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Chapter 4: Problem 100

Consider three molecules: \(\mathrm{A}, \mathrm{B},\) and \(\mathrm{C}\). Molecule A has a hybridization of \(s p^{3} .\) Molecule \(\mathrm{B}\) has two more effective pairs (electron pairs around the central atom) than molecule A. Molecule C consists of two \(\sigma\) bonds and two \(\pi\) bonds. Give the molecular structure, hybridization, bond angles, and an example for each molecule.

Short Answer

Expert verified
Molecule A has an \(sp^3\) hybridization, a tetrahedral molecular structure, bond angles of approximately 109.5°, and an example is methane (CH4). Molecule B has an \(sp^3d^2\) hybridization, an octahedral molecular structure, bond angles of 90°, and an example is sulfur hexafluoride (SF6). Molecule C has an \(sp\) hybridization, a linear molecular structure, bond angles of 180°, and an example is carbon dioxide (CO2).

Step by step solution

01

Molecule A

Molecule A has a hybridization of \(sp^3\). This type of hybridization leads to a tetrahedral molecular structure with bond angles of approximately 109.5°. Example: A classic example of an \(sp^3\) hybridized molecule is methane (CH4), with a central carbon atom bonded to four hydrogen atoms.
02

Molecule B

Molecule B has two more effective pairs (electron pairs around the central atom) than molecule A. Since molecule A has four effective pairs, molecule B must have six effective pairs which corresponds to an \(sp^3d^2\) hybridization. An \(sp^3d^2\) hybridized molecule has an octahedral molecular structure with bond angles of 90°. Example: One example of an \(sp^3d^2\) hybridized molecule is sulfur hexafluoride (SF6), where a central sulfur atom is bonded to six fluorine atoms.
03

Molecule C

Molecule C consists of two sigma (\(\sigma\)) bonds and two pi (\(\pi\)) bonds. Typically, a molecule with this composition has a double bond. A double bond consists of one \(\sigma\) bond and one \(\pi\) bond. Since there are two double bonds, the central atom is bonded to two other atoms, which means the hybridization of the central atom will be \(sp\). The molecular structure would be linear, with a bond angle of 180°. Example: A common example of a molecule with this structure is carbon dioxide (CO2). In CO2, the central carbon atom forms two double bonds with two oxygen atoms.

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Most popular questions from this chapter

Which of the following are predicted by the molecular orbital model to be stable diatomic species? a. \(\mathrm{N}_{2}^{2-}, \mathrm{O}_{2}^{2-}, \mathrm{F}_{2}^{2-}\) b. \(\mathrm{Be}_{2}, \mathrm{B}_{2}, \mathrm{Ne}_{2}\)

Biacetyl and acetoin are added to margarine to make it taste more like butter. Complete the Lewis structures, predict values for all \(\mathrm{C}-\mathrm{C}-\mathrm{O}\) bond angles, and give the hybridization of the carbon atoms in these two compounds. Must the four carbon atoms and two oxygen atoms in biacetyl lie in the same plane? How many \(\sigma\) bonds and how many \(\pi\) bonds are there in biacetyl and acetoin?

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Draw the Lewis structures, predict the molecular structures, and describe the bonding (in terms of the hybrid orbitals for the central atom) for the following. a. \(\mathrm{XeO}_{3}\) b. \(\mathrm{XeO}_{4}\) c. \(\mathrm{XeOF}_{4}\) d. \(\mathrm{XeOF}_{2}\) e. \(\mathrm{XeO}_{3} \mathrm{F}_{2}\)
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