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Chapter 9: Problem 50

Consider the \(\mathrm{SCl}_{2}\) molecule. (a) What is the electron configuration of an isolated S atom? (b) What is the electron configuration of an isolated Cl atom? (c) What hybrid orbitals should be constructed on the S atom to make the S-Cl bonds in \(\mathrm{SCl}_{2} ?\) (d) What valence orbitals, if any, remain unhybridized on the S atom in \(\mathrm{SCl}_{2} ?\)

Short Answer

Expert verified
(a) The electron configuration of an isolated S atom is \(1s^2 2s^2 2p^6 3s^2 3p^4\). (b) The electron configuration of an isolated Cl atom is \(1s^2 2s^2 2p^6 3s^2 3p^5\). (c) The hybrid orbitals needed for S-Cl bonds in \(\mathrm{SCl}_{2}\) are sp3 hybrid orbitals. (d) There are no unhybridized valence orbitals remaining on the S atom in \(\mathrm{SCl}_{2}\) as all four valence orbitals participate in sp3 hybridization.

Step by step solution

01

Part (a) - Electron Configuration of Sulfur

First, we need to determine the electron configuration of an isolated sulfur (S) atom. Sulfur has 16 electrons, and its electron configuration follows the Aufbau principle: S: \(1s^2 2s^2 2p^6 3s^2 3p^4\)
02

Part (b) - Electron Configuration of Chlorine

Next, we need to find the electron configuration of an isolated chlorine (Cl) atom. Chlorine has 17 electrons, and its electron configuration is as follows: Cl: \(1s^2 2s^2 2p^6 3s^2 3p^5\)
03

Part (c) - Hybrid Orbitals for S-Cl Bonds

To determine the hybrid orbitals needed for S-Cl bonds in \(\mathrm{SCl}_{2}\), we take into account the valence shell electron pair repulsion (VSEPR) theory. The central sulfur atom forms two sigma bonds with the two chlorine atoms and has two lone pairs. In VSEPR theory, this arrangement corresponds to a bent molecular geometry with a bond angle of about 104.5 degrees. Thus, we need a hybridization compatible with four orbitals arranging themselves in a bent geometry. This requires the sulfur atom to undergo sp3 hybridization, forming four sp3 hybrid orbitals – two to form sigma bonds with the chlorine atoms and two to hold the lone pairs.
04

Part (d) - Unhybridized Valence Orbitals on Sulfur

As we determined in part (c), sulfur undergoes sp3 hybridization for the \(\mathrm{SCl}_{2}\) molecule. Since all four valence orbitals (one 3s and three 3p) on sulfur are used in the hybridization process, there are no unhybridized valence orbitals remaining on the sulfur atom in \(\mathrm{SCl}_{2}\).

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Most popular questions from this chapter

The nitrogen atoms in \(\mathrm{N}_{2}\) participate in multiple bonding, whereas those in hydrazine, \(\mathrm{N}_{2} \mathrm{H}_{4},\) do not. (a) Draw Lewis structures for both molecules. (b) What is the hybridization of the nitrogen atoms in each molecule? (c) Which molecule has the stronger \(N-N\) bond?

(a) The nitric oxide molecule, NO, readily loses one electron to form the \(\mathrm{NO}^{+}\) ion. Which of the following is the best explanation of why this happens: (i) Oxygen is more electronegative than nitrogen, (ii) The highest energy electron in NO lies in a \(\pi_{2 p}^{*}\) molecular orbital, or (iii) The \(\pi_{2 p}^{*}\) MO in NO is completely filled. (b) Predict the order of the \(\mathrm{N}-\mathrm{O}\) bond strengths in \(\mathrm{NO}, \mathrm{NO}^{+},\) and \(\mathrm{NO}^{-},\) and describe the magnetic properties of each.(c) With what neutral homonuclear diatomic molecules are the \(\mathrm{NO}^{+}\) and \(\mathrm{NO}^{-}\) ions isoelectronic (same number of electrons)?

(a) Methane \(\left(\mathrm{CH}_{4}\right)\) and the perchlorate ion \(\left(\mathrm{ClO}_{4}^{-}\right)\) are both described as tetrahedral. What does this indicate about their bond angles? (b) The \(\mathrm{NH}_{3}\) molecule is trigonal pyramidal, while \(\mathrm{BF}_{3}\) is trigonal planar. Which of these molecules is flat?

Describe the bond angles to be found in each of the following molecular structures: (a) trigonal planar, (b) tetrahedral, (c) octahedral, (d) linear.

(a) What is the difference between hybrid orbitals and molecular orbitals? (b) How many electrons can be placed into each MO of a molecule? (c) Can antibonding molecular orbitals have electrons in them?
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