Identify the species undergoing oxidation and reduction. a. `H_(2)S(g)+Cl_(2)(g)rarr2HCl(g)+S(s)` b. `3Fe_(3)O_(4)(s)+8Al(s)rarr9Fe(s)+4Al_(2)O_(3)(s)` c. `2Na(s)+H_(2)(g)rarr2NaH(s)`

Identify the species undergoing oxidation and reduction. a. `H_(2)S(g)

1.	Identify the species undergoing oxidation and reduction. a. `H_(2)S(g)+Cl_(2)(g)rarr2HCl(g)+S(s)` b. `3Fe_(3)O_(4)(s)+8Al(s)rarr9Fe(s)+4Al_(2)O_(3)(s)` c. `2Na(s)+H_(2)(g)rarr2NaH(s)`
Answer» (i) `H_(2)S` is oxidised because a more electronegative element , chlorine is added to hydrogen (or a more electropositive element , hydrogen has been removed from S). Chlorine is reduced due to addition of hydrogen to it . (ii) Aluminium is oxidised because oxygen is added to it . ferrous ferric oxide `(Fe_(3)O_(4))` is reduced because oxygen has beem removed from it . (iii) With the careful application of the concept of electronegativity only we may infer that sodium is oxidised and hydrogen is reduced . Reaction (iii) chosen here prompts us to think in terms of another way to define redox reactions .

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Identify the species undergoing oxidation and reduction. a. `H_(2)S(g)+Cl_(2)(g)rarr2HCl(g)+S(s)` b. `3Fe_(3)O_(4)(s)+8Al(s)rarr9Fe(s)+4Al_(2)O_(3)(s)` c. `2Na(s)+H_(2)(g)rarr2NaH(s)`

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