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1.
Which would be the best oxidising agent? A. N2O B. NH4Cl C. NO2 D. HNO3 |
Answer
D. HNO3 The nitrogen is in the highest state of +5. Hence it can easily undergo reduction, and hence behave as an oxidising agent. |
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2.
Consider the reaction where ClO3-1 becomes Cl-1 , the chlorine : A. takes up 6 electrons B. takes up 4 electrons C. is unchanged D. takes up 7 electrons |
Answer
A. takes up 6 electrons The Cl in ClO3-1 is +5. It takes up 6e- to become Cl-1 |
| 3. What is the charge of each aluminium ion in aluminium oxide? |
Answer
+3 The formula for aluminium oxide is Al2O3. Each O is -2 hence -6 in total. Thus the Al is +6, which shows that each Al is +3 |
| 4. Does a reducing agent gain or lose electrons? |
Answer
lose electrons A reducing agent itself undergoes an oxidation ½ reaction. Hence it loses electrons. |
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5.
In the following incomplete reaction, the Fe2+ ion is an oxidising agent. What is X most likely? A. Fe B. Fe2+ C. Fe3+ D. Fe4+ |
Answer
Fe Since the Fe2+ ion is an oxidising agent, it must undergo a reduction ½ reaction. |
| 6. Is H2SO4 most likely to be an oxidising agent or a reducing agent? |
Answer
oxidising agent The S is in the +6 state and easily undergoes reduction. Hence the molecule is an oxidising agent. |
| 7. What is meant by a “redox” reaction? |
Answer
A type of reaction that involves a transfer of electrons.
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8.
What is the charge of mercury in: mercury (ii) oxide? |
Answer
+2 The Roman Numeral (ii) refers to the charge of the substance in front of it. Hence Hg+2 |
| 9. Why can redox reactions be used to create electricity? |
Answer
Redox reactions involve a transfer of electrons. Indirect transfer of electrons such as in the Voltaic Cell, produces useful electricity.
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10.
What redox role does ammonia play in this reaction? NH3 + O2 → NO + H2O |
Answer
Reducing Agent The N in ammonia changes from -3 to +2 in NO This is oxidation. Hence ammonia is a reducing agent. |