Redox Reactions

Match

Match the following charges accordingly.

• proton

• electron

• neutron

+

-

0

• +

• -

• 0

Multiple Choice

TRUE or FALSE?

The definition of oxidation has evolved from it just being a reaction involving O₂.

• True

• False

Multiple Choice

In redox reactions that involve transfer of electrons between reactants, the yielded product will be...

• ionic

• covalent

• binary compound

• all of the choices

Dropdown

In redox reactions the involve loss and gain of electrons,

oxidation is defined as ​

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while reduction is defined as ​

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Dropdown

Reducing agent, also known as ​

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, is the species that is ​

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since it ​

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electron

Dropdown

Oxidizing agent, also known as ​

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, is the species that is ​

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since it

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electron​

Multiple Choice

In the reaction, 2Na(s) + Cl₂(g) ⟶ 2NaCl(s), what is the oxidizing agent?

Given the Half-Reaction:

2Na(s) ⟶ 2Na⁺(s) + 2e⁻

Cl₂(g) + 2e⁻ ⟶ 2Cl⁻(s)

• Cl

• Na

• NaCl

Multiple Choice

In the reaction, 2Na(s) + Cl₂(g) ⟶ 2NaCl(s), which species gains electrons?

Given the Half-Reaction:

2Na(s) ⟶ 2Na⁺(s) + 2e⁻

Cl₂(g) + 2e⁻ ⟶ 2Cl⁻(s)

• Cl

• Na

• NaCl

Multiple Choice

In the reaction, 2Na(s) + Cl₂(g) ⟶ 2NaCl(s), what species is oxidized?

Given the Half-Reaction:

2Na(s) ⟶ 2Na⁺(s) + 2e⁻

Cl₂(g) + 2e⁻ ⟶ 2Cl⁻(s)

• Cl

• Na

• NaCl

Multiple Choice

In the reaction, 2Na(s) + Cl₂(g) ⟶ 2NaCl(s), what species is provides electrons?

Given the Half-Reaction:

2Na(s) ⟶ 2Na⁺(s) + 2e⁻

Cl₂(g) + 2e⁻ ⟶ 2Cl⁻(s)

• Cl

• Na

• NaCl

Multiple Choice

In the reaction, 2Na(s) + Cl₂(g) ⟶ 2NaCl(s), what is the reductant?

Given the Half-Reaction:

2Na(s) ⟶ 2Na⁺(s) + 2e⁻

Cl₂(g) + 2e⁻ ⟶ 2Cl⁻(s)

• Cl

• Na

• NaCl

Multiple Choice

Based on the reaction, 2Na(s) + Cl₂(g) ⟶ 2NaCl(s), how many electrons did 2 moles of Na provide?

Given the Half-Reaction:

2Na(s) ⟶ 2Na⁺(s) + 2e⁻

Cl₂(g) + 2e⁻ ⟶ 2Cl⁻(s)

• 1

• 2

• 0

• 3

Multiple Choice

Based on the reaction, 2Na(s) + Cl₂(g) ⟶ 2NaCl(s), how many electrons did 1 mole of Na provide?

Given the Half-Reaction:

2Na(s) ⟶ 2Na⁺(s) + 2e⁻

Cl₂(g) + 2e⁻ ⟶ 2Cl⁻(s)

• 1

• 2

• 0

• 3

Fill in the Blank

-2 + (-3) =

-

Fill in the Blank

-5 - (-3)

-

Fill in the Blank

0 - (-2)

Fill in the Blank

-2 - (-6)

Open Ended

Check Your Learning

Assign oxidation states to the elements whose atoms are underlined in each of the following compounds or ions:

(a) KNO₃

(b) AlH₃

(c) NH₄⁺

(d) H₂PO₄⁻

Open Ended

Balance the following redox reaction that takes place using the oxidation number method:

Al(s) + HCl(aq) $$\rightarrow$$ AlCl₃(aq) + H₂(g)

Open Ended

Balance the following redox reaction using the half-reaction method in an acidic solution.

Fe²⁺(aq) + Cr₂O₇^2-(aq) → Fe³⁺(aq) + Cr³⁺(aq)

Open Ended

REFLECTION:

Chemical reactions need to be balanced, just like the activities in your life.

How do you keep things in your life balanced?