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Chapter 9: Problem 47

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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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

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 鈥� More overlap equals a stronger bond.
  • Electronegativity of the atoms 鈥� 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.

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Most popular questions from this chapter

Consider the \(\mathrm{SCl}_{2}\) molecule. (a) What is the electron configuration of an isolated \(\mathrm{S}\) atom? (b) What is the electron configuration of an isolated \(\mathrm{Cl}\) atom? (c) What hybrid orbitals should be constructed on the \(S\) atom to make the \(\mathrm{S}-\mathrm{Cl}\) bonds in \(\mathrm{SCl}_{2}\) ? (d) What valence orbitals, if any, remain unhybridized on the \(\mathrm{S}\) atom in \(\mathrm{SCl}_{2}\) ?

Vinyl chloride, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}\), is a gas that is used to form the important polymer called polyvinyl chloride (PVC). Its Lewis structure is (a) What is the total number of valence electrons in the vinyl chloride molecule? (b) How many valence electrons are used to make \(\sigma\) bonds in the molecule? (c) How many valence electrons are used to make \(\pi\) bonds in the molecule? (d) How many valence electrons remain in nonbonding pairs in the molecule? (e) What is the hybridization at each carbon atom in the molecule?

There are two compounds of the formula \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}:\) The compound on the right is called cisplatin, and the compound on the left is called transplatin. (a) Which compound has a nonzero dipole moment? (b) One of these compounds is an anticancer drug, and one is inactive. The anticancer drug works by its chloride ions undergoing a substitution reaction with nitrogen atoms in DNA that are close together, forming a \(\mathrm{N}-\mathrm{Pt}-\mathrm{N}\) angle of about \(90^{*} .\) Which compound would you predict to be the anticancer drug?

Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle.

(a) An \(\mathrm{AB}_{2}\), molecule is linear. How many nonbonding electron pairs are around the A atom from this information? (b) How many nonbonding electrons surround the Xe in \(\mathrm{XeF}_{2} ?(\mathbf{c})\) Is \(\mathrm{XeF}_{2}\) linear?
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