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Pb + 2 Ag+ --> Pb+2 + 2 Ag. The chemical species being reduced is
be reduced
increases as electrons are lost
Sn+2
electrons
both an oxidation and reduction reaction
is oxidized
Ag+
Cu
The reaction 2 NaCl --> 2 Na + Cl2 is an example of
be reduced
increases as electrons are lost
Sn+2
electrons
both an oxidation and reduction reaction
is oxidized
Ag+
Cu
An oxidizing agent will always
be reduced
increases as electrons are lost
Sn+2
electrons
both an oxidation and reduction reaction
is oxidized
Ag+
Cu
In a redox reaction, the species that loses electrons
be reduced
increases as electrons are lost
Sn+2
electrons
both an oxidation and reduction reaction
is oxidized
Ag+
Cu
Oxidation-reduction reactions occur because of the competition between particles for
be reduced
increases as electrons are lost
Sn+2
electrons
both an oxidation and reduction reaction
is oxidized
Ag+
Cu
In the reactions Sn+2 + 2 Fe+3 --> Sn+4 + 2 Fe+2, the reducing agent is
be reduced
increases as electrons are lost
Sn+2
electrons
both an oxidation and reduction reaction
is oxidized
Ag+
Cu
As an element is oxidized, its oxidation number
be reduced
increases as electrons are lost
Sn+2
electrons
both an oxidation and reduction reaction
is oxidized
Ag+
Cu
A solution of 1.0 M Pb(NO3)2 will not react with a container made of
be reduced
increases as electrons are lost
Sn+2
electrons
both an oxidation and reduction reaction
is oxidized
Ag+
Cu
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