Oxidation-Reduction Reactions (4.2.3)

Question 1

• In an oxidation-reduction reaction, electrons are transferred between a pair of reacting species.

Answer 1

• In an oxidation-reduction reaction, electrons are transferred between a pair of reacting species.

Question 2

• An oxidation-reduction reaction involves two half-reactions.

Answer 2

• An oxidation-reduction reaction involves two half-reactions.

Question 3

• Oxygen is a powerful oxidizing agent (oxidant) as can be seen in the formation of rust during which iron loses electrons to oxygen.

Answer 3

• Oxygen is a powerful oxidizing agent (oxidant) as can be seen in the formation of rust during which iron loses electrons to oxygen.

Question 4

In an oxidation-reduction reaction, electrons are
transferred between a pair of reacting species.
The oxidizing agent (oxidant), in this case the silver
ion, gains electrons. The reducing agent
(reductant), in this case copper, donates electrons.
Oxidation involves a loss of electrons and reduction
involves a gain of electrons.
An oxidation-reduction reaction involves two halfreactions.

Magnesium metal reacts, in an oxidation-reduction
reaction, with hydrochloric acid to produce hydrogen
gas. In the first half-reaction, oxidation involves the
loss of two electrons from the magnesium atom. In
the second half-reaction, reduction involves the gain
of an electron each by two hydrogen ions.
The two half-reactions can be combined, by
summing, to produce the full reaction. The
transferred electrons cancel on either side.
The oxidation reaction gets its name from oxygen,
which is a powerful oxidizing agent (oxidant).
A common oxidation-reduction reaction is the
rusting of iron. In this reaction, iron undergoes
oxidation involving a loss of electrons and oxygen
undergoes reduction involving a gain of electrons.
Iron(III) oxide (rust) forms in a later reaction with
water.

Answer 4

In an oxidation-reduction reaction, electrons are
transferred between a pair of reacting species.
The oxidizing agent (oxidant), in this case the silver
ion, gains electrons. The reducing agent
(reductant), in this case copper, donates electrons.
Oxidation involves a loss of electrons and reduction
involves a gain of electrons.
An oxidation-reduction reaction involves two halfreactions.

Magnesium metal reacts, in an oxidation-reduction
reaction, with hydrochloric acid to produce hydrogen
gas. In the first half-reaction, oxidation involves the
loss of two electrons from the magnesium atom. In
the second half-reaction, reduction involves the gain
of an electron each by two hydrogen ions.
The two half-reactions can be combined, by
summing, to produce the full reaction. The
transferred electrons cancel on either side.
The oxidation reaction gets its name from oxygen,
which is a powerful oxidizing agent (oxidant).
A common oxidation-reduction reaction is the
rusting of iron. In this reaction, iron undergoes
oxidation involving a loss of electrons and oxygen
undergoes reduction involving a gain of electrons.
Iron(III) oxide (rust) forms in a later reaction with
water.