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Chemistry > Unit 9 > Flashcards

Unit 9 Flashcards

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0
Q

How are particles of solids packed together?**

A

More closely than those of liquids & gases

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1
Q

What is a solid?**

A

Has definite shape & definite volume

Has enough kinetic energy to vibrate, but not move out of position

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2
Q

What are the intermolecular forces in solids?

A

Much more effective in solids than in liquids and gases

Solids are very ordered

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3
Q

What are the properties of solids?**

A

1) definite shape & definite volume
2) definite melting point
3) high density & Incompressibility
4) low rate of diffusion

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4
Q

What are the types of solids?**

A

Crystalline solids

Amorphous solids

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5
Q

What are most solids?**

A

Crystalline solids, meaning they contain crystals (either single crystals or groups of crystals fused together)

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6
Q

What is a crystal?

A

A substance in which the particles are arranges in an orderly, geometric, repeating pattern

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7
Q

What is crystal structure?

A

The total 3D arrangement of particles in a crystal

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8
Q

Coordinate system**

A

Lattice

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9
Q

What is unit cell?

A

The smallest portion of a crystal lattice that shows the 3D pattern of the entire lattice

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10
Q

What are the type of symmetry classified by?**

A

By scientists according to the shape of the crystals

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11
Q

What does amorphous come from?**

A

Greek “without shape”

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12
Q

What is freezing? Energy? Particles?**

A

Liquid to solid
Loss of heat energy
Increase in order of the particles

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13
Q

What is melting? Energy? Particles?**

A

Solid to liquid
Absorption of heat energy
Decrease in order of particles

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14
Q

What is evaporation? At what temperature? Example**

A

Liquid to gas
At temperatures below the boiling point
Ex. Water in puddles

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15
Q

What is vaporization? At what temperature? Example**

A

Liquid to gaseous state
At the boiling point
Ex. Boiling water on a stove

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16
Q

What is condensation? Example**

A

Gas to liquid

Ex. Water vapor condensing on cold glass

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17
Q

What is sublimation? Example**

A

Solid directly to a gas without going through the liquid state
Ex. Ice cubes in freezer shrinking

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18
Q

What is deposition? Example**

A

Gas directly to a solid without going through the liquid state
Ex. Water vapor to ice

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19
Q

What is molar heat of fusion?

A

The amount of heat energy required to melt one mole of solid at its melting point

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20
Q

What is magnitude for molar heat of fusion?

A

A measure of the attraction between the particles of a solid

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21
Q

What is molar heat of vaporization?

A

The amount of heat energy needed to vaporize one mole of liquid at its boiling point

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22
Q

What is magnitude for molar heat of vaporization?

A

A measure of the attraction between the particles of the liquid

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23
Q

What type of bond is water? What type of structure does it have? What are the bond angles?**

A

Polar covalent bond
Bent structure
Bond angles are 105 degrees

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24
Q

What is a physical property of water?**

A

Unusual: expanding in volume as it freezes

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25
Q

What is a mixture?**

A

A combination of more than one pure substances

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26
Q

What is a homogenous mixture?**

A

The mixing is the same throughout

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27
Q

What are solutions? Example?

A

2 or more substances uniformly spread thought a single phase; mixture of substances that has the same composition & properties throughout
Ex. Sugar & water

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28
Q

What is solute?**

A

That which dissolves

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29
Q

What is solvent?**

A

That which does the dissolving

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30
Q

What is a heterogeneous mixture?**

A

The mixing is not the same throughout

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31
Q

What are colloids? Examples**

A

A mixture of very tiny particles of pure substances that are dispersed in another substance but do not settle out
Ex. Blood, fog, gelatin, whipped cream, paint

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32
Q

What are emulsions?

A

A mixture of Immiscible liquids in which the liquids are spread throughout one another; a specific type of colloid
Ex. Mayo, cream, butter & lotion

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33
Q

What is a suspension? Examples**

A

A mixture that looks uniform when stirred or shaken, but separates into different layers when it is no longer agitated
Ex. Muddy water, Italian dressing, oil & water

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34
Q

What is the Tyndall effect? Example

A

The scattering of light by colloidal particles dispersed In a transparent medium
Ex. Headlight beams are visible on a foggy night

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35
Q

What can the Tyndall effect be used to do?

A

Distinguish between a solution & a colloid

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36
Q

What is an electrolyte?

A

A substance that dissolves in water to give a solution that conducts electric current

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37
Q

What is a nonelectrolyte?

A

A substance that dissolves in water to give a solution that does not conduct an electric current

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38
Q

What are the factors affecting the rate of dissolution?

A
  1. Increasing the surface area Of the solute
  2. Agitating a solution
  3. Heating a solution
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39
Q

Where does dissolution occur?

A

At the surface of the solute

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40
Q

What does it mean to be soluble?

A

Able to dissolve

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41
Q

What is there for every solute & solvent combination?

