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Honors Chemistry > Semester 2 Final Review Part 2 > Flashcards

Semester 2 Final Review Part 2 Flashcards

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1
Q

What is cohesion?

A

Attraction of liquid particles for each other

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2
Q

What is adhesion?

A

Attraction of liquid particles to particles of solid surfaces

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3
Q

Below the surface of a liquid, the particles are pulled?

A

Equally in all directions by cohesive forces

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4
Q

Surface particles are pulled only sideways and downwards because?

A

So they have a net downward force

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5
Q

Does it take energy to oppose net force and increase surface area?

A

Yes

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6
Q

What is surface tension?

A

The tendency of liquids to decrease surface area to the smallest size possible

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7
Q

A solid to a gas is called?

A

Sublimation

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8
Q

A gas to a solid is called?

A

Deposition

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9
Q

Does temperature change when a substance changes state?

A

No

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10
Q

It takes energy to overcome what?

A

The forces holding particles together

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11
Q

What is a good measure of the strength of the forces that hold particles together?

A

Boiling point and melting point

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12
Q

Do ionic substances have much higher forces of attraction than covalent substances?

A

Yes

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13
Q

Why do ionic substances have higher forces of attraction?

A

They are closer together

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14
Q

Compounds with smaller ions or bigger ions have the highest melting points?

A

Smaller ions because there are smaller distances between them

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15
Q

What are intermolecular forces?

A

Forces of attraction between molecules of covalent compounds

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16
Q

Are intermolecular forces weaker than the forces between atoms in the molecule?

A

Yes

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17
Q

What is a dipole?

A

One end of the molecule has a partial positive charge while the other has a partial negative charge

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18
Q

How will molecules orientate themselves in dipoles?

A

So that the opposite charges attract principle operates effectively

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19
Q

Is it true that very polar molecules have high dipole-dipole forces?

A

Yes

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20
Q

The more polar the molecules are,

A

The higher the boiling point of the substance

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21
Q

What is a special case of dipole-dipole interactions?

A

Hydrogen bonding

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22
Q

What is hydrogen bonding?

A

A hydrogen atom is bonded to a highly electronegative atom of one molecule which is attracted to two unshared electrons of another molecule

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23
Q

Is it true that compounds with hydrogen bonding have higher boiling points than comparable compounds?

A

Yes

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24
Q

When can a strong hydrogen bond form?

A

When a hydrogen atom is covalently bonded to very electronegative atoms in the upper-right part of the periodic table

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25
Q

How does a london dispersion force work?

A

When the electrons move toward one side of an atom or molecule, that side momentarily is negative and the other is positive

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26
Q

What is a london dispersion force?

A

The dipole-dipole force resulting from the uneven distribution of electrons and the creation of temporary dipoles

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27
Q

Nonpolar molecules can only experience what type of intermolecular force?

A

LDF

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28
Q

Polar covalent molecules experience both?

A

Dipole-dipole and LDF

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29
Q

Dipole-dipole force are generally stronger than?

A

LDF

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30
Q

Larger compounds (molar mass) have stronger?

A

LDF because its proportional to number os electrons present and molar mass

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31
Q

What is the enthalpy of fusion? ΔHfus

A

The energy added during melting or removed during freezing

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32
Q

What is the enthalpy of vaporization? ΔHvap

A

The energy added during vaporization or removed during condensation

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33
Q

Which one is greater: energy of vaporization or energy of fusion

A

Energy of vap. because more energy is needed to go from liquid to gas because particles are farther apart

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34
Q

Is this true? Molar enthalpy increases as a substance’s temperature increases. Molar enthalpy is highest at the boiling point.

A

Yes

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35
Q

What equation can be used to find the molar enthalpy of vaporization and fusion?

A

q=nΔHvap

q=nΔHfus

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36
Q

As a solid melts, the entropy of its particles ____

A

Increases

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37
Q

An increase of entropy due to a solid melting is?

A

entropy of fusion (ΔSfus)

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38
Q

As a liquid vaporizes, the entropy of the particles _______.

A

increases

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39
Q

An increase of entropy due to a liquid vaporizing is?

A

entropy of vaporization (ΔSvap)

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40
Q

A substances entropy of vaporization is much ____ than its entropy of fusion

A

Larger

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41
Q

Are intermolecular forces significant in the gaseous state?

A

No

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42
Q

What is the formula for Tmp?

A

ΔHfus/ΔSfus

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43
Q

What is the formula for Tbp?

A

ΔHvap/ΔSvap

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44
Q

What is a phase?

A

A region that has the same composition and properties throughout

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45
Q

What is dynamic equilibrium?

A

Particles are constantly moving between two or more phases yet there is no net change in the amount of substance in either phase

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46
Q

When does dynamic equilibrium exist?

A

When no heat is added or removed

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47
Q

What is a phase diagram?

A

A graph that shows the relationship between the physical state of a substance and the temperature and pressure of the substance

48
Q

What are the 3 lines in a phase diagram?

A

Liquid-gas equilibrium, liquid-solid equilibrium, and solid-gas equilibrium

49
Q

What is the triple point?

A

Where the temperature and pressure at which the three states of a substance coexist at equilibrium

50
Q

What is the supercritical fluid?

A

The substance above the critical point

51
Q

What is the critical point?

A

At a temperature and pressure where the liquid and vapor pressure phases are identical

52
Q

What is a solution?

A

Homogeneous mixture, particles are molecule-sized so that the mixture is uniform

53
Q

What is suspension?

A

Heterogeneous mixture that has been well-mixed, but particles will settle out over time

54
Q

What is solvent?

A

The main ingredient in a solution, water is the most common solvent

55
Q

What is the solute?

