Redox Concepts

What is oxidation?

• Oxidation is the gain of electrons.

• Oxidation is the process of reducing a substance.

• Oxidation is the loss of electrons.

• Oxidation is the opposite of reduction.

Define reduction in terms of redox reactions.

• Reduction is the loss of electrons by a molecule, ion, or atom, resulting in an increase in oxidation state.

• Reduction is the gain of electrons by a molecule, ion, or atom, resulting in a decrease in oxidation state.

• Reduction is the process of converting a substance into its oxidized form.

• Reduction is the reaction where oxygen is gained by a substance.

Give an example of an oxidizing agent.

• Carbon dioxide

• Sodium chloride

• Hydrogen peroxide (H2O2)

• Chlorine gas

Name a common reducing agent used in redox reactions.

• Aluminum oxide (Al2O3)

• Sodium chloride (NaCl)

• Oxygen gas (O2)

• Hydrogen gas (H2)

Explain what a half-reaction is in the context of redox chemistry.

• A half-reaction involves only the reduction part

• A half-reaction involves only the oxidation part

• A half-reaction in redox chemistry represents either the oxidation or reduction part of a complete redox reaction.

• A half-reaction is a complete redox reaction

How do you balance redox reactions using the half-reaction method?

• Use the trial-and-error method to balance redox reactions.

• Guess the coefficients for each element in the reaction.

• Follow the steps of the half-reaction method to balance redox reactions.

• Balance redox reactions by randomly assigning numbers to elements.

What is the oxidation number of an element in its elemental form?

• 1

• 0

• -1

• 2

How can you determine the oxidation number of an element in a compound?

• Count the number of vowels in the element's name

• Flip a coin to decide the oxidation number

• Ask a friend for their opinion

• Follow the rules based on the type of element and its position in the compound.

Provide an example of a redox reaction and balance it.

• 2H2 + O2 -> 2H2O

• 4Fe + 3O2 -> 2Fe2O3

• NaCl + H2O -> NaOH + HCl

• Cu + 2HCl -> CuCl2 + H2

Why is it important to balance redox reactions?

• To ensure conservation of mass and charge, and to accurately represent the reaction.

• To change the products of the reaction

• To add complexity to the reaction

• To speed up the reaction rate