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

Expert verified
(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

01

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.
02

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.
03

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.

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