Reduction and oxidation reactions
Quiz
•
Chemistry
•
11th - 12th Grade
•
Hard

Jake MCEWAN
Used 11+ times
FREE Resource
7 questions
Show all answers
1.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
When an atom gains electrons, we say that the atom has been:
Reduced
Oxidised
Deionised
Decomposed
Answer explanation
Reduction = gains electrons
Oxidation = loses electrons
Two acronyms/mnemonics that people use to help them remember:
"OIL RIG" = "Oxidation Is Loss, Reduction Is Gain"
"LEO the lion says GER" = "Lose Electrons: Oxidation; Gain Electrons: Reduction"
2.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
2NaCl → 2Na + Cl2
This reaction is an example of:
neither an oxidation nor a reduction reaction.
an oxidation reaction.
a reduction reaction.
an oxidation and reduction reaction.
Answer explanation
In this reaction, the starting reactant is an ionic compound; NaCl consists of Na+ and Cl- ions.
The Na+ gains a negatively charged electron to become Na, and the Cl- loses electrons to become Cl2. Both reduction and oxidation are occurring.
This holds true for any reaction that involves a transfer of electrons; in order for one species to gain electrons, another species has to lose electrons. Reduction must always be accompanied by oxidation.
3.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
Mg + 2AgNO3 → 2Ag + Mg(NO3)2
In this reaction, the species that is being reduced is:
Mg
Ag
Mg2+
Ag+
Answer explanation
When identifying the species being oxidised and reduced, compare each element on either side of the equation.
In this reaction, Mg is becoming Mg2+, and Ag+ is becoming Ag. Thus, Mg is being oxidised to Mg2+ (loses electrons, becomes more positive) and Ag+ is being reduced to Ag (gains electrons, becomes less positive).
Note that the NO3- ion is unchanged throughout the reaction, and is simply changing partners from Ag+ to Mg2+; it is acting as a "spectator ion".
4.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
Zn + CuSO4 → Cu + ZnSO4
In this reaction, the species acting as the oxidising agent is:
Cu2+
Zn2+
Cu
Zn
Answer explanation
An oxidising agent is a chemical that causes another species to become oxidised. It does this by accepting electrons from the oxidised species, and thus is being reduced.
Cu2+ is being reduced to Cu (gains electrons), and is thus the oxidising agent.
Remember:
Oxidising agent = species being reduced
Reducing agent = species being oxidised
5.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
SnCl2 + 2FeCl3 → SnCl4 + 2FeCl2
In this reaction, the species acting as the reducing agent is:
Sn2+
Sn4+
Fe3+
Fe2+
Answer explanation
Slightly more complicated as all species are positive cations, but the same principle holds.
Sn2+ → Sn4+ (more positive = loses electrons = oxidised; reducing agent)
Fe3+ → Fe2+ (less positive = gains electrons = reduced; oxidising agent)
6.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
A solution of Pb(NO3)2 will not react with:
Zn
Fe
Sn
Cu
Answer explanation
On p 141 of the textbook:
Metal-ion solutions will not react with less reactive metals (weaker reducing agents). In the reactivity series of metals, the only metals less reactive than Pb are Cu, Ag, and Au. Thus, Cu will not react with a solution of Pb(NO3)2.
7.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
When magnesium metal is burned in air, it becomes a fine white powder. The magnesium metal has been:
Oxidised
Reduced
Neither oxidised nor reduced
Both oxidised and reduced
Answer explanation
In combustion, a substance is reacted with oxygen, causing it to form an oxide.
Another way to think of oxidation is a gain of oxygen (thus the name "oxidation"), as it is losing electrons to oxygen in the reaction. Conversely, if a species loses oxygen it is being reduced.
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