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Chapter 10: Problem 37

Consider the following molecules. Without using the shortcut rules, determine the oxidation state for each atom in the molecules and show how you calculated it. (a) \(\mathrm{H}_{2}\) (b) \(\mathrm{O}_{2}\) (c) \(\mathrm{Cl}_{2}\) (d) IF

Short Answer

Expert verified
In summary, the oxidation states for each atom in the given molecules are: (a) In H₂, both hydrogen atoms have an oxidation state of 0. (b) In O₂, both oxygen atoms have an oxidation state of 0. (c) In Cl₂, both chlorine atoms have an oxidation state of 0. (d) In IF, iodine (I) has an oxidation state of +1 and fluorine (F) has an oxidation state of -1.

Step by step solution

01

Determine the oxidation state of H₂

In a H₂ molecule, there are two hydrogen atoms bonded together. Since both atoms are the same, the electrons in the bond are equally shared between them. Therefore, each hydrogen atom has an oxidation state of 0.
02

Determine the oxidation state of O₂

In an O₂ molecule, two oxygen atoms are bonded together. As in the case of H₂, the electrons in the bond are equally shared between the two oxygen atoms because both atoms are the same. Thus, the oxidation state for each oxygen atom is also 0.
03

Determine the oxidation state of Cl₂

The Cl₂ molecule is made up of two chlorine atoms bonded together. Again, since both atoms are the same, the electrons in the bond are equally shared between them, and the oxidation state for each chlorine atom is 0.
04

Determine the oxidation state of IF

The IF molecule is formed by the bond between iodine (I) and fluorine (F). Since fluorine is more electronegative than iodine, the electrons in the bond are assigned to the fluorine atom. Therefore, the oxidation state for iodine (I) is +1, and the oxidation state for fluorine (F) is -1. To summarize: (a) In H₂, each hydrogen atom has an oxidation state of 0. (b) In O₂, each oxygen atom has an oxidation state of 0. (c) In Cl₂, each chlorine atom has an oxidation state of 0. (d) In IF, iodine (I) has an oxidation state of +1, and fluorine (F) has an oxidation state of -1.

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Most popular questions from this chapter

Lithium is a very active metal, so active that it reacts with water to make flammable hydrogen gas. \(\mathrm{Li}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{LiOH}(s)+1 / 2 \mathrm{H}_{2}(g)\) (a) What metal would you use in combination with Li to make a battery having the highest voltage? (Consult the EMF series.) (b) Too rapid a discharge of a lithium battery (which can occur if there is a short circuit) can overheat a lithium battery and cause it to explode and catch fire. Why is trying to put out such a fire with water a bad idea? (c) Would lithium be the anode or cathode in a lithium ion battery? Explain.

For each redox reaction, indicate which substance is the oxidizing agent and which is the reducing agent. \(4 \mathrm{Fe}+3 \mathrm{O}_{2} \rightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}\)

\(\mathrm{Ca}+2 \mathrm{H}^{+} \rightarrow \mathrm{Ca}^{2+}+\mathrm{H}_{2}\)

Use the shortcut rules to assign an oxidation state to each atom: (a) \(\mathrm{PF}_{6}\) (b) \(\mathrm{Mo}_{2} \mathrm{O}_{7}^{2-}\) (c) \(\mathrm{HPbO}_{2}^{-}\) (d) \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\)

Tin cans are actually iron plated with tin. What is the advantage of the tin coating?
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