Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Honors Chemistry > Semester 2 Final Review Part 1 > Flashcards

Semester 2 Final Review Part 1 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is a chemical reaction?

A

Process by which one or more substance change into one or more new substances

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are reactants?

A

Original substances in a reaction (written on left side)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are products?

A

Substances that are created (written on right)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is a chemical equation?

A

Equation that shows the chemical formulas and relative amounts of all reactants and products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are signs of a chemical reaction?

A

Odor, color change, change in temp, formation of gas, precipitate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is a chemical change?

A

New substance forms with properties that are different from the original substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are some chemical changes?

A

Density, boiling point, melting point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is a physical change?

A

Changes of state which are not chemical changes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are some physical changes?

A

Evaporation, condensation, melting, freezing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

If energy is being released in a chemical reaction than it is a ?

A

Product

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

If energy is being absorbed in a chemical reaction than it is a ?

A

Reactant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is a coefficient?

A

A number in front of the element or compound that multiplies the number of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What happens if you cannot balance the equation do to half odd numbers?

A

Multiply current coefficients by 2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are the five reaction types?

A

Combustion, synthesis, decomposition, single replacement, and double replacement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Why is classifying reactions important?

A

Allows scientists to predict products of reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What happens in a combustion reaction?

A

Carbon molecule reacts with oxygen and products are ALWAYS carbon dioxide and water

Heat is given off

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What happens in a synthesis reaction?

A

Two atoms or compounds are being combined to form one compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What happens in a decomposition reaction?

A

One compound breaks down into two smaller elements or compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Metal oxides and water make what?

A

Metal hydroxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Carbonates break down into what?

A

Metal oxide and carbon dioxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What happens in a single replacement reaction?

A

Single element reacts with compound and displaces another element from compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What happens in a double replacement reaction?

A

Two compounds in an aqueous solution appear to exchange ions to form new compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What must one of the products be in a double replacement reaction?

A

One of the products must be a solid precipitate, a agase, or molecular compound such as water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Metal oxides and carbon dioxide form?

A

Carbonates

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Metal hydroxides break into?

A

Metal oxide and water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Carbonates break down into?

A

Metal oxide and carbon dioxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

How do you know if an element will displace another element?

A

Use the activity series

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

How do you use the activity series?

A

If an element is listed above another element it can displace anything below it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What are the diatomic elements?

A

Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, and Iodine

Never found as single atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What happens to ionic compounds when they dissolve in water?

A

They separate into ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

When does a double replacement reaction take place?

A

If the dissolved ions react to form a precipitate, gas, or liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What are subscripts?

A

Numbers that tell you the number of atoms of that element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

How can you predict if a precipitate will form?

A

Use the Solubility Rules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What are the solubility rules?

A

Guidelines that you use to determine if an ionic compound is soluble or insoluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What does soluble mean?

A

Dissolves in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

What does insoluble mean?

A

Does not dissolve in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What happens if a reaction forms an insoluble ionic compound?

A

Precipitate forms, indicated by (s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

What do total ionic equations show?

A

Show all the soluble ions and insoluble solid, liquid, or gases in compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

What do net ionic equations show?

A

Only the ions that change in a reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

What happens if there is no change?

A

No reaction occurs (solid, liquid, or gas must be formed in order to change)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

What are spectator ions?

A

Ions that remain unchanged in the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

If one of the compounds is not soluble will the reaction take place?

A

Yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

If both of the compounds are soluble will the reaction take place?

A

No reaction occurs

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

What is a word equation?

A

A chemical reaction is expressed in words rather than chemical formulas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

What is stoichiometry?

A

Branch of chemistry that deals with quantities of substances in chemical reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

Can the amount of product be predicted based on your reactants using stoichiometry?

A

Yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

Can you calculate the amount of reactants needed to make the desired amount of product?

A

Yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

Can the amount of by-product be predicted?

A

Yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

What do stoichiometry problems begin with?

A

A balanced chemical equation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

What do coefficients in a balanced chemical equation show?

A

Relative number of moles of a substance in the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

What are coefficients used to determine?

A

The mole ratios

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

What are mole ratios?

A

Conversion factors used to convert moles of one substance into moles of another substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

How do you solve a stoichiometry?

A

Set up mole ratio to cancel out substance that you are given and convert to substance that you want

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

How do you get from mass to moles?

A

Use molar mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

How do you get from volume to moles?

A

Volume (density) to moles

22.4 L in one mol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

What is Avogadro’s number?

A

6.02 x 1023 particles/mol)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

What is a limiting reactant?

A

A substance that controls how much product can form and is used completely in the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

What is a excess reactant?

