Question

For each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. (b) The greater the orbital overlap in a bond, the shorter the bond. \((\mathbf{c})\) To create a hybrid orbital, you could use the \(s\) orbital For each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. (b) The greater the orbital overlap in a bond, the shorter the bond. \((\mathbf{c})\) To create a hybrid orbital, you could use the \(s\) orbital

Short answer

(a) False: Greater overlap results in a stronger bond. (b) True: Greater overlap leads to shorter bond lengths. (c) True: An s orbital can be used to create hybrid orbitals, such as sp, sp2, or sp3.

Step-by-step solution

Statement (a): The greater the orbital overlap in a bond, the weaker the bond.

False. The greater the orbital overlap in a bond, the stronger the bond. This is because increased overlap between atomic orbitals allows for more effective sharing of electrons, resulting in a stronger bond.

Statement (b): The greater the orbital overlap in a bond, the shorter the bond.

True. A larger orbital overlap results in a stronger bond, and stronger bonds are generally shorter in bond length. When orbitals overlap more effectively, the electrons shared between them can be more tightly held, thus leading to a shorter bond.

Statement (c): To create a hybrid orbital, you could use the s orbital.

True. Hybrid orbitals are formed by combining different types of atomic orbitals, such as s, p, and d orbitals. An s orbital can be combined with a p orbital to create sp, sp2, or sp3 hybrid orbitals, which are used in bonding in various molecular geometries.

Key concepts

Orbital Overlap

One of the key concepts in chemical bonding is orbital overlap. Orbital overlap happens when atomic orbitals on two different atoms overlap to form a bond. The degree of overlap directly impacts the strength and length of the bond. To visualize, think about atomic orbitals as clouds where electrons reside. When these clouds "merge" or overlap, electrons are shared between the two atoms.

• Greater overlap means more electron sharing, leading to a stronger bond.
• Stronger bonds generally result in shorter bond lengths.

To sum up, more overlap means stronger and often shorter bonds, as electrons are more effectively shared which enhances the hold between the atoms.

Hybrid Orbitals

Hybrid orbitals help explain the shapes and bonding in complex molecules. They are formed by merging different atomic orbitals on the same atom. For example, an s and a p orbital can hybridize to create new orbitals like sp, sp2, or sp3. This mixing allows atoms to form the equivalent number of bonds with equal strength and helps maintain the structural integrity of molecules.

• Sp hybrids result from one s and one p orbital and form linear structures.
• Sp2 hybrids result from one s and two p orbitals forming trigonal planar shapes.
• Sp3 hybrids emerge from one s and three p orbitals creating tetrahedral structures.

Because hybrid orbitals allow for different spatial arrangements, they impact how molecules interact, react, and adopt complex structures.

Bond Strength

Bond strength is influenced by how tightly atoms are held together in a molecule. Two main factors affect bond strength:

• Extent of orbital overlap – More overlap equals a stronger bond.
• Electronegativity of the atoms – More electronegative atoms can pull shared electrons closer, adding to bond strength.

Stronger bonds have higher bond dissociation energies, meaning they require more energy to break. By understanding bond strength, it's easier to predict the stability of molecules and explain their chemical reactivity.
In molecular chemistry, knowing the strength of bonds helps chemists design new compounds and anticipate how molecules might behave in different environments.