• Metals can be ranked in order of reactivity -this is called the?reactivity series?or just?activity series
• Metals higher in reactivity can?displace?less reactive metals from their compounds in solutions or from their oxides
• An example of a?metal displacement reaction?occurs between magnesium and aqueous copper (II) sulfate solution

Mg (s) + CuSO₄?(aq) → MgSO_4??(aq) +? Cu (s)

• What are the?redox processes?going on here? If we split the equation into half equations it’s easy to see which species is?oxidized?and which is?reduced:

Mg? ?→ Mg²⁺+ 2e^{-? ? ? ? ?}Loss of electrons? =? oxidation

Cu²⁺?+ 2e^-?→ Cu?^{? ? ? ? ? ?}Gain of electrons? =? reduction

• The more reactive metal acts as a?reducing agent
• This allows metals to be ranked from most reactive (strongest reducing agents) to least reactive:

The more reactive a metal is the better it is at pushing electrons onto less reactive metal ions. Magnesium is better at pushing electrons onto copper(II) ions than copper is at pushing electrons onto magnesium ions

Answer:

The correct option is?D.

• • The first reaction tells you that zinc is more reactive than tin (Zn > Sn):

Zn(s) + Sn²⁺(aq) → Zn²⁺(aq) + Sn(s)

• • The second reaction tells you that zinc is more reactive than copper (Zn > Cu):

Cu(s) + Zn²⁺(aq) → No Reaction

• • The third reaction tells you that tin is more reactive than copper (Sn > Cu):

Sn(s) + Cu²⁺(aq) → Sn²⁺(aq) + Cu(s)

• • The fourth reaction tells you that copper is more reactive than silver (Cu > Ag):

Ag(s) + Cu²⁺(aq) → No Reaction

• Given the?activity series?of metals it is possible to predict whether a?displacement reaction?will take place or not ( if it is?feasible)
• For example will calcium displace lead from lead(IV)oxide?

PbO_2??+? 2Ca? →? Pb? +? 2CaO

• Deduce the?redox?half equations

Ca? ?→ Ca²⁺+ 2e^{-? ? ? ? ?}

Pb⁴⁺?+ 4e^-?→ Pb?

• Ca is above Pb in the?activity series, so this reaction is?feasible
• The?more reactive?metal undergoes?oxidation?(Ca in this case)
• The less reactive?metal ion undergoes?reduction