A

Not completely used up in the reaction, leftover when reaction is complete

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

What is the theoretical yield?

A

The maximum product that can be made, always based on the limiting reactant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

How do you find limiting and excess reactant?

A

Determine how much can be made from either substance, compare their amount of products, theoretical yield is lower amount of product

61
Q

What is actual yield?

A

How much product is actually produced by the reaction, always less than theoretical yield

62
Q

What is a percent yield?

A

Convenient way to describe the efficiency of reaction

63
Q

What is the percent yield equation?

A

(Actual yield/theoretical yield) x 100

64
Q

What is energy?

A

Ability to do work or produce heat

65
Q

What two basic forms does energy exist in?

A

Potential and kinetic energy

66
Q

What is potential energy?

A

Energy due to the composition or position of an object

67
Q

What is kinetic energy?

A

Energy of motion

68
Q

What type of energy do chemical systems contain?

A

Both kinetic and potential energy

69
Q

What is the kinetic energy of a substance related to?

A

The constant random motion of its representative particle and proportional to the temperature

70
Q

What does the potential energy of a substance depend on?

A

The type of atoms, the number and type of chemical bonds, and how the atoms are arranged

71
Q

What is heat?

A

Energy that is in the process of flowing from a warmer object to a cooler object

72
Q

What symbol is used to represent heat?

A

Q

73
Q

What is a calorie (cal)?

A

The amount of energy required to raise the temperature of 1 gram of pure water by 1 degree Celsius

74
Q

What nutritional Calorie equals how many calories?

A

1000 calories or 1 kilocalorie

75
Q

What is a joule?

A

SI unit of heat and energy equivalent to 0.2390 calories

76
Q

What does the total energy of a sample include?

A

Total energy of particles in a sample plus system’s volume times pressure

77
Q

What is the symbol for enthalpy?

A

H

78
Q

What happens as energy transfers away from a sample?

A

Particles kinetic energy slows down (decrease in temp)

79
Q

What does enthalpy equal if the system is at constant pressure?

A

The heat transferred

80
Q

What is temperature?

A

Measure of average kinetic energy of the particle in a sample of matter

81
Q

What is molar heat capacity?

A

Energy needed to increase the temperature of 1 mol of substance by 1 K

82
Q

What is the symbol and unit for molar heat capacity?

A

C and J/k mol

83
Q

What is the molar heat capacity equation?

A

Q= nCΔt

84
Q

What can molar heat capacity be used to calculate?

A

Heat absorbed and released

85
Q

How are molar heat capacity and specific heat capacity related?

A

Molar mass

86
Q

What can you use to find molar mass?

A

M x Cp = C

87
Q

What is thermochemistry?

A

Branch concerned with the energy (heat) changes that accompany chemical and phase changes

88
Q

What does thermochemistry help predict?

A

Whether a chemical reaction will occur and what kind of energy change it will have

89
Q

What is a system?

A

Specific part of the universe that contains the reaction or process

90
Q

What are the surroundings?

A

Everything else other than the system

91
Q

What is the universe defined as in thermochemistry?

A

System + the surroundings

92
Q

What is enthalpy?

A

The heat content of a system at constant pressure

93
Q

How can you find enthalpy?

A

H = internal energy + (pressure x volume)

94
Q

What is the symbol used for enthalpy?

A

H

95
Q

What is the only way to measure the energy of a system?

A

A change in energy which is called molar enthalpy change

96
Q

What would you use if you are looking for specific heat but you are only given mass and temperatures of both substances?

A

-mCpΔt= mCpΔt

97
Q

Positive enthalpy changes are _____?

A

Endothermic

98
Q

Negative enthalpy changes are ____?

A

Exothermic

99
Q

What is 1 Calorie equal to?

A

4.1858 kJ

100
Q

What is 1 joule equal to?

A

0.2390 calories

101
Q

What are 1000 calories equal to?

A

1 Calorie

102
Q

What is a calorimeter?

A

Insulated device used for measuring the amount of heat absorbed or released during a chemical or physical process

103
Q

What does a calorimeter determine?

A

Specific heat of an unknown metal

104
Q

What is a thermochemical equation?

A

Balanced chemical equation that includes the physical states of all reactants and products and energy change

105
Q

What is the energy change usually expressed as?

A

ΔH

106
Q

What is the enthalpy of combustion?

A

ΔHcomb enthalpy change for complete burning of substance

107
Q

What is the molar enthalpy of vaporization?

A

ΔHvap heat required to vaporize one mole of a liquid

108
Q

What is the molar enthalpy of fusion?

A

ΔHfus is the heat required to melt one mole of a solid

109
Q

If ΔH is negative

A

energy is released to the surroundings.

