Answer:
The oxidation reaction: Ni → Ni⁴⁺ + 4e.
The reduction reaction: 2Cl₂ + 4e → 4Cl⁻.
Explanation:
- The mentioned reaction: <em>Ni + 2Cl₂ → NiCl₄.</em>
- It is an oxidation-reduction reaction comes from two half reactions.
<em>The oxidation reaction:</em> in it Ni losses 4 electrons and is oxidized to Ni⁴⁺ according to the reaction:
<em>Ni → Ni⁴⁺ + 4e.</em>
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<em>The reduction reaction: </em>every molecule of Cl₂ will gain 2 electrons and is reduced to 2Cl⁻ according to the reaction:
<em>2Cl₂ + 4e → 4Cl⁻.</em>
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- The summation of the two-half reactions will give the reaction:
<em>Ni + 2Cl₂ → NiCl₄.</em>
Energy is not created nor destroyed, therefore it is reused.
The thing you MUST do FIRST is look for any H's, O's, or F's in the equation
1)any element just by itself not in a compound, their oxidation number is 0
ex: H2's oxidation number is 0
ex: Ag: oxidation number is 0 if its just something like Ag + BLA = LALA
2) the oxidation number of H is always +1, unless its just by itself (see #1)
3) the oxidation number of O is always -2, unless its just by itself (see #1)
4) the oxidation number of F is always -1, unless its just by itself (see#1)
ok so after you have written those oxidation numbers in rules 1-4 over each H, F, or O atom in the compound, you can look at the elements that we havent talked about yet
for example::::
N2O4
the oxidation number of O is -2.
since there are 4 O's, the charge is -8. now remember that N2O4 has to be neutral so the N2 must have a charge of +8
+8 divided by 2 = +4
N has an oxidation number of +4.
more rules:
5) the sum of oxidation numbers in a compound add up to 0 (when multiplied by the subscripts!!!) (see above example)
6) the sum of oxidation numbers in a polyatomic ion is the charge (for example, PO4 has a charge of (-3) so
oxidation # of O = -2. (there are 4 O's = -8 charge on that side ) P must have an oxidation number of 5. (-8+5= -3), and -3 is the total charge of the polyatomic ion
Answer:
A reaction in which the chemical properties get changed on addition of two or more compound s