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Chapter 9: Problem 47

For each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. (b) The greater the orbital overlap in a bond, the shorter the bond. (c) To create a hybrid orbital, you could use the sorbital on one atom with a porbital on another atom. (d) Nonbonding electron pairs cannot occupy a hybrid orbital.

Short Answer

Expert verified
(a) False - Greater orbital overlap leads to a stronger bond. (b) True - Greater orbital overlap leads to a shorter bond. (c) False - Hybrid orbitals are formed on the same atom by combining its atomic orbitals. (d) False - Nonbonding electron pairs can occupy hybrid orbitals.

Step by step solution

01

Statement (a)

The greater the orbital overlap in a bond, the weaker the bond. This statement is **false**. The greater the orbital overlap in a bond, the stronger the bond. In simple terms, the more overlapping between orbitals leads to a higher electron density between atoms resulting in a stronger attraction between the positively charged nuclei and the electrons, hence, a stronger bond is formed.
02

Statement (b)

The greater the orbital overlap in a bond, the shorter the bond. This statement is **true**. In cases where there is more overlapping, the electron density is higher between the atoms. Due to this increased electron density, the nuclei of both atoms are attracted more, and as a result, the bond length decreases. Hence, a greater orbital overlap leads to a shorter bond.
03

Statement (c)

To create a hybrid orbital, you could use the s-orbital on one atom with a p-orbital on another atom. This statement is **false**. Hybrid orbitals are formed on the same atom by combining its different atomic orbitals, such as s, p, and d orbitals (if available). The creation of hybrid orbitals occurs before the bond formation. However, the mix of atomic orbitals is determined by how many other atoms are bonded to the nucleus of the atom in question. After these hybrid orbitals are formed, they then overlap with orbitals from other atoms to form chemical bonds.
04

Statement (d)

Nonbonding electron pairs cannot occupy a hybrid orbital. This statement is **false**. Nonbonding electron pairs can and do occupy hybrid orbitals. These nonbonding electron pairs are also called lone pairs. In molecules, these lone pairs are located in hybrid orbitals that are not involved in bonding with other atoms. Hence, nonbonding electron pairs can exist in a hybrid orbital.

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Most popular questions from this chapter

Place the following molecules and ions in order from smallest to largest bond order: \(\mathrm{H}_{2}^{+}, \mathrm{B}_{2}, \mathrm{N}_{2}^{+}, \mathrm{F}_{2}^{+},\) and \(\mathrm{Ne}_{2}\) .

Name the proper three-dimensional molecular shapes for each of the following molecules or ions, showing lone pairs as needed: \((\mathbf{a}) \mathrm{ClO}_{2}^{-}(\mathbf{b}) \mathrm{SO}_{4}^{2-}(\mathbf{c}) \mathrm{NF}_{3}(\mathbf{d}) \mathrm{CCl}_{2} \mathrm{Br}_{2}(\mathbf{e}) \mathrm{SF}_{4}^{2+}\)

Describe the characteristic electron-domain geometry of each of the following numbers of electron domains about a central atom: \((\mathbf{a}), \mathbf{( b )} 4,(\mathbf{c}) 5,(\mathbf{d}) 6\)

What is the hybridization of the central atom in (a) \(\mathrm{SiCl}_{4}\), \((\mathbf{b}) \mathrm{HCN},(\mathbf{c}) \mathrm{SO}_{3},(\mathbf{d}) \mathrm{TeCl}_{2} ?\)

(a) Sketch the molecular orbitals of the \(\mathrm{H}_{2}^{-}\) ion and draw its energy-level diagram.(b) Write the electron configuration of the ion in terms of its MOs. (c) Calculate the bond order in \(\mathrm{H}_{2}^{-} .(\mathbf{d})\) Suppose that the ion is excited by light, so that an electron moves from a lower-energy to a higher-energy molecular orbital. Would you expect the excited-state \(\mathrm{H}_{2}\) -ion to be stable? (e) Which of the following statements about part (d) is correct: (i) The light excites an electron from a bonding orbital to an antibonding orbital, (ii) The light excites an electron from an antibonding orbital to a bonding orbital, or (iii) In the excited state there are more bonding electrons than antibonding electrons?
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