Unit 7 Reactions Exam Review. Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead Copper...
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Unit 7 Reactions Exam Review
Unit 7 Reactions Exam Review. Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead Copper Mercury Silver Which metals would be replaced in a solution
Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead
Copper Mercury Silver Which metals would be replaced in a solution
made from one of their compounds, if a piece of lead metal were
added?
Slide 3
Question 1 Potassium Calcium Sodium Magnesium Aluminum Lead
Copper Mercury Silver Which metals would be replaced in a solution
made from one of their compounds, if a piece of lead metal were
added? Copper, Mercury, Silver
Slide 4
Question 2 Potassium Calcium Sodium Magnesium Aluminum Lead
Copper Mercury Silver You have a mixture that contains solutions of
both Sodium and Aluminum compounds. You wish to recover the
aluminum but not the sodium. What other metal should you add to
this mixture?
Slide 5
Question 2 Potassium Calcium Sodium Magnesium Aluminum Lead
Copper Mercury Silver You have a mixture that contains solutions of
both Sodium and Aluminum compounds. You wish to recover the
aluminum but not the sodium. What other metal should you add to
this mixture? Magnesium
Slide 6
Question 3 Potassium Calcium Sodium Magnesium Aluminum Lead
Copper Mercury Silver Which metals would be replaced in a solution
made from one of their compounds, if a piece of sodium metal were
added?
Slide 7
Question 3 Potassium Calcium Sodium Magnesium Aluminum Lead
Copper Mercury Silver Which metals would be replaced in a solution
made from one of their compounds, if a piece of sodium metal were
added? All of them except Potassium and Calcium Sodium and
below
Slide 8
Question 4 Potassium Calcium Sodium Magnesium Aluminum Lead
Copper Mercury Silver Which of the metals listed above could NOT
then be used to remove the mercury from a nitrate solution?
Slide 9
Question 4 Potassium Calcium Sodium Magnesium Aluminum Lead
Copper Mercury Silver Which of the metals listed above could NOT
then be used to remove the mercury from a nitrate solution?
Silver
Slide 10
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc.
Slide 11
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. Synthesis
Slide 12
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB
Slide 13
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB
Decomposition
Slide 14
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B
Slide 15
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B Single Replacement
Slide 16
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B Single Replacement AB + C AC + B
Slide 17
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B Single Replacement AB + C AC + B Double Replacement
Slide 18
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B Single ReplacementAB + C AC + B Double Replacement AB + CD AD
+ CB
Slide 19
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B Single ReplacementAB + C AC + B Double Replacement AB + CD AD
+ CB Combustion (Complete)
Slide 20
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B Single ReplacementAB + C AC + B Double Replacement AB + CD AD
+ CB Combustion C x H y + O 2 CO 2 + H 2 O (Complete)
Slide 21
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B Single ReplacementAB + C AC + B Double Replacement AB + CD AD
+ CB CombustionC x H y + O 2 CO 2 + H 2 O (Complete) Combustion
(Incomplete)
Slide 22
Question 5 List the types of reactions and write examples of
each using the letters A, B, etc. SynthesisA + B AB DecompositionAB
A + B Single ReplacementAB + C AC + B Double Replacement AB + CD AD
+ CB CombustionC x H y + O 2 CO 2 + H 2 O (Complete) CombustionC x
H y + O 2 CO + H 2 O (Incomplete)
Slide 23
Question 6 Copper metal reacts with silver nitrate solution
What type of reaction that took place between the copper &
silver nitrate?
Slide 24
Question 6 Copper metal reacts with silver nitrate solution
What type of reaction that took place between the copper &
silver nitrate? Single Replacement
Slide 25
Question 7 Copper metal reacts with silver nitrate solution
What is the skeletal chemical reaction equation?
Slide 26
Question 7 Copper metal reacts with silver nitrate solution
What is the skeletal chemical reaction equation? Cu + Ag(NO 3 )
Cu(NO 3 ) 2 + Ag or Cu + Ag(NO 3 ) Cu(NO 3 ) + Ag
Slide 27
Question 8 Copper metal reacts with silver nitrate solution
This reaction shows which metal is more reactive?
