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7 Cards in this Set
- Front
- Back
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oxidation
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*complete loss of electrons
*shift of electrons away from atom in covalent bond *gain of oxygen *loss of hydrogen *increase in oxidation number |
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reduction
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*complete gain of electrons
*shift of electrons toward atom in covalent bond *loss of oxygen *gain of hydrogen *decrease in oxidation number |
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reducing agent
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(always reactants)
substance in a redox reaction that loses electrons |
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oxidizing agent
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(always reactants)
substance in a redox reaction that gains electrons |
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Which atoms are oxidized and which are reduced in this reaction?
Zn + 2MnO2 + 2NH4Cl = ZnCl2 + Mn2O3 + 2NH3 + H2O |
*The element zinc is oxidized b/c it's oxidation number increases 0 to +2. The manganese ion is reduced because its oxidation number decreases +4 to +3.
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Balance the following equation:
Fe2O3 + CO = Fe + CO2 |
1. Assign oxidation numbers.
2. Identify which atoms are oxidized and which are reduced. -Iron decreases in oxidation number from +3 to 0 (reduction) -Carbon increases in oxidation number from +2 to +4 (oxidation) 3. Make the total increase in oxidation number equal to the total decrease in oxidation number by using appropriate coefficients. -The formula Fe2O3 does not need a coefficient b/c the formula already indicates 2 Fe. |
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What is the oxidation number of:
Br- Fe+3 Ca+2 |
Rule #1: The oxidation number of a monatomic ion is equal to its ionic charge.
Br-1: -1 Fe+3: +3 Ca+2: +2 |
