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Mg + PbCl2 --> MgCl2 + Pb. Which statement correctly describes the oxidation and reduction that occur?
Ag+
is oxidized
Mg is oxidized and Pb+2 is reduced
Sn+2
Cu
electrons
be reduced
Fe+3
An oxidizing agent will always
Ag+
is oxidized
Mg is oxidized and Pb+2 is reduced
Sn+2
Cu
electrons
be reduced
Fe+3
A solution of 1.0 M Pb(NO3)2 will not react with a container made of
Ag+
is oxidized
Mg is oxidized and Pb+2 is reduced
Sn+2
Cu
electrons
be reduced
Fe+3
Pb + 2 Ag+ --> Pb+2 + 2 Ag. The chemical species being reduced is
Ag+
is oxidized
Mg is oxidized and Pb+2 is reduced
Sn+2
Cu
electrons
be reduced
Fe+3
In a redox reaction, the species that loses electrons
Ag+
is oxidized
Mg is oxidized and Pb+2 is reduced
Sn+2
Cu
electrons
be reduced
Fe+3
In the reactions Sn+2 + 2 Fe+3 --> Sn+4 + 2 Fe+2, the oxidizing agent is
Ag+
is oxidized
Mg is oxidized and Pb+2 is reduced
Sn+2
Cu
electrons
be reduced
Fe+3
In the reactions Sn+2 + 2 Fe+3 --> Sn+4 + 2 Fe+2, the reducing agent is
Ag+
is oxidized
Mg is oxidized and Pb+2 is reduced
Sn+2
Cu
electrons
be reduced
Fe+3
Oxidation-reduction reactions occur because of the competition between particles for
Ag+
is oxidized
Mg is oxidized and Pb+2 is reduced
Sn+2
Cu
electrons
be reduced
Fe+3
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