Question

question 12 (1 point)
in the reaction $ce{fe(s) + o_{2}(g) -> fe_{2}o_{3}(s)}$
which element loses electrons in the process?

$circ$ iron

$circ$ oxygen

$circ$ iron and oxygen

$circ$ iron (iii) oxide

$circ$ no element loses electrons

Explanation:

In the reaction \( \text{Fe}(s) + \text{O}_2(g)
ightarrow \text{Fe}_2\text{O}_3(s) \), we analyze the oxidation states. Iron (Fe) in its elemental form (Fe(s)) has an oxidation state of 0. In \( \text{Fe}_2\text{O}_3 \), the oxidation state of Fe is +3 (since oxygen has an oxidation state of -2, and for the compound to be neutral, \( 2x + 3(-2) = 0 \) gives \( x = +3 \)). An increase in oxidation state means the element is oxidized, and oxidation involves losing electrons. Oxygen (O) in \( \text{O}_2(g) \) has an oxidation state of 0, and in \( \text{Fe}_2\text{O}_3 \), it has an oxidation state of -2, so it is reduced (gains electrons). So iron loses electrons.

Answer:

A. iron