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Chapter 5: Problem 28

For each of the questions, four choices have been provided. Select the correct alternative. A species \(\mathrm{H}_{3} \mathrm{O}^{+}\) pyramidal in shape. The number of lone pairs of electrons is (a) 0 (b) 1 (c) 2 (d) 3

Short Answer

Expert verified
Answer: There is 1 lone pair of electrons in the \(\mathrm{H}_{3} \mathrm{O}^{+}\) species.

Step by step solution

01

Find the total number of valence electrons

Oxygen has 6 valence electrons, and hydrogen has 1 valence electron, making a total of 3 valence electrons from the hydrogens. Since the species has a positive charge of +1, we will subtract one electron from the total. Total valence electrons = 6 (oxygen) + 3 (hydrogen) - 1 (positive charge) = 8
02

Calculate the number of electron pairs

Divide the total number of valence electrons by 2 to find the number of electron pairs: Number of electron pairs = 8 / 2 = 4
03

Determine the molecular geometry

The \(\mathrm{H}_{3} \mathrm{O}^{+}\) species has a pyramidal shape. In the pyramidal geometry, the central atom (oxygen) forms three covalent bonds with the hydrogen atoms, and there is one lone pair on the central atom (oxygen).
04

Identify the number of lone pairs of electrons

The molecular geometry shows that there is one lone pair of electrons on the central atom (oxygen) in the \(\mathrm{H}_{3} \mathrm{O}^{+}\) species. So, the correct answer is: (b) 1

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Most popular questions from this chapter

For each of the questions, four choices have been provided. Select the correct alternative. The number of sigma and pi bonds in benzene are (a) \(6 \sigma\) and \(3 \pi\) bonds (b) \(12 \sigma\) and \(3 \pi\) bonds (c) \(9 \sigma\) and \(3 \pi\) bonds (d) \(6 \sigma\) and \(6 \pi\) bonds

For each of the questions, four choices have been provided. Select the correct alternative. The lesser covalency of \(\mathrm{FeCl}_{2}\) over \(\mathrm{FeCl}_{3}\) is due to (a) lower polarizing power of \(\mathrm{Fe}^{+2}\) than that of \(\mathrm{Fe}^{+3}\) ion (b) lower polarizing power of \(\mathrm{Fe}^{+3}\) than that of \(\mathrm{Fe}^{+2}\) (c) higher polarizability of \(\mathrm{Fe}^{+3}\) than \(\mathrm{Fe}^{+2}\) (d) higher polarizability of \(\mathrm{Fe}^{+2}\) than \(\mathrm{Fe}^{+3}\)

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