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Chapter 22: Problem 34

Name the following compounds and assign oxidation states to the halogens in them: (a) \(\mathrm{BCl}_{3}\), (b) \(\mathrm{Sr}\left(\mathrm{IO}_{4}\right)_{2}\), (c) \(\mathrm{LiOCl}\) (d) \(\mathrm{HClO}\) (e) \(\mathrm{CuClO}\) (f) \(\mathrm{Mg}\left(\mathrm{IO}_{2}\right)\).

Short Answer

Expert verified
The compounds and their corresponding oxidation states of the halogens are as follows: (a) Boron trichloride (BCl3), chlorine has an oxidation state of -1. (b) Strontium periodate (Sr(IO4)2), iodine has an oxidation state of +7. (c) Lithium hypochlorite (LiOCl), chlorine has an oxidation state of +1. (d) Hypochlorous acid (HClO), chlorine has an oxidation state of +1. (e) Copper(I) chlorate (CuClO), chlorine has an oxidation state of +5. (f) Magnesium iodite (Mg(IO2)), iodine has an oxidation state of +3.

Step by step solution

01

(a) Naming and oxidation state of halogen in BCl3)

For the compound BCl3, the name is boron trichloride. The oxidation state of chlorine in boron trichloride is -1.
02

(b) Naming and oxidation state of halogen in Sr(IO4)2)

For the compound Sr(IO4)2, the name is strontium periodate. The oxidation state of iodine in strontium periodate is +7.
03

(c) Naming and oxidation state of halogen in LiOCl)

For the compound LiOCl, the name is lithium hypochlorite. The oxidation state of chlorine in lithium hypochlorite is +1.
04

(d) Naming and oxidation state of halogen in HClO)

For the compound HClO, the name is hypochlorous acid. The oxidation state of chlorine in hypochlorous acid is +1.
05

(e) Naming and oxidation state of halogen in CuClO)

For the compound CuClO, the name is copper(I) chlorate. The oxidation state of chlorine in copper(I) chlorate is +5.
06

(f) Naming and oxidation state of halogen in Mg(IO2))

For the compound Mg(IO2), the name is magnesium iodite. The oxidation state of iodine in magnesium iodite is +3.

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Most popular questions from this chapter

Complete and balance the following equations: (a) $\mathrm{Mg}_{3} \mathrm{~N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ (b) \(\mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (c) $\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ (d) \(\mathrm{NH}_{3}(a q)+\mathrm{H}^{+}(a q) \longrightarrow\) (e) \(\mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow\) Which ones of these are redox reactions?

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