OXIDAT ATION-REDUCTION REACTIONS this case iron ih a strosger r reducing agent t

Question

OXIDAT ATION-REDUCTION REACTIONS this case iron ih a strosger r reducing agent than copper since the copper l) lons were sodium metal is added to the in Therefore, sodium is a stronger reducing agent than baction occurs metal is added to the original copper(Ill sact solution, no agent than both iron or copper. Finally, If silver Ag(c' + ar'. Iaal no reaction silver i, not capable of reducing the copper(I) ions because copper is a stronger reducing agent than silver. If the data from all four of the above reactions is complled. a st of Increasing strengths can be written. weak strong t Na reducing agents Fe Na" Fe2+ oxidizing agents weak Ag Ag. strong In this experiment you will perform several reactions to determine the relative strengths of oxidlzing and reducing agents. You willl also write balanced redox equa using the half reaction method, for each reaction that occurs Objectives In this experiment. you will perform several displacement reactions with metals to determine their relative strengths as oxidizing and reducing agents: write redox equations for all reactions that occur: and. prepare a table of half-reactions for the metals tested in order of their rela- tive strength as oxidizing agents EQUIPMENT graduated cylinder (10 mL beaker (50 mL) 6 to 8 test tubes laboratory burner ring stand and ring wire gauze watch glass dropper pipet forceps

Explanation / Answer

The colour of SnCl2 is yellow, where the Oxidation Number of Sn is +2. Also, when it undergoes transition to +4 state, the number of electrons that are unpaired is 0 in such a +4 state. So, there are no electrons which can absorb energy, to show a certain colour for the compound, as all the electrons are paired. Hence, the compound SnCl4 is clear in colour.

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