A

A limit as to the amount of solute that can be dissolved

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42
Q

What is solution equilibrium?

A

The physical state in which the opposing processes of dissolution & crystallization of a solute occur at equal rates

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43
Q

What is a saturated solution?

A

A solution that contains the maximum amount of dissolved solute

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44
Q

What is an unsaturated solution?

A

A solution that contains less solute than a saturated solution under the existing conditions

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45
Q

What is a super saturated solution?

A

A solution that contains mor dissolved solute than a saturated solution contains under the same conditions

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46
Q

What is the solubility of a substance?

A

The amount of that substance required to form a saturate solution with a specific amount of solvent at a specified temperature

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47
Q

What is the attraction between water molecules and the ions strong enough to do? What is this process called? What are the ions said to be?

A

Draw the ions away from the crystal surface(solute) & into solution
Hydration
Hydrated

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48
Q

some ionic substances form crystals that incorporate water molecules known as

A

Hydrates

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49
Q

What are ionic compounds In no polar solvents?

A

They are not generally soluble

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50
Q

What are liquids classified by?

A

How they mix

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51
Q

What is miscible?

A

Two or more liquids that are able to dissolve freely into one another
They are soluble in each other

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52
Q

When do changes in state occur?

A

When the particles of the substance absorb/release a certain amount of energy

53
Q

What does adding heat energy do to the kinetic energy & order of particles?

A

Increases the kinetic energy of the substance & decreases the order of particles

54
Q

For molar heat of vaporization, what does stronger attraction mean?

A

More energy will be required to overcome it so the molar heat of vaporization will be larger

55
Q

What are the molecules in solid or liquid water linked by?**

A

Hydrogen bonding

56
Q

What does ice consist of?**

A

Water molecules in the hexagonal arrangement

57
Q

What accounts for the relatively low density of ice?**

A

Empty spaces

58
Q

What happens as the ice is heated?

A

The increased energy of the molecules causes them to move & vibrate more vigorously

59
Q

What happens when the melting point of ice is reached?

A

The energy of the molecules is so great that the rigid open structure of the ice crystals breaks down & ice turns into liquid water

60
Q

What is any observable odor or taste causes by in pure liquid water?

A

Impurities such as dissolved minerals, liquids or gases

61
Q

Why do colloids appear homogeneous?**

A

Because individual particles cannot be seen, but they are large enough to scatter light

62
Q

What do ionic compounds yield? Examples

A

Cations & anions that are free to move making an electric current possible
Ex. NaCl & any ionic compound
Ex. Certain highly polar compounds

63
Q

Do neutral molecules in a solution conduct an electric current?

A

No because it does not contain mobile charges particles

64
Q

What does solubility vary with?

A

Temperature

65
Q

For gases, what also must be specified?

A

Pressure

66
Q

What do similarities of substances depend on?

A
  1. Types of bonding
  2. Polarity
  3. Intermolecular forces between molecules of solute & solvent
67
Q

What are the 6 basic crystal structures?**

A
  1. Isometric
  2. Tetragonal
  3. Orthorhombic
  4. Monoclinic
  5. Triclinic
  6. Hexagonal
68
Q

How are particles arranged in amorphous solids? Shape? How long do they hold their shape for? How do they flow? Examples?**

A 
Randomly
They do not have a natural regular shape 
Hold their shape for a long time 
Flow very slowly
Ex. Glass & plastic
69
Q

What is the heat of fusion for water?**

A

334 kJ/kg

70
Q

What is the heat of vaporization for water?**

A

2260 kJ/kg

71
Q

What does stirring or shaking help to do?

A

Disperse the solute particles & bring fresh solvent into contact with the solute surface. Similar to crushing

72
Q

How is hydronium ion formed?

A

A proton is transferred directly from HCl to a water molecule, where it becomes covalently bonded to oxygem

73
Q

What is osmotic pressure dependent on?

A

The concentration of solute particles, not on the type of solute particles

74
Q

What does increasing the concentration of the solution do to the osmotic pressure?

A

It increases as well

75
Q

What are cell membranes?

A

Semipermeable so regulation of osmosis is vital to cell life

76
Q

What do cells do when placed in a solution of higher concentration?

A

Lose water & shrink

77
Q

What do cells do when placed in a solution of lower concentration?

A

Gain water & swell

78
Q

In vertebrates, what are cells protected from?

A

From swelling & shrinking by blood & lymph that surround the cells

79
Q

What are blood & lymph in concentration to the concentration inside the cell?

A

Equal

80
Q

What does hydrogen bonding between molecules require?

