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Ch.4 - Reactions in Aqueous Solution
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblem 50f
Chapter 4, Problem 50f

Determine the oxidation number for the indicated element in each of the following substances: (f) Cl in NaClO4.

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Identify the oxidation number of each element in the compound NaClO₄. Sodium (Na) is in Group 1 of the periodic table, so it has an oxidation number of +1.
Oxygen (O) typically has an oxidation number of -2. Since there are four oxygen atoms, the total contribution from oxygen is 4(-2) = -8.
Let the oxidation number of chlorine (Cl) be x. Write the equation for the sum of oxidation numbers in the compound: +1 (for Na) + x (for Cl) + 4(-2) (for O) = 0.
Simplify the equation: 1 + x - 8 = 0.
Solve for x to find the oxidation number of Cl.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation Number

The oxidation number, or oxidation state, is a value assigned to an element in a compound that reflects its degree of oxidation or reduction. It indicates the number of electrons an atom gains, loses, or shares when forming chemical bonds. Oxidation numbers are crucial for understanding redox reactions and determining the electron flow in chemical processes.
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Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as the fact that the oxidation number of an element in its elemental form is zero, and for monoatomic ions, it equals the charge of the ion. In compounds, the sum of the oxidation numbers must equal the overall charge of the compound. These rules help in systematically determining the oxidation states of elements in various compounds.
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Chlorine Compounds and Oxidation States

Chlorine can exhibit multiple oxidation states, commonly ranging from -1 to +7. In compounds like NaClO4, chlorine typically has a positive oxidation state due to its bonding with more electronegative elements like oxygen. Understanding the common oxidation states of chlorine is essential for accurately determining its oxidation number in different chemical contexts.
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Related Practice
Textbook Question

Determine the oxidation number for the indicated element in each of the following substances: (c) P in AgPF6

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Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) P4(s) + 10 HClO(aq) + 6 H2O(l) → 4 H3PO4(aq) + 10 HCl(aq) (b) Br2(l) + 2 K(s)→ 2 KBr(s) (c) CH3CH2OH(l) + 3 O2(g) → 3 H2O(l) + 2 CO2(g) (d) ZnCl2(aq) + 2 NaOH(aq) → Zn(OH)2(s) + 2 NaCl(aq)

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Determine the oxidation number for the indicated element in each of the following substances: (e) Pt in PtCl4 (f) O in OF2.

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Which element is oxidized, and which is reduced in the following reactions? (a) N2(g) + 3 H2(g) → 2 NH3(g)

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Determine the oxidation number for the indicated element in each of the following substances: (d) N in HNO3

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