Experiment 5 - Activity Series of Metal:s . What is reduction? How do you identi

Question

Experiment 5 - Activity Series of Metal:s . What is reduction? How do you identify reduction? 2. What is oxidation? How do you identify oxidation? 3. How do you identify the oxiding agent and the reducing agent? reactive that another metal experimentally in the lab? to balance the equation and include the states. 4. Explain how would you determine if a metal is more s. Write the equations for the following reactions. Make sure a. Zinc metal and hydrochloric acid b. Tin metal and lead sulfate e. Magnesium metal and copper nitrate d. Silver metal and sulfuric acid e. Iron metal and phosphoric acid f. Lead metal and acetic aci

Explanation / Answer

1.Reduction: it is defined as

Addition of electrons

Addition of hydrogen or any electropositive element

Removal of oxygen or any electronegative element in a reaction .

The decrease in oxidation number of a species in a reaction indicates that it has undergone reduction.

2. Oxidation: it is defined as

Removal of electrons

Removal of hydrogen or any electropositive element

Addition of oxygen or any electronegative element.

The increase in oxidation number of a species in a reaction indicates that the species has undergone oxidation.

3. Oxidising and reducing agent: in a reaction any species which losses electrons is a reducing agent. I,e it gives electrons to other species. Reduces other species and undergoes oxidation .

In a reaction Any species which gains electrons is an oxidising agent. I,e accepts electron from other species, oxidises other species and undergoes reduction .

4. Metal + water-----> liberate hydrogen gas------> most reactive metals   

Metal + HCl --------> liberate hydrogen gas -------> reactive metals but less than those which react with water.

Some metals doesn't liberate hydrogen gas with either water or HCl (acid) these are leas reactive metals.

Reactivity order: Metals liberating hydrogen gas from water (ex: Na) > metals liberating hydrogen gas from acids(ex: Fe) > metals that doesn't liberate hydrogen gas with either water or HCl.

Or

Dip a metal piece in aqueous metal solution of the other metal. If the dipped metal displaces the other metal from the solution it means the dipped metal is more reactive than the metal in its aqueous form .

Ex. Dip a zinc rod in aq. Copper solution (CuSO4) there is a copper deposit on zinc rod which implies zinc displaces copper from its aqueous medium. Hence zinc is more reactive metal than copper.

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