling point

A

Physical

67
Q

Concentration has an impact on ___ properties- solution reactivity

A

Chemical

68
Q

Amount of solute=

A

Mass of solute in grams

69
Q

Amount of solution=

A

Volume in milliliters

70
Q

Concentration=

A

Amount of solute/ amount of solution

71
Q

%m/v =

A

Grams of solute/ milliliters of substance
*100%
(Must be in grams and milliliters)

72
Q

Mass/mass percent is most useful for solutions of 2 solids whose masses are easily obtained

A

%m/m= grams solute/ grams solutions

*100%

73
Q

Solute+ solvent=

A

Solution

74
Q

As percentage is the number of parts of solute in ___ parts of solution, ppt and ppm change the calculation only by orders of magnitude

A

100

75
Q

ppt=

A

g solute/ g solution * 10^3 ppt

76
Q

ppm=

A

g solute/ g solution * 10^6 ppm

77
Q

The most common mole based concentration unit.

A

Molarity (M)

78
Q

Defined as the number of moles of solute per liter of solution.

A

M=moles of solute/ liters of solution

Molarity

79
Q

Is required to prepare a less concentrated solution from a more concentrated one.

A

Dilution

80
Q

Dilution is required to prepare a ___ concentrated solution from a ___ concentrated one.

A

Less

More

81
Q

Molarity of solution before dilution

A

M1

82
Q

Molarity of solution after dilution

A

M2

83
Q

Volume of solution before dilution

A

V1

84
Q

Volume of solution after dilution

A

V2

85
Q

Formula for dilution

A

M1V1 = M2V2

86
Q

Solution properties that depend on the concentration of the solute particles, rather than the identity of the solute

A

Colligative properties

87
Q

Vapor pressure ___

A

Lowering

88
Q

___ point depression

A

Freezing

89
Q

Boiling point ___

A

Elevation

90
Q

Osmotic ___

A

Pressure

91
Q

Colligative properties-

A

Vapor pressure lowering
Freezing point depression
Boiling point elevation
Osmotic pressure

92
Q

States that when a nonvolatile solute is added to a solvent, the vapor pressure of the solvent decreases on proportion to the concentration of the solute

A

Raoult’s law

Vapor pressure lowering

93
Q

Solute molecules serve as a ___ to the escape of solvent molecules resulting in a decrease in the vapor pressure

A

Barrier

Vapor pressure lowering

94
Q

One consequence of this law is the effect of the solute on the ___ and ___ points of a solution

A

Freezing
Boiling

Vapor pressure lowering

95
Q

Freezing point depression may be explained considering the ___ between solid and liquid states

A

Equilibrium

Freezing point depression

96
Q

Solute molecules interfere with the rate at which liquid water molecules associate to form the ___

A

Solid state

Freezing point depression

97
Q

Proportional to the number of solute particles

A

Freezing point depression

98
Q

Boiling point elevation can be explained considering the definition as the temperature at which ___ ___ of the liquid equals the __ ___

A

Vapor pressure
Atmospheric pressure

Boiling point elevation

99
Q

If a ___ is present then the increase in boiling temperature is necessary to raise the vapor pressure to atmospheric temperature

A

Solute

Boiling point elevation

100
Q

Is proportional to the number of solute particles

A

Boiling point elevation

101
Q

An ___ will affect boiling point to a greater degree than a ___ of the same concentration

A

Electrolyte
Nonelectrolyte

Boiling point elevation

102
Q

Solute concentration is expressed in mole based units

A

Molality (m)

103
Q

Number of ___ is critical, not the mass of solute in molality

A

Particles

104
Q

Moles of solute per kg of solvent

A

Molality (m)

105
Q

Equation for molality (m)

A

Moles solute/ kg solvent

106
Q

The movement of solvent from a dilute solution to a more concentrated solution through a semipermeable membrane

A

Osmosis

Osmotic pressure

107
Q

Osmosis is the movement of solvent from a ___ solution to a __ ___ solution through a semipermeable membrane

A

Dilute
More concentrated

Osmotic pressure

108
Q

Osmosis requires __ to stop this flow

A

Pressure

109
Q

The amount of pressure requires to stop the flow across a semipermeable membrane

A

Osmotic pressure

110
Q

Living cells contain aqueous solution and these cells are also surrounded by ___ ___

A

Aqueous solution

Tonicity and the cell

111
Q

Cell function requires maintenance of the same ___ __ inside and outside the cell

A

Osmotic pressure

Tonicity and the cell

112
Q

Solute concentration of fluid surrounding cells higher than inside results in a ___ solution causing water to flow into the surroundings causing collapse =__

A

Hypertonic

Crenation

113
Q

Solute concentration of fluid surrounding cells too low results in a __ solution causing water to flow into the cell, causing rupture=___

A

Hypotonic

Hemolysis

114
Q

___ solutions have identical osmotic pressure and no osmotic pressure difference cross the cell membrane

A

Isotonic

115
Q

Water is often referred to as the

A

Universal solvent

116
Q

excellent solvent for polar molecules

A

Water

117
Q

Most abundant liquid on earth

A

Water

118
Q

60% of the human body is

A

Water

119
Q

Transports ions, nutrients, and waste into and out of cells

A

Water

120
Q

Solvent for biochemical reactions in cells and digestive tract

A

Water

121
Q

Reactant or product in some biochemical processes

A

Water

122
Q

Two common ways of ions in solution

A

Moles per liter (molarity)

Equivalents per liter (eq/L)

123
Q

Emphasis on the number of individual ions

A

Moles per liter (molarity)

124
Q

Emphasis on charge

A

Equivalents per liter (eq/L)

125
Q

An ___ will lower freezing point or raise boiling point more than a __

A

Electrolyte

Nonelectrolyte

126
Q

An ___ will break apart into ions (dissociate) when it is dissolved in water and a ___ does not

A

Electrolyte

Nonelectrolyte

127
Q

NaCl - _ moles of particles for every 1 mol of NaCl

A

2

128
Q

CaCl2- _ moles of particles for every 1 mole of CaCl2.

A

3

129
Q

C6H12O6 (glucose)- _ mole of particle for every one mole of glucose

A

1

130
Q

Moles of solvent is not temperature __

A

Dependent

131
Q

The eq/mol value of the ion is simply the number of ___ on the __, regardless of whether that charge is positive or negative

A

Charges

Ion

132
Q

When describing ions in blood, urine, or blood plasm, often use

A

Milliequivents/L (meq/L)

133
Q

1 eq=

A

10^3 meq

Chemistry (3 decks)

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