Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 56

Hydrogen and oxygen usually have oxidation states of +1 and \(-2,\) respectively, in their compounds. The following cases serve to remind us that there are exceptions. What are the oxidation states of the atoms in each of the following compounds? (a) \(\mathrm{MgH}_{2}\) (b) \(\mathrm{CsO}_{3} ;\) (c) HOF; (d) \(\mathrm{NaAlH}_{4}\)

Short Answer

Expert verified
The oxidation states of the atoms in the compounds are: (a) Mg (+2), H (-1); (b) Cs (+1), O (-2); (c) H (+1), O (-2), F (+1); (d) Na (+1), Al (+3), H (-1).

Step by step solution

01

Assign Oxidation States for \(\mathrm{MgH}_{2}\)

Magnesium (Mg) is in group 2 and thus has an oxidation state of +2. Hydrogen generally has an oxidation state of +1, but in this case there are two hydrogens attaching to magnesium, therefore hydrogen needs an oxidation state of -1 to balance the +2 charge. Thus, the oxidation states are Mg (+2) and H (-1).
02

Assign Oxidation States for \(\mathrm{CsO}_{3}\)

Cesium (Cs) is in group 1 and thus has an oxidation state of +1. Oxygen generally has an oxidation state of -2, and there are three of them in the compound. Therefore, the oxidation states are Cs (+1) and O (-2).
03

Assign Oxidation States for HOF

In this molecule, oxygen has its usual oxidation state of -2. Since the total charge of the molecule is 0, the charges of hydrogen and fluorine must balance out the -2 charge. Hydrogen usually has an oxidation state of +1. In order for the total charge to be zero, fluorine must have an oxidation state of +1. Thus, the oxidation states are H (+1), O (-2), and F (+1).
04

Assign Oxidation States for \(\mathrm{NaAlH}_{4}\)

Sodium (Na) is in group 1 and thus has an oxidation state of +1. Aluminum (Al) is in group 13 and thus has an oxidation state of +3. Multiple hydrogen atoms are present and they balance the charge from sodium and aluminum by taking an oxidation state of -1. Thus, the oxidation states are Na (+1), Al (+3), and H (-1).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Nitrogen forms five oxides in which its oxidation states are \(+1,+2,+3,+4,\) and \(+5,\) respectively. Write appropriate formulas for these compounds.

A \(1.562 \mathrm{g}\) sample of the alcohol \(\mathrm{CH}_{3} \mathrm{CHOHCH}_{2} \mathrm{CH}_{3}\) is burned in an excess of oxygen. What masses of \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) should be obtained?

Explain which of the following statement(s) is (are) correct for sorbic acid, \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{2},\) an inhibitor of mold and yeast. (a) It has a \(\mathrm{C}: \mathrm{H}:\) O mass ratio of 3: 4: 1 (b) It has the same mass percent composition as the aquatic herbicide, acrolein, \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}\) (c) It has the same empirical formula as aspidinol, \(\mathrm{C}_{12} \mathrm{H}_{16} \mathrm{O}_{4},\) a drug used to kill parasitic worms. (d) It has four times as many \(\mathrm{H}\) atoms as \(\mathrm{O}\) atoms, but four times as much O as H by mass.

The organic solvent thiophene is a carbon-hydrogensulfur compound that yields \(\mathrm{CO}_{2}, \mathrm{H}_{2} \mathrm{O},\) and \(\mathrm{SO}_{2}\) when burned in an excess of oxygen. When subjected to combustion analysis, a \(1.3020 \mathrm{g}\) sample of thiophene produces \(2.7224 \mathrm{g} \mathrm{CO}_{2}, 0.5575 \mathrm{g} \mathrm{H}_{2} \mathrm{O},\) and \(0.9915 \mathrm{g} \mathrm{SO}_{2} .\) What is the empirical formula of thiophene?

A hydrocarbon mixture consists of \(60.0 \%\) by mass of \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(40.0 \%\) of \(\mathrm{C}_{x} \mathrm{H}_{y} .\) When \(10.0 \mathrm{g}\) of this mixture is burned, \(29.0 \mathrm{g} \mathrm{CO}_{2}\) and \(18.8 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\) are the only products. What is the formula of the unknown hydrocarbon?
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free