Textbook Question
One of the molecular orbitals of the H2− ion can be sketched as follows:
a. Is the molecular orbital a 𝜎 or 𝜋 MO? Is it bonding or antibonding?
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Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 107c
Azo dyes are organic dyes that are used for many applications, such as the coloring of fabrics. Many azo dyes are derivatives of the organic substance azobenzene, C12H10N2. A closely related substance is hydrazobenzene, C12H12N2. The Lewis structures of these two substances are
(Recall the shorthand notation used for benzene.) (c) Predict the N¬N¬C angles in each of the substances.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They help visualize the arrangement of electrons and the connectivity of atoms, which is crucial for predicting molecular geometry and reactivity. Understanding how to draw and interpret Lewis structures is essential for analyzing the properties of organic compounds like azo dyes and their derivatives.
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Lewis Dot Structures: Ions
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences bond angles and overall shape. For azo dyes and related compounds, knowing the molecular geometry helps predict the N-N-C angles and the physical properties of the substances.
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01:33Molecular Geometry with Two Electron Groups
Bond Angles
Bond angles are the angles formed between two adjacent bonds at an atom. They are influenced by the hybridization of the atom and the presence of lone pairs, which can repel bonding pairs and alter angles. In the context of azo dyes and hydrazobenzene, predicting the N-N-C bond angles requires an understanding of the molecular geometry and the steric effects of the surrounding atoms.
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Related Practice
Textbook Question
One of the molecular orbitals of the H2− ion can be sketched as follows:
d. Compared to the H—H bond in H2, the H—H bond in H2− is expected to be which of the following?
i. shorter and stronger
ii. longer and stronger
iii. shorter and weaker
iv. longer and weaker or
v. the same length and strength
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Textbook Question
Place the following molecules and ions in order from smallest to largest bond order: H2+,B2,N2+,F2+, and Ne2.
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Textbook Question
Carbon monoxide, CO, is isoelectronic to N2. (d) Would you expect the p2p MOs of CO to have equal atomic orbital contributions from the C and O atoms? If not, which atom would have the greater contribution?
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Textbook Question
The energy-level diagram in Figure 9.40 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the to the molecular orbital. a. Assuming this electronic transition corresponds to the HOMO–LUMO transition, what is the HOMO in ethylene?
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Textbook Question
The energy-level diagram in Figure 9.40 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the to the molecular orbital. b. Assuming this electronic transition corresponds to the HOMO–LUMO transition, what is the LUMO in ethylene?
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