Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 135

An ionic compound of potassium and oxygen has the empirical formula KO. Would you expect this compound to be potassium(II) oxide or potassium peroxide? Explain.

Short Answer

Expert verified
The given compound (KO) has potassium with an oxidation state of +1 and oxygen with an oxidation state of -1. Comparing this with the known compounds potassium(II) oxide (K2O) and potassium peroxide (K2O2), the compound matches the composition and oxidation states of potassium peroxide (K2O2). Therefore, the ionic compound of potassium and oxygen with the empirical formula KO is potassium peroxide (K2O2).

Step by step solution

01

Identify the oxidation state of potassium and oxygen in the given compound

The oxidation state of potassium (K) in the given empirical formula (KO) is +1 since it belongs to Group 1 in the periodic table. The oxidation state of oxygen (O) in the compound is -1, as the total charge of the compound must be neutral.
02

Compare the given compound with the known compounds potassium(II) oxide and potassium peroxide

Potassium(II) oxide (K2O) has the following oxidation states: potassium has an oxidation state of +1 (each potassium ion) and oxygen has an oxidation state of -2. This means there are two potassium ions for each oxygen ion in the compound. Potassium peroxide (K2O2) has the following oxidation states: potassium has an oxidation state of +1 (each potassium ion) and each oxygen in the peroxide ion (O2^2-) has an oxidation state of -1. So there are two potassium ions and one peroxide ion (which contains two oxygen atoms) in this compound.
03

Determine the identity of the given compound based on the comparison

From Step 1, we determined that the given compound (KO) has potassium with an oxidation state of +1 and oxygen with an oxidation state of -1. Comparing this with the oxidation states found in Step 2, we can conclude that the given compound matches the composition and oxidation states of potassium peroxide (K2O2). Therefore, based on the information provided and our analysis, the ionic compound of potassium and oxygen with the empirical formula KO is potassium peroxide (K2O2).

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

An electron is excited from the \(n=1\) ground state to the \(n=\) 3 state in a hydrogen atom. Which of the following statements are true? Correct the false statements to make them true. a. It takes more energy to ionize (completely remove) the electron from \(n=3\) than from the ground state. b. The electron is farther from the nucleus on average in the \(n=3\) state than in the \(n=1\) state. c. The wavelength of light emitted if the electron drops from \(n=3\) to \(n=2\) will be shorter than the wavelength of light emitted if the electron falls from \(n=3\) to \(n=1 .\) d. The wavelength of light emitted when the electron returns to the ground state from \(n=3\) will be the same as the wavelength of light absorbed to go from \(n=1\) to \(n=3\) e. For \(n=3,\) the electron is in the first excited state.

Which of the following statements is(are) true? a. F has a larger first ionization energy than does Li. b. Cations are larger than their parent atoms. c. The removal of the first electron from a lithium atom (electron configuration is 1\(s^{2} 2 s^{1} )\) is exothermic - that is, removing this electron gives off energy. d. The He atom is larger than the \(\mathrm{H}^{+}\) ion. e. The Al atom is smaller than the Li atom.

Small daily doses of lithium carbonate taken orally are often given to treat manic-depressive psychoses. This dosage maintains the level of lithium ion in the blood at about \(1 \times 10^{-3} \mathrm{mol} / \mathrm{L}\) . a. What is the formula of lithium carbonate? b. What mass of lithium ion is present per liter of blood in these patients?

The successive ionization energies for an unknown element are $$\begin{aligned} I_{1} &=896 \mathrm{kJ} / \mathrm{mol} \\ I_{2} &=1752 \mathrm{kJ} / \mathrm{mol} \\ I_{3} &=14,807 \mathrm{kJ} / \mathrm{mol} \\\ I_{4} &=17,948 \mathrm{kJ} / \mathrm{mol} \end{aligned}$$ To which family in the periodic table does the unknown element most likely belong?

In defining the sizes of orbitals, why must we use an arbitrary value, such as 90% of the probability of finding an electron in that region?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

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