110
Q

If ΔH is positive

A

energy is absorbed from the surroundings.

111
Q

What is calorimetry?

A

Used to measure energy released or absorbed from a reaction by measuring a change in temperature of a standard liquid and setting enthalpy equal to the reaction change

ΔH lost = ΔH gained

112
Q

What can be used to measure calorimetry?

A

-mCpΔt= mCpΔt

113
Q

What is Hess’s Law?

A

If you add 2 or more thermochemical equations to produce a final equation, the sum of enthalpy changes is the enthalpy change for the final reaction

114
Q

Why is the overall enthalpy change equal to the sum of the enthalpy changes?

A

If 2 processes start and end with the same reactants and products, they will have the same enthalpy change, even if the steps are different.

115
Q

How can you use Hess’s Law?

A

Look for products and reactants for the desired equation, manipulate equations to put products and reactants in the correct locations, make sure whatever you do to the equation you do to ΔH

116
Q

What equation is used to determine how the standard enthalpies of formation to determine the enthalpy change in a chemical reaction

A

ΔHrxn = ΔHproducts - ΔHreactants

117
Q

What do you do when a coefficient is in front of the substance in the ΔHrxn = ΔHproducts - ΔHreactants
equation.

A

Multiply the ΔH by the coefficient when determining ΔHrxn

118
Q

What is the standard enthalpy of formation?

A

The change in enthalpy that accompanies the formation of one mole of the compound in its standard state from its elements in their standard states. ΔHf

119
Q

What is entropy?

A

A measure of the number of possible ways that the energy of a system can be distributed, units J/k

120
Q

What is entropy related to?

A

Related to the freedom of the system’s particles to move and the ways they can be arranged

121
Q

Is it true that all systems naturally become more random?

A

Yes

122
Q

What are factors that increase entropy?

A

Particles’ freedom of movement increase, dissolving a solid, increase volume, increase energy, reducing the pressure of a gas

123
Q

When does entropy increase?

A

As a substance changes from a solid to a liquid and from a liquid to a gas

124
Q

If the reaction or process is exothermic, what happens to ΔSsurroundings?

A

Increase of temperature of surroundings occurs and ΔSsurroundings is positive

125
Q

Is it true that elements can have values for S not equal to O

A

Yes

126
Q

Reactions are more likely to occur when?

A

If enthalpy is negative (exothermic reactions), but some still occur if enthalpy is positive

127
Q

A process is more likely to occur if entropy increases because?

A

It is becoming more random

128
Q

What is free energy?

A

Energy that is available or leftover

129
Q

What is it called for the reactions that take place at constant pressure and temperature with free energy?

A

Gibbs Free Energy

130
Q

What is the Gibbs Free Energy Equation?

A

ΔGsystem = ΔHsystem – TΔSsystem

131
Q

What does the tendency of a reaction to occur depend on?

A

Both ΔH and ΔS.

132
Q

What is something to note when doing Gibbs Free Energy?

A

ΔS is given in J/K so it must be put into kJ in order to add or subtract to find ΔG

133
Q

What is a spontaneous reaction?

A

One that, once begun, occurs with no outside assistance (means that reaction is possible)

134
Q

What a reaction is spontaneous what is ΔG?

A

Negative

135
Q

If ΔG is positive what will happen to the reaction?

A

Will not occur

136
Q

If ΔG is 0 what will happen to the reaction?

A

System is at equilibrium

137
Q

A more negative ΔG tends to occur in reactions that?

A

Release a lot of energy

138
Q

ΔG depends on?

A

Temperature

139
Q

A chemical reaction has NOT occurred if the products have?

A

The same chemical properties as the reactants.

140
Q

An insoluble solid produced by a chemical reaction in a solution is called?

A

A precipitate

141
Q

A solid produced by a chemical reaction that then separates from the solution is called a(n)…?

A

Precipitate

142
Q

A _____ is a substance that speeds up a chemical reaction but does not participate in the reaction. It is written over the arrow in a chemical equation.

A

catalyst

143
Q

Chemical equations are balanced so they do not violate the ___________.

A

law of conservation of mass

144
Q

Nonmetal oxides react with water to produce ____________.

A

Acids

145
Q

Enthalpy is?

A

Energy of a system at constant pressure.

146
Q

How is a celsius temperature converted to kelvins?

A

By adding 273.15

147
Q

The greater the kinetic energy of the particles in a sample of matter

A

The higher the temperature is.

148
Q

In the expression q=nCΔT, what do q and n represent?

A

Heat and moles of particles

149
Q

Compared with a single gas, a mixture of gasses is

A

More disordered

Honors Chemistry (13 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions