Oxidation | MCQs

Explanation

A reducing agent, also known as a reductant.

It is a substance that causes another substance to be reduced by donating electrons to it.

In the process, the reducing agent itself becomes oxidized, as it loses electrons.

This means that the reducing agent's oxidation state increases. 

Explanation

In NH₄⁺, nitrogen has an oxidation state of –3 (typical for ammonia-like groups).

In NO₃⁻, nitrogen has an oxidation state of +5 due to its bonding with three oxygen atoms.

Explanation

3-Hexanone is a ketone, and on oxidative cleavage with KMnO₄/H₂SO₄, it splits at the carbonyl group.

The cleavage yields acetic acid (CH₃COOH) and butanoic acid (CH₃CH₂CH₂COOH).

Explanation

Explanation

Methane reacts with oxygen to produce carbon dioxide and water, releasing heat.

This is a combustion reaction, typical for hydrocarbons burning in oxygen.

Explanation

Iron rusts when it reacts with oxygen and water in the air, forming iron hydroxide (Fe(OH)₃).

This compound eventually dehydrates to form iron oxide, the reddish-brown rust.

Explanation

In HNO₃ (nitric acid):

Hydrogen (H) = +1

Oxygen (O) = -2 (×3 = -6)

Let nitrogen = x

So, +1 + x + (−6) = 0

⇒ x = +5

Nitrogen has an oxidation state of +5 in HNO₃.

Explanation

Oxidation is a chemical reaction involving the loss of electrons. 

Oxidation:

When a substance loses electrons during a chemical reaction, it is said to be oxidized. 

Reduction:

The opposite of oxidation is reduction, which is when a substance gains electrons. 

Explanation

Aluminium burns in oxygen with a brilliant white flame, producing aluminium oxide (Al₂O₃).

This reaction is highly exothermic.

It is often seen in thermite reactions and metal combustion demonstrations.

Explanation

When hydrogen sulfide (H2S) reacts with sulfur dioxide (SO2), the reaction produces sulfur (S) and water (H2O).

2H2​S+SO2​→3S+2H2​O

• Reactants: Hydrogen sulfide (H₂S) and Sulfur dioxide (SO₂)

• Products: Elemental Sulfur (S) and Water (H₂O)