Question

Which one of the following compounds has sp \(^{2}\) hybridization? (a) \(\mathrm{CO}_{2}\) (b) \(\mathrm{SO}_{2}\) (c) \(\mathrm{N}_{2} \mathrm{O}\) (d) \(\mathrm{CO}\)

Short answer

The compound with sp \(^2\) hybridization is (b) SO\(_2\).

Step-by-step solution

Understanding Hybridization

Hybridization is a concept used to predict the shape and bonding properties of molecules. An atom exhibits sp \(^2\) hybridization when one s orbital and two p orbitals mix, resulting in three equivalent orbitals.

Analyze Compound CO2

The carbon atom in CO\(_2\) is double-bonded to each oxygen atom. Carbon uses sp hybridization here (combining one s and one p orbital) as it forms only two bonds resulting in a linear structure.

Analyze Compound SO2

In SO\(_2\), sulfur forms double bonds with each oxygen. It uses sp\(^2\) hybridization, combining one s and two p orbitals, due to the presence of a lone pair and the geometry being trigonal planar.

Analyze Compound N2O

In N\(_2\)O, the bonding involves multiple bonds and linear structure. One of the nitrogen atoms typically uses sp hybridization due to linear geometry.

Analyze Compound CO

In CO, carbon is triple-bonded to oxygen, leading it to use sp hybridization, resulting in a linear structure.

Key concepts

sp2 Hybridization

Hybridization is a concept in chemistry that combines atomic orbitals to form new hybrid orbitals. These new configurations help explain the geometry of molecules and their bonding properties. In the case of sp ybridization, one s orbital and two p orbitals mix, forming three identical sp orbitals. This hybridization type is often associated with molecules having a trigonal planar geometry.

These sp orbitals form * 120-degree angles, * create a flat, triangular shape, * and typically involve one central atom double-bonded to other atoms, sometimes accompanied by a lone pair of electrons.

In the compound , sulfur showcases sp hybridization as it binds with oxygen atoms, forming a planar structure. This contrasts with the linear geometry in and , where sp hybridization occurs.

Molecular Geometry

Molecular geometry is the three-dimensional arrangement of atoms in a molecule. It is crucial in determining many physical and chemical properties, such as reactivity and polarity. The geometry around an atom is predicted using the VSEPR (Valence Shell Electron Pair Repulsion) theory, which considers the repulsion between electron pairs to minimize electron pair repulsion.

For sp hybridized atoms, the geometry is typically trigonal planar. This means that the central atom is surrounded by three groups in the same plane, forming 120-degree angles. An example of trigonal planar geometry is the molecule, where the sulfur atom central point bonds with two oxygen atoms and holds a lone pair of electrons. This arrangement results in the planar shape, characteristic of sp hybridized molecules.

Recognizing molecular geometry helps predict molecular behaviors and interactions, which forms the groundwork for understanding how compounds react and interact on a molecular level.

Chemical Bonding

Chemical bonding involves the force holding atoms together in molecules or compounds. Different types of bonds, such as ionic, covalent, and metallic, vary based on how electrons are shared or transferred between atoms.

In the context of sp hybridization, the focus is often on covalent bonding. Here, atoms share electrons to fulfill the octet rule, stabilizing the molecule. In , sulfur forms double bonds with oxygen atoms, signifying a strong covalent bond with shared electron pairs.

Understanding the type of chemical bonding is crucial since it impacts molecule stability, reactivity, and physical properties such as boiling and melting points. The sp hybridized molecules often have distinct properties due to the specific nature of their bonding and geometric arrangement.