Question

the number of electrons gained or lost when iron reacts with water

Answer 1

Let’s examine the oxidation and reduction reactions that are involved in the redox reaction of rusting. First, iron, in the presence of moisture (H2O) will lose electrons, becoming a positively charged ion in water:

Oxidation reaction: Iron is oxidized (loses e-)

Fe(s) Fe2+(aq) + 2 e-

Those electrons are then used to reduce the oxygen dissolved in the water (remember that water will have some dissolved oxygen and also H+ and OH- ions):

Reduction reaction: Oxygen is reduced (gains e-)

O2 + 4e- + 4 H+ 2 H2O

Those Fe2+ ions react with the OH- ions in water to produce iron hydroxide, which will dry in several steps to produce rust:

Fe2+ + 2OH- Fe(OH)2 Fe2O3 (rust)

Notice that the redox reaction needs water, which explains why a moist environment speeds up the rusting process. Rusting can occur in dry climates, but it tends to happen much more slowly due to the relatively low humidity in the air.

Because it is difficult to remember the definitions of oxidation and reduction that involve the movement of electrons, a common mnemonic that can help you keep these rules in mind is:




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Alplali
Ace