Redox Reactions
- In reactions, metals generally lose electrons = oxidation.
- In reactions, non - metals generally gain electrons = reduced.
- Metals undergo redox reactions with dilute hydrochloric and dilute sulphuric acids.
Examples
Zn + 2HCl --> ZnCl2 + H2
- Zn goes from 0 to +2 = oxidation.
- H goes from +1 to 0 = reduction.
Mg + H2SO4 --> MgSO4 + H2
- Mg goes from 0 to +2 = oxidation
- H goes from +1 to 0 = reduction
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