Question

12. Fill in the blanks to the following rules for assigning oxidation number. Write your answer on the line provided. 1.Atoms in their free state have an oxidation number of (A)

(+6) \mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2-}(-2)[+6(2)+(-2(7))=-2 Oxygen is assigned an oxidation number of, (c)EXCEPT when it is in a peroxide ion where it has an oxidation state of -1. (+1) \mathrm{H}_{2} \mathrm{O}(-2),(+7) \mathrm{MnO}_{4}^{-}(-2),(+1) \mathrm{H}_{2} \mathrm{O}_{2}(-1) Hydrogen in compounds or ions carries a(D)oxidation state, EXCEPT when combined with a metal cation. . Group (E)+ and 2A atoms in compounds carry oxidation numbers of +1 and +2, respectively. Halogens in binary compounds contain a -1 charge. (+1) \mathrm{HCl}(-1),(+1) \mathrm{NaI}(-1),(+3) \mathrm{BF}_{3}(-1) Given compounds that do not follow rules 1-7, usevalues to assign oxidation(+3)NF3(-1), (+1)ICI(-1)(F)+numbers. The sum of the oxidation numbers of individual atoms in a compound or a complex ion is equal to the charge of the compound or ion. (+1)LiCl(-1), (+2)CaO(-2)

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