A

A high KE & therefore water has a relatively high boiling point compared to other liquids

81
Q

As temperature is increased, water molecules

A

Move farther apart

82
Q

Groups of water molecule absorb energy to

A

Break into separate molecules

83
Q

Hydrogen bonds between molecules of liquid water at 0 degrees celsius are

A

Fewer & more disordered than those between molecules of ice at the same temperature

84
Q

Liquid water is ___ than ice

A

Denser

85
Q

Water molecules are able to

A

Crowd closer together

86
Q

Rigid structure of water has

A

Broken down

87
Q

Increasing KE allows water molecules

A

To overcome molecular attractions

88
Q

What is Immiscible?

A

Describes 2 or more liquids that do not mix into each other

They are not soluble in each other

89
Q

What do increases in pressure do to gas solubilities in liquids?

A

Increase them

90
Q

What does pressure do to solubility?

A

Has very little effect on the solubilities of liquids or solids in liquid solvents

91
Q

What does Increasing temperature do to the solubility of solids?

A

Increases them

92
Q

What does increasing the temperature usually do to gas solubility?

A

Decreases it

93
Q

What is the concentration of a solution?

A

A measure of the amount of the solute in a given amount of solvent or solution

94
Q

What is molarity? What must you know?

A

The number of moles of solute in one liter of solution

Must know the molar mass of the solute

95
Q

Molarity= ?

A

M= amount of solute (mol)
————————–
Volume of solution (L)

96
Q

What is molality?

A

The concentration of a solution expressed in moles of solute per kilogram of solvent

97
Q

Molality= ?

A

m= amount of solute (mol)
————————-
Mass of solvent (kg)

98
Q

What is dissociation?

A

The separation of ions that occurs when an ionic compound dissolves

99
Q

What can some molecular compounds also form in solution?

A

Ions

Usually polar compounds

100
Q

What are ions formed from?

A

Solute molecules by the action of the solvent In a process called ionization

101
Q

What is ionization?

A

Creation of ions where there were none

Different then dissociation

102
Q

What does the extent to which a solute ionizes in solution depend on?

A

The strength of the bonds within the molecules(intramolecular forces) & between th esolute & solvent (intermolecular forces)

103
Q

What is the hydronium ion?

A

H3O

H doesn’t exist alone

104
Q

What are strong electrolytes?

A

Any compound of which all or almost all of the dissolved compound exists as ions in aqueous solution

105
Q

What are weak electrolytes?

A

A compound of which a relatively small amount of the dissolved compound exists as ions in aqueous solution

106
Q

What do semipermeable membranes do?

A

Allow the movement of some particles while blocking the movement of other particles

107
Q

What is osmosis?

A

The movement of solvent through a semipermeable membrane from the side of lower solute concentration to the side of high solute concentration

108
Q

When does osmosis occur?

A

Whenever 2 solutions of different concentrations are separated by a semipermeable membrane

109
Q

What is osmotic pressure?

A

The external pressure that must be applied to stop osmosis

110
Q

Are the melting point & freezing point the same or a different temperature? **

A

They’re the same

111
Q

Are the boiling point & condensation point the same temperature or different?**

A

They’re the same

112
Q

What does which way the substance goes depend on?

A

Whether energy is being added or removed

113
Q

What can water exist in?**

A

All 3 physical states: solid, liquid & gas

114
Q

What is water on earth?**

A

The most abundant liquid

115
Q

How much of earths surface does water make up? Where is a significant amount of this water?**

A

About 75%

A significant amount of this water is frozen in glaciers

116
Q

What is water to all organisms?**

A

An essential component

117
Q

What % of the mass of livings things is water?**

A

70-90%

118
Q

How many molecules per group in liquid water?**

A

Usually from 4-8

119
Q

At room temperature pure liquid water is:

A
  1. Transparent
  2. Odorless
  3. Tasteless
  4. Almost colorless
120
Q

What are substances that dissolve in water classified according to?

A

Whether they yield molecules or ions in solutions

121
Q

Why does any solid solute In a liquid solvent dissolve?

A

Because molecules or ions of the solute are attracted by the solvent

122
Q

In general, the more finely divided a substance is…

A

The greater the surface area & the more quick it dissolves

123
Q

What does increasing the temperature of the solvent result in?

A

The faster motion of the solvent molecules and the kinetic energy increases

124
Q

At higher temperature, the collisions between solvent molecules & the solute are

A

More frequent

125
Q

What is the rate at which a solid dissolves?

A

Unrelated to solubility

126
Q

The attraction between the ionic solutes & no polar solvent is

A

Not strong enough to overcome the intramolecular forces holding the solute together

127
Q

What are the ways to express the concentrations of solutions?

A

Molarity

Molality

128
Q

What is The strength with which substances conduct an electric current related to?

A

Their ability to form ions in solutions

129
Q

What do strong electrolytes yield when they dissolve in water?

A

Only ions

130
Q

How is the strength of electrolytes related to the concentration of a solution?

A

They’re unrelated

131
Q

What are weak electrolytes not the same as?

A

Nonelectrolytes where none of the dissolved compound exists as ions

Chemistry (4 decks)

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