The Activity Series of the Elements (11.1.4) Flashcards
• The spontaneity of a redox reaction depends on the relative redox strengths of
the component species.
• The spontaneity of a redox reaction depends on the relative redox strengths of
the component species.
• There is an inverse relationship between the strength of a metal as a reductant
and its cation as an oxidant; a metal that is a strong reductant will have a cation
that is a weaker oxidant.
• There is an inverse relationship between the strength of a metal as a reductant
and its cation as an oxidant; a metal that is a strong reductant will have a cation
that is a weaker oxidant.
• The redox activity series relates the relative redox strengths of elements.
• The redox activity series relates the relative redox strengths of elements.
When copper wire is placed into a solution of silver
nitrate (AgNO3), a redox reaction occurs resulting in
a solution of copper nitrate Cu(NO3)2 and silver
metal (Ag0
). In this reaction Cu is oxidized (donates
electrons) and Ag+
is reduced (gains electrons).
The reducing agent is Cu, while the oxidizing
agent is Ag+
.
The spontaneity of this redox reaction depends on
the relative redox strengths of the component
species.
If a silver spoon is placed into the solution the
reverse reaction will not occur. Copper metal is a
better reducing agent than silver metal (it is able to
lose electrons more easily), thus silver metal
cannot react with Cu(NO3)2 to reform Cu0
and
AgNO3.
There is an inverse relationship between the
strength of a metal as a reductant and its cation as
an oxidant; a metal that is a strong reductant will
have a cation that is a weak oxidant.
If a strip of zinc metal were placed in a solution of
copper nitrate Cu(NO3)2 what would happen? The
answer depends on which is the better reducing
agent, copper metal or zinc metal (which is able to
donate electrons more easily?).
The redox activity series reveals relative redox
strengths of elements.
The chart shows that copper cation is a better
oxidizing agent (oxidant) than zinc cation, therefore,
copper cation is more easily reduced than zinc
cation. This means that Cu(NO3)
2
would react with
Zn0
to form Cu0
and Zn(NO3)2.
When copper wire is placed into a solution of silver
nitrate (AgNO3), a redox reaction occurs resulting in
a solution of copper nitrate Cu(NO3)2 and silver
metal (Ag0
). In this reaction Cu is oxidized (donates
electrons) and Ag+
is reduced (gains electrons).
The reducing agent is Cu, while the oxidizing
agent is Ag+
.
The spontaneity of this redox reaction depends on
the relative redox strengths of the component
species.
If a silver spoon is placed into the solution the
reverse reaction will not occur. Copper metal is a
better reducing agent than silver metal (it is able to
lose electrons more easily), thus silver metal
cannot react with Cu(NO3)2 to reform Cu0
and
AgNO3.
There is an inverse relationship between the
strength of a metal as a reductant and its cation as
an oxidant; a metal that is a strong reductant will
have a cation that is a weak oxidant.
If a strip of zinc metal were placed in a solution of
copper nitrate Cu(NO3)2 what would happen? The
answer depends on which is the better reducing
agent, copper metal or zinc metal (which is able to
donate electrons more easily?).
The redox activity series reveals relative redox
strengths of elements.
The chart shows that copper cation is a better
oxidizing agent (oxidant) than zinc cation, therefore,
copper cation is more easily reduced than zinc
cation. This means that Cu(NO3)
2
would react with
Zn0
to form Cu0
and Zn(NO3)2.
This list of reduction reactions is a helpful tool for predicting how two metals and metal ions will interact with one another. Which statement about the redox activity series is not correct?
As you move down the list, the ability of the metal component to reduce another metal increases. (C)
The metal component that acts as a reducing agent is the metal form, listed on the right hand side. As you move down the list, the ability of the metal component to reduce another metal decreases.
Which statement about an oxidant and its corresponding reducing agent is correct?
Example: In the reaction
K+ (aq) + e− → K(s)
K+ is the oxidant and K(s) is its corresponding reducing agent.
A strong oxidant will have a weak corresponding reducing agent. (A)
As a general rule, the stronger the oxidant, the weaker its corresponding product reducing agent. Conversely, the stronger the reducing agent, the weaker its corresponding product oxidant is.
When a copper wire is placed in silver nitrate solution:
Cu(s) + 2Ag(NO3 ) (aq) → Cu(NO3 )2(aq) + 2Ag(s)
The final solution is blue in color. In addition, a metallic powder precipitates. Which of the following correctly summarizes this event?
Ag(NO3 ) (aq) is the oxidant. Cu(s) is the reducing agent. Cu(NO3 )2(aq) is the final solution. Ag(s) is the metallic powder. (A)
Cu(s) is oxidized by the oxidant, Ag(NO3 ) (aq). Ag(NO3 ) (aq) is reduced by the reducing agent, Cu(s). The only solution in the product is Cu(NO3 )2(aq); therefore, this is the final solution. The only metal product is Ag(s), and this is the metallic powder.
In an expanded redox activity series, aluminum is located above iron. Which statement correctly predicts what will happen (or not happen) when these two metals and its cations interact?
Aluminum will act as the stronger reducing agent and iron metal ion will act as the stronger oxidant. (B)
This is correct because aluminum is the stronger reducing agent. We know this because aluminum is located above iron in the series.
