Consider three molecules: A, B, and 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 \(\mathrm{C}\) 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 sp^3 hybridization with a tetrahedral structure and bond angles of 109.5 degrees, such as in Methane (CH4). Molecule B has sp^3d^2 hybridization with an octahedral structure and bond angles of 90 degrees, such as in Sulfur hexafluoride (SF6). Molecule C has two σ bonds and two π bonds, suggesting sp or sp^2 hybridization. An example is Ethene (C2H4) with sp^2 hybridization, a trigonal planar structure, and bond angles of 120 degrees.

Step by step solution

01

Molecule A Properties

Molecule A is given with a hybridization of sp^3. This means it has 4 effective pairs (electron pairs) around the central atom. These electron pairs could be either bonding or lone pairs. Since it's hybridized with sp^3, it has a tetrahedral molecular structure, and bond angles of approximately 109.5 degrees.
02

Molecule A Example

One example of a molecule with sp^3 hybridization is Methane (CH4). In this case, the carbon atom is the central atom and all four electron pairs are bonding pairs. All four hydrogen atoms are bonded to the carbon using single sigma bonds, making the molecular structure tetrahedral.
03

Molecule B Properties

Molecule B is said to have two more effective pairs than molecule A. Since molecule A has 4 effective pairs, molecule B has a total of 6 effective pairs. This means that the central atom in molecule B is hybridized with sp^3d^2 hybrid orbitals. With 6 effective pairs, the molecular structure would be octahedral and the bond angles equal to 90 degrees.
04

Molecule B Example

One example of a molecule with sp^3d^2 hybridization is Sulfur hexafluoride (SF6). In this case, the sulfur atom is the central atom and all six electron pairs are bonding pairs. Six fluorine atoms are bonded to the sulfur using single sigma bonds, making the molecular structure octahedral.
05

Molecule C Properties

Molecule C consists of two σ (sigma) bonds and two π (pi) bonds, and we need to determine its molecular structure, hybridization, and bond angles. Given the presence of two π bonds, the central atom must be either in sp or sp^2 hybridization.
06

Molecule C Example

An example of a molecule with two σ bonds and two π bonds is Ethene (C2H4). In this case, each carbon atom is hybridized with sp^2 orbitals. Ethene has a trigonal planar molecular structure, and bond angles are approximately 120 degrees.

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