Slide 28
Question 8 Copper metal reacts with silver nitrate solution
This reaction shows which metal is more reactive? Copper
Slide 29
Question 9 Sulfur dioxide is produced from the burning of
sulfur. What type of reaction that took place between the sulfur
& oxygen gas?
Slide 30
Question 9 Sulfur dioxide is produced from the burning of
sulfur. What type of reaction that took place between the sulfur
& oxygen gas? Synthesis
Slide 31
Question 10 Sulfur dioxide is produced from the burning of
sulfur. What is the skeletal chemical reaction equation?
Slide 32
Question 10 Sulfur dioxide is produced from the burning of
sulfur. What is the skeletal chemical reaction equation? S + O 2 SO
2
Slide 33
Question 11 Sulfur dioxide is produced from the burning of
sulfur. What is the balanced equation for the reaction?
Slide 34
Question 11 Sulfur dioxide is produced from the burning of
sulfur. What is the balanced equation for the reaction? S + O 2 SO
2
Slide 35
Question 12 In a chemical reaction, what is the relationship
between the total mass of the reactants and the total mass of the
products?
Slide 36
Question 12 In a chemical reaction, what is the relationship
between the total mass of the reactants and the total mass of the
products? They are the SAME (Law of Conservation of Mass)
Slide 37
Question 13 Which substances are the reactants and which are
the products?
Slide 38
Question 13 Which substances are the reactants and which are
the products? Reactants: H 2 & O 2 ; products: H 2 O
Slide 39
Question 14 What is the skeletal chemical reaction
equation?
Slide 40
Question 14 What is the skeletal chemical reaction equation? H
2 + O 2 H 2 O
Slide 41
Question 15 What is the balanced equation for the
reaction?
Slide 42
Question 15 What is the balanced equation for the reaction? 2H
2 + O 2 2H 2 O
Slide 43
Question 16 What type of reaction took place?
Slide 44
Question 16 What type of reaction took place?
Decomposition
Slide 45
Question 17 What is the word equation that describes this
reaction?
Slide 46
Question 17 What is the word equation that describes this
reaction? Hydrogen bromide breaks down into hydrogen gas and
bromine gas
Slide 47
Question 18 What are the reactant(s) and product(s)?
Slide 48
Question 18 What are the reactant(s) and product(s)? Reactants
HBr; products: H 2 and Br 2
Slide 49
Question 19 What is the balanced equation for this
reaction?
Slide 50
Question 19 What is the balanced equation for this reaction?
2HBr H 2 + Br 2
Slide 51
Question 20 Copper metal is heated in an evaporating dish using
a Bunsen burner. After 10 minutes it looses its copper color and
turns black, indicating it has reacted with the oxygen in the air
to make copper oxide. The type of reaction that took place
was?
Slide 52
Question 20 Copper metal is heated in an evaporating dish using
a Bunsen burner. After 10 minutes it looses its copper color and
turns black, indicating it has reacted with the oxygen in the air
to make copper oxide. The type of reaction that took place was?
Synthesis (Cu + O 2 CuO)
Slide 53
Question 21 What are the reactants and products of this
reaction?
Slide 54
Question 21 What are the reactants and products of this
reaction? Reactants: HCl and NaOH; products: NaCl and H 2 O
Slide 55
Question 22 The type of reaction that took place would BEST be
classified as:
Slide 56
Question 22 The type of reaction that took place would BEST be
classified as: Double replacement
Slide 57
Question 23 What is the balanced equation for this
reaction?
Slide 58
Question 23 What is the balanced equation for this reaction?
HCl + NaOH NaCl + H 2 O (skeletal and balanced are same)
Slide 59
Question 24 Clear lead nitrate solution is added to a test tube
containing potassium chloride solution and a white solid
immediately begins to form in the bottom of the test tube. The
products of this reaction are most likely?
Slide 60
Question 24 Clear lead nitrate solution is added to a test tube
containing potassium chloride solution and a white solid
immediately begins to form in the bottom of the test tube. The
products of this reaction are most likely? Lead chloride and
potassium nitrate
Slide 61
Question 25 Clear lead nitrate solution is added to a test tube
containing potassium chloride solution and a white solid
immediately begins to form in the bottom of the test tube. The type
of reaction that took place would BEST be classified as?
Slide 62
Question 25 Clear lead nitrate solution is added to a test tube
containing potassium chloride solution and a white solid
immediately begins to form in the bottom of the test tube. The type
of reaction that took place would BEST be classified as? Double
replacement
Slide 63
Question 26 If the reaction rate was increased for a reaction,
without changing the products, what can you assume was added to the
reaction?
Slide 64
Question 26 If the reaction rate was increased for a reaction,
without changing the products, what can you assume was added to the
reaction? Catalyst
Slide 65
Question 27 In an equation, the number of molecules of a given
substance is indicated by what?
Slide 66
Question 27 In an equation, the number of molecules of a given
substance is indicated by what? Coefficient
Slide 67
Question 28 A piece of Calcium metal is placed in a test tube
containing hydrochloric acid (HCl) and immediately begins to fizz
and disappear. After a few minutes, the test tube begins to get hot
to the touch; when the flaming splint test is preformed a loud
popping noise is heard. This reaction can be classified as
what?
Slide 68
Question 28 A piece of Calcium metal is placed in a test tube
containing hydrochloric acid (HCl) and immediately begins to fizz
and disappear. After a few minutes, the test tube begins to get hot
to the touch; when the flaming splint test is preformed a loud
popping noise is heard. This reaction can be classified as what?
Single replacement
Slide 69
Question 29 A piece of Calcium metal is placed in a test tube
containing hydrochloric acid (HCl) and immediately begins to fizz
and disappear. After a few minutes, the test tube begins to get hot
to the touch; when the flaming splint test is preformed a loud
popping noise is heard. From the flaming splint you can conclude
that one of the products is?
Slide 70
Question 29 A piece of Calcium metal is placed in a test tube
containing hydrochloric acid (HCl) and immediately begins to fizz
and disappear. After a few minutes, the test tube begins to get hot
to the touch; when the flaming splint test is preformed a loud
popping noise is heard. From the flaming splint you can conclude
that one of the products is? Hydrogen gas [ H 2 (g) ]
Slide 71
Question 30 A piece of Calcium metal is placed in a test tube
containing hydrochloric acid (HCl) and immediately begins to fizz
and disappear. After a few minutes, the test tube begins to get hot
to the touch; when the flaming splint test is preformed a loud
popping noise is heard. Would this reaction be endothermic or
exothermic? Explain your answer.
Slide 72
Question 30 A piece of Calcium metal is placed in a test tube
containing hydrochloric acid (HCl) and immediately begins to fizz
and disappear. After a few minutes, the test tube begins to get hot
to the touch; when the flaming splint test is preformed a loud
popping noise is heard. Would this reaction be endothermic or
exothermic? Explain your answer. Exothermic; test tube gets hot to
the touch
Slide 73
Question 31 A piece of Calcium metal is placed in a test tube
containing hydrochloric acid (HCl) and immediately begins to fizz
and disappear. After a few minutes, the test tube begins to get hot
to the touch; when the flaming splint test is preformed a loud
popping noise is heard. The other product is most likely what?
Slide 74
Question 31 A piece of Calcium metal is placed in a test tube
containing hydrochloric acid (HCl) and immediately begins to fizz
and disappear. After a few minutes, the test tube begins to get hot
to the touch; when the flaming splint test is preformed a loud
popping noise is heard. The other product is most likely what?
Calcium chloride (CaCl 2 )
Slide 75
Question 32 Methane gas (CH 4 ) is burned and reacts with
oxygen from the air The type of reaction that took place was?
Slide 76
Question 32 Methane gas (CH 4 ) is burned and reacts with
oxygen from the air The type of reaction that took place was?
Combustion
Slide 77
Question 33 Methane gas (CH 4 ) is burned and reacts with
oxygen from the air What is the balanced equation for the above
reaction?
Slide 78
Question 33 Methane gas (CH 4 ) is burned and reacts with
oxygen from the air What is the balanced equation for the above
reaction? CH 4 + 2O 2 CO 2 + 2H 2 O
Slide 79
Question 34 A substance that enters into a chemical reaction is
called what?
Slide 80
Question 34 A substance that enters into a chemical reaction is
called what? Reactant
Slide 81
Question 35 A substance that is formed by a chemical reaction
is called what?
Slide 82
Question 35 A substance that is formed by a chemical reaction
is called what? Product
Slide 83
Question 36 In a true chemical reaction a new substance must
form. True or False?
Slide 84
Question 36 In a true chemical reaction a new substance must
form. True or False? True (forming a new substance is the
definition of a chemical reaction)
Slide 85
Question 37 What does the stand for?
Slide 86
Question 37 What does the stand for? Yields or Reacts or Forms
or Produces
Slide 87
Question 38 What is the chemical equation for magnesium reacts
with chlorine to produce magnesium chloride?
Slide 88
Question 38 What is the chemical equation for magnesium reacts
with chlorine to produce magnesium chloride? Mg + Cl 2 MgCl 2
Slide 89
Question 39 The total number of atoms of each element remains
the same in a balanced equation. True of False?
Slide 90
Question 39 The total number of atoms of each element remains
the same in a balanced equation. True of False? True
Slide 91
Question 40 The activity series of metals ranks elements in
order of what?
Slide 92
Question 40 The activity series of metals ranks elements in
order of what? Reactivity (Decreasing)
Slide 93
Question 41 CuCl 2 + Mg Cu + MgCl 2 Which is the more active
metal?
Slide 94
Question 41 CuCl 2 + Mg Cu + MgCl 2 Which is the more active
metal? Magnesium (its able to displace the copper)
Slide 95
Question 42 What is a catalyst? Name two ways that catalysts
can change the nature of a chemical reaction.
Slide 96
Question 42 What is a catalyst? Name two ways that catalysts
can change the nature of a chemical reaction. Catalyst is neither
reactant nor product. Not used up in reaction. Speeds up reaction
rate and/or lowers reaction temperature.
Slide 97
Question 43 How would you show that heat was used during a
reaction?
Slide 98
Question 43 How would you show that heat was used during a
reaction? Include the word heat as one of the reactants.
Slide 99
Question 44 How would you show that platinum was being used as
a catalyst?
Slide 100
Question 44 How would you show that platinum was being used as
a catalyst? Place the letters Pt over the top of the reaction
arrow
Slide 101
Question 45 What is the symbol for equilibrium?
Slide 102
Question 45 What is the symbol for equilibrium?
Slide 103
Question 46 Predict the products of the following reaction: Pb
+ Cu(SO 4 ) ______ + ______
Slide 104
Question 46 Predict the products of the following reaction: Pb
+ Cu(SO 4 ) ______ + ______ Pb + Cu(SO 4 ) > Pb(SO 4 ) + Cu
Slide 105
Question 47 N 2 + 3H 2 2NH 3 + Heat In the synthesis of ammonia
(NH 3 ), which direction (forward or reverse) would be favored if:
Temperature was raised Hydrogen was decreased Pressure was
increased
Slide 106
Question 47 N 2 + 3H 2 2NH 3 + Heat In the synthesis of ammonia
(NH 3 ), which direction (forward or reverse) would be favored if:
Temperature was raised Reverse Hydrogen was decreased Pressure was
increased
Slide 107
Question 47 N 2 + 3H 2 2NH 3 + Heat In the synthesis of ammonia
(NH 3 ), which direction (forward or reverse) would be favored if:
Temperature was raised Reverse Hydrogen was decreased Reverse
Pressure was increased
Slide 108
Question 47 N 2 + 3H 2 2NH 3 + Heat In the synthesis of ammonia
(NH 3 ), which direction (forward or reverse) would be favored if:
Temperature was raised Reverse Hydrogen was decreased Reverse
Pressure was increased Forward
Slide 109
Question 48 Draw energy diagrams illustrating endothermic and
exothermic reactions, and one showing the impact of adding a
catalyst.