A

The substance that is dissolved in the solvent

56
Q

What are colloids?

A

Stable heterogeneous mixtures, particles repel each other because they have an electric charge, particles will not collect into larger particles

57
Q

Mixtures can be separated using what?

A

Physical properties

58
Q

What are the methods of separation?

A

Filtering, centrifuge, decant, evaporate, distillation, chromatography

59
Q

What is chromatography?

A

Separates compounds of mixture based on how quickly molecules dissolved in a mobile phase solvent move along a solid phase

60
Q

What is distillation?

A

Separates boiling points of compounds based on their boiling points

61
Q

What is a distillate?

A

Materials with lower vapor pressures evaporate first and are removed from the solution

62
Q

What is parts per million (ppm)?

A

The amount of solute in the solution used to express the amount of an impurity in another substance

63
Q

How is ppm calculated?

A

g of solute/g of solvent x 1000000

64
Q

What is concentration?

A

Ratio of solute to solvent in a solution

65
Q

What is molarity?

A

Mol solute/L solution

66
Q

What is molality?

A

Mol solute/kg solution

67
Q

What is the formula for a dilution?

A

M1V1 = M2V2

68
Q

What does gas solubility depend on?

A

Temperature and pressure

69
Q

What is Henry’s Law?

A

The solubility of a gas increase as the partial pressure of the gas on the surface of the liquid increases

70
Q

The higher the pressure, the

A

More gas dissolves

71
Q

The lower the pressure, the

A

Less gas dissolves

72
Q

As temperature increases, the solubility of a gas

A

Decreases

73
Q

Why are gases less soluble in high temperatures?

A

The increased motion allows gas molecules to escape from the solution

74
Q

If you open warm pop what happens?

A

Gas bubbles will escape

75
Q

What is solubility?

A

The maximum amount of solute that can dissolve in a solvent at a given temperature

76
Q

What formula is used for solubility?

A

grams solute/100 g solvent

77
Q

What does saturated mean?

A

Holds enough/as much solute as it can

78
Q

Solubilities of solids _____ as temperature increases

A

Increase

79
Q

What is important to remember with solubility?

A

Like dissolves like

80
Q

What is an emulsion?

A

Made of colloid-sized droplets suspended in liquid in which they would ordinarily be insoluble unless stabilized

81
Q

What is an electrolyte?

A

A substance that dissolves in a liquid solvent and provides ions that conduct electricity

82
Q

What do strong electrolytes do?

A

Completely dissociate into ions and conduct electricity well (ionic compounds)

83
Q

What do weak electrolytes do?

A

Provide few ions in a solutions, conduct electricity weakly

84
Q

What is a nonelectrolyte?

A

A liquid or solid substance that does not allow the flow of an electric current (covalent compounds)

85
Q

What do colligative properties depend on?

A

The number of particles of solute in a solution

86
Q

What formula is used for freezing point depression?

A

Δtf = Kfm

87
Q

What formula is used for boiling point depression?

A

Δtb = Kbm

88
Q

What is a completion reaction?

A

All of the reactant reacts to form product

89
Q

What is a reverse reaction?

A

The products can reform reactants

90
Q

What is chemical equilibrium?

A

The forward and reverse reactions reach a state of balance in which the concentrations of the reactants and products remain the same even though individual atoms may be changing

91
Q

What is the rate?

A

Speed at which a process occurs

92
Q

What is a complex ion?

A

Any metal atom or ion that is bonded to more than 1 atom or molecule

93
Q

What is a ligand?

A

Molecules or anions that readily bond to metal ions

94
Q

What are complex ions formed from?

A

Transition metals

95
Q

What is the solubility product of the salt in water?

A

Maximum concentration of salt in an aqueous solution

96
Q

When do reversible reactions reach equilibrium?

A

When the concentration of the reactants and the products is constant

97
Q

If Keq >1

A

Products are favored at equilibrium

98
Q

If Keq <1

A

Reactants are favored at equilibrium

99
Q

Keq=1

A

Equilibrium

100
Q

What is stress?

A

Something that causes a change in a system at equilibrium

101
Q

What are the 3 kinds of stress?

A

Change in concentration, temperature, and pressure

102
Q

What happens when stress is applied?

A

Eq is disrupted and rates are no longer equal

103
Q

What is Le Chatelier’s Principle?

A

System adjusts to reduce change

104
Q

How does equilibrium shift right?

A

Add a reactant, remove a product

105
Q

How does equilibrium shift left?

A

Remove a reactant, add a product

106
Q

Exothermic reactions usually lead to a shift in favor of

A

Reactants

107
Q

Endothermic reactants usually lead to a shift in favor of

A

Products

108
Q

Changes in pressure can affect ____ at equilibrium

A

Gases

109
Q

A pressure increase favors

A

The reaction that produces fewer gas molecules

110
Q

Acids have a ____ taste?

A

Sour

111
Q

Acids are usually?

A

Liquids or gases

112
Q

Bases taste?

A

Bitter

113
Q

Bases are what?

A

Good cleaning agent, slippery, usually solids

114
Q

What are the seven common strong acids?

A

HCl, HBr, HI, nitric acid, sulfuric acid, HClO4, and HIO4

115
Q

What are the seven common weak acids?

A

Acetic acid, HCN, HF, HNO3, nitrous acid, sulfurous acid, HOCl, H3PO4

116
Q

What are strong bases?

A

NaOH, KOH, Ca(OH)2, Ba(OH)2, Na3PO4

117
Q

What are weak bases?

A

NH3, Na2CO3, K2CO3, C6H5NH2, (CH3)3N

Honors Chemistry (13 decks)

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