Question

Among the following compounds, the one that is polar and has the central atom with sp \(^{2}\) hybridization is: (a) \(\mathrm{SiF}\) (b) \(\mathrm{BF}_{3}\) (c) \(\mathrm{HClO}_{2}\) (d) \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Short answer

The polar compound with sp \(^{2}\) hybridization is \( \mathrm{HClO}_{2} \).

Step-by-step solution

Understanding Hybridization

Identify the hybridization of the central atom in each compound. - For \( \mathrm{SiF} \), Silicon typically forms four bonds with tetrahedral geometry, usually sp\(^{3}\) hybridization. - For \( \mathrm{BF}_{3} \), Boron forms three bonds, creating a planar structure indicative of sp\(^{2}\) hybridization.- In \( \mathrm{HClO}_{2} \), Chlorine is the central atom. With one lone pair and two bonds, it indicates sp\(^{2}\) hybridization.- For \( \mathrm{H}_{2} \mathrm{CO}_{3} \),Carbon creates three sigma bonds and no lone pairs, suggesting sp\(^{2}\) hybridization.

Evaluating Molecular Polarity

Consider the symmetry and electronegativity differences to determine polarity:- \( \mathrm{SiF} \):Molecule symmetry or lack of other atoms prevents polarity determination.- \( \mathrm{BF}_{3} \):Symmetrical planar structure with uniform electronegativity differences makes it nonpolar. - \( \mathrm{HClO}_{2} \):Asymmetrical structure and chlorine electronegativity give the molecule a polar characteristic.- \( \mathrm{H}_{2} \mathrm{CO}_{3}\): Although carbon is central and typically sp\(^{2}\) hybridized, symmetrical structure often leads to complex polars; not a simple polar.

Identify the Correct Compound

The compound that meets both criteria of having sp\(^{2}\) hybridization and being polar is \( \mathrm{HClO}_{2} \). It has chlorine as the central atom, exhibiting sp\(^{2}\) hybridization with a polar, asymmetrical molecular structure.

Key concepts

Hybridization in Chemistry

Atoms in molecules form bonds by combining their atomic orbitals to create hybrid orbitals. This process is known as hybridization. You can think of it as a way atoms rearrange their electrons before forming bonds. This rearrangement allows atoms to achieve stable electron configurations by sharing electrons with other atoms.
Here's how hybridization generally works:

• Atomic orbitals, like s and p, mix to form new orbitals called hybrid orbitals.
• These hybrid orbitals determine the geometry and bond angles around the central atom.
• Common types of hybridization include sp, sp², and sp³.

Knowing the type of hybridization helps predict the molecular geometry and reactivity of the molecule.

sp2 Hybridization

sp² hybridization occurs when one s and two p atomic orbitals mix, forming three equivalent sp² hybrid orbitals. This type is quite significant when dealing with molecules that form a trigonal planar structure.
Some critical points about sp² hybridization include:

• The hybridized orbitals lie on the same plane, approximately 120 degrees apart, forming a Y shape.
• The remaining p orbital that is not hybridized is perpendicular to the sp² plane and often participates in forming pi bonds.
• It's common in molecules with double bonds, such as alkenes or aromatic compounds.

Understanding sp² hybridization allows better comprehension of the bonding and properties of many organic compounds.

Molecular Geometry

Molecular geometry is the three-dimensional arrangement of atoms in a molecule. It greatly influences molecular behavior and reactivity. Different types of hybridization result in specific molecular shapes or geometries.
For example:

• In sp² hybridization, the resulting shape is trigonal planar due to the 120-degree bond angles.
• The geometry is influenced by the presence of lone pairs, which can affect the molecular shape by altering the bond angles.

Analyzing molecular geometry helps predict the molecule's physical properties, such as polarity, and its interaction with other molecules.

Chemical Bonds

Chemical bonds are the forces holding atoms together in a molecule. They form due to the attraction between oppositely charged ions or through the sharing of electrons between atoms.
Key points about chemical bonds include:

• There are several types of chemical bonds, such as ionic, covalent, and metallic bonds.
• Covalent bonds, where electrons are shared between atoms, often involve hybridized orbitals for better overlap and stronger interactions.
• The number and types of bonds an atom forms are closely related to its hybridization state.

Understanding chemical bonds is essential for grasping how molecules are constructed and interact in chemical reactions.