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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblema 7d
Capitolo 9, Problema 7d

Consider the following hydrocarbon:
d. Identify all the 120° bond angles in the molecule.

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1
Identify the type of hydrocarbon given in the problem.
Recognize that 120° bond angles are characteristic of sp2 hybridized carbon atoms.
Determine which carbon atoms in the molecule are sp2 hybridized.
Look for carbon atoms that are part of double bonds or are in a trigonal planar geometry.
List all the bond angles around these sp2 hybridized carbon atoms that are 120°.

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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 the angles between bonds. Understanding molecular geometry is crucial for predicting bond angles, such as the 120° angles typically found in trigonal planar structures.
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Molecular Geometry with Two Electron Groups

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs. According to VSEPR, electron pairs will arrange themselves to minimize repulsion, leading to specific bond angles. In hydrocarbons with trