AP Chemistry : AP Chemistry

Study concepts, example questions & explanations for AP Chemistry

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Example Questions

Example Question #31 : Chemical Reactions

For the following unbalanced redox reaction, how many electrons are transferred and which chemical species is being oxidized?

Possible Answers:

Two electrons are transferred; Hg is oxidized

One electron is transferred; Hg is oxidized

Two electrons are transferred; P is oxidized

One electron is transferred; P is oxidized

Correct answer:

Two electrons are transferred; Hg is oxidized

Explanation:

To begin, we will need to separate the given reaction into the two half-reactions by identifying changes in oxidation number. In this case, mercury (Hg) and phosphorus (P) show a change in oxidation number. Mercury begins with an oxidation number of zero, and ends with an oxidation number of . Phosphorus begins with an oxidation number of  and ends with an oxidation number of . Note that the oxidation numbers for fluorine and iodine reamain constant at  for each.

Now we can begin to look at the half-reactions.

Balance the atoms.

Now balance the electrons. We know that each mercury atom loses one electron and each fluorine atom gains one electron.

We can see that two electrons are tranferred. To identify the element being oxidized, we must find the element that is losing electrons. In this case, mercury is being oxidized.

Example Question #1 : Balancing Oxidation Reduction Reactions

How many electrons are involved in the following reaction?

Possible Answers:

2 e-

3 e-

5 e-

1 e- 

4 e-

Correct answer:

5 e-

Explanation:

02

The common factor between 1 e- and 5 e- is 5.  Therefore the number of electrons involved is 5 e-.

Example Question #2 : Oxidation Reduction Reactions

How many electrons are involved in the following reaction?

Possible Answers:

10 e- 

2 e-

5 e-

4 e-

1 e-

Correct answer:

10 e- 

Explanation:

01

The common factor between 2 e- and 5 e- is 10.  Therefore the number of electrons involved is 10 e-.

Example Question #2 : Balancing Oxidation Reduction Reactions

What is the balanced coefficient on OH- for the following reaction:

                (under basic conditions)

Possible Answers:

3

2

5

1

4

Correct answer:

2

Explanation:

03

 

Add them together:

 

Simplify: 

 

Add Hydroxides to each side to counter H+.

 

Simplify:

Example Question #4 : Oxidation Reduction Reactions

What is the sum of all the balanced coefficients in the following reaction:

                    (basic conditions)

Possible Answers:

16

12

10

8

14

Correct answer:

14

Explanation:

04

Add the equations together

 

Simplify

 

Add 2 OH- to each side to cancel out the H+.

 

Simplify:

Example Question #2 : Oxidation Reduction Reactions

For the redox reaction shown, which of the following half reactions occurs in the anode?

Possible Answers:

Correct answer:

Explanation:

Recall that oxidation always occurs at the anode (in both the electrochemical and galvanic cells).  loses two electrons in this case to become . The presence of  is hinted by the ionic compound .

Example Question #301 : Ap Chemistry

When is the oxidation number of H (-1)?

Possible Answers:
Only when it is bonded to Flourine
Never
When it is bonded to a less electronegative element
Only when it is bonded to Chlorine
When it is bonded to a more electronegative element
Correct answer: When it is bonded to a less electronegative element
Explanation:

We typically think of Hydrogen as having an oxidation number of +1.  However when it is bonded to a less electronegative element such as Na it is actually assigned an oxidation number of -1.  

Example Question #1 : Oxidation State

What is the oxidation number of manganese in ?

Possible Answers:

Correct answer:

Explanation:

Potassium always has an oxidation state of , while oxygen always has an oxidation state of . Since we have four oxygens, there is a total charge of  from them.

The most important rule of oxidation numbers is that their sum must equal the charge on the molecule. In this compound, we have .

Manganese needs to cancel out the charge from potassium and oxygen in order to give us a neutral compound.

Example Question #1 : Oxidation State

What is the oxidation number of chlorine in perchlorate?

Possible Answers:

Correct answer:

Explanation:

Perchlorate is a complex ion with the formula .

The most important rule for oxidation number is that the sum of the oxidation states of the atoms must equal the overall molecular charge.

This compound has four oxygens, which always have a oxidation state.

Chlorine usually has an oxidation state of , but in this case it must balance out the oxygens.

Chlorine must be .

Example Question #302 : Ap Chemistry

Consider the following balanced equation:

2Al_{(s)}+3H_2SO_{4\hspace{1 mm}(aq)}\rightarrow Al_2(SO_4)_{3\hspace{1 mm}(aq)}+\hspace{1 mm}H_{2\hspace{1 mm}(g)}

What is the difference between the oxidation state of aluminum on the right side of the equation versus the left?

Possible Answers:

No difference

Correct answer:

Explanation:

2Al_{(s)}+3H_2SO_{4\hspace{1 mm}(aq)}\rightarrow Al_2(SO_4)_{3\hspace{1 mm}(aq)}+\hspace{1 mm}H_{2\hspace{1 mm}(g)}

On the left side of the equation, Al_{(s)} is a solid, so its oxidation state is zero, but on the right side it is in a salt, so it is not in its zero state.

Sulfate, SO_4^{-2}, is an anionic salt, and there are three sulfate ions in each complex, yielding a net charge of -6. The two aluminum ions must have a net charge of +6, which, divided over two aluminum ions, yields an oxidation state of +3 for each aluminum ion.

The difference comes from simple subtraction: 3-0=3.

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