Question

What is being oxidized in the following reaction?

2F2(g) + Si(s) $LaTeX: \longrightarrow$ ⟶ SiF4(s)

Explain Why

Answer 1

Si(s) is being oxidized

At left side (reactant side) Si(s) oxidation state is zero, after reacting with Fluorine gas it becomes SiF₄(s) [silicon tetrafluoride]. We know that fluorine is highest electronegative atom in the periodic table, it will never loses electrons. Hence silicon lost four electrons and those four electrons are gained by four fluorine atoms to become fluoride (F^-) ions and then combined with Si⁴⁺ ion to give ionic compound SiF₄ as a solid compound. Loss of electrons or addition of oxygen or decreasing oxidation state from negative to positive is called as oxidation.

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