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Chapter 9: Problem 7

The orbital diagram that follows presents the final step in the formation of hybrid orbitals by a silicon atom. What type of hybrid orbital is produced in this hybridization? [Section 9.5\(]\)

Short Answer

Expert verified
The type of hybrid orbital produced in the hybridization of a silicon atom is the sp³ hybrid orbital. This is because silicon combines one 3s and three 3p orbitals, obtaining a total of four orbitals participating in the hybridization process.

Step by step solution

01

Determine the electron configuration of silicon

First, we need to determine the electron configuration of a silicon (Si) atom. Silicon has 14 electrons. Its electron configuration is: 1s² 2s² 2p⁶ 3s² 3p²
02

Identify the valence electron orbitals

Next, let's identify the orbitals containing the valence electrons. In the electron configuration we found, the valence electrons are in the 3s and 3p orbitals. The valence electron configuration for silicon is: 3s² 3p²
03

Determine the orbitals participating in the hybridization

We need to figure out which orbitals are involved in the hybridization process. Since silicon has 4 valence electrons (2 in 3s and 2 in 3p), it needs 4 orbitals to accommodate these electrons. Silicon merges one 3s and three 3p orbitals in the hybridization process.
04

Identify the type of hybrid orbitals formed

Since silicon combines one 3s and three 3p orbitals, we have a total of four orbitals participating in the hybridization process. Therefore, the type of hybrid orbitals formed is sp³ hybrid orbitals. In conclusion, the type of hybrid orbital produced in the hybridization of a silicon atom is the sp³ hybrid orbital.

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Most popular questions from this chapter

Draw the Lewis structure for each of the following molecules or ions, and predict their electron-domain and molecular geometries: (a) \(\mathrm{AsF}_{3},\) (b) \(\mathrm{CH}_{3}^{+},\) (c) \(\mathrm{BrF}_{3},\) (d) \(\mathrm{ClO}_{3}^{-},\) (e) \(\mathrm{XeF}_{2}\), (f) \(\mathrm{BrO}_{2}^{-}\).

In the series \(\mathrm{SiF}_{4}, \mathrm{PF}_{3},\) and \(\mathrm{SF}_{2},\) estimate the \(\mathrm{F}-\mathrm{X}-\mathrm{F}\) bond angle in each case and explain your rationale. [Section 9.2\(]\)

In which of these molecules or ions does the presence of nonbonding electron pairs produce an effect on molecular shape, assuming they are all in the gaseous state? (a) \(\mathrm{SiH}_{4}\) (b) \(\mathrm{PF}_{3},\) (c) \(\mathrm{HBr}\), (d) \(\mathrm{HCN},\) (e) \(\mathrm{SO}_{2}\)

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

Draw sketches illustrating the overlap between the following orbitals on two atoms: (a) the \(2 s\) orbital on each atom, (b) the \(2 p_{z}\) orbital on each atom (assume both atoms are on the \(z\) -axis), \((\mathrm{c})\) the \(2 s\) orbital on one atom and the \(2 p_{z}\) orbital on the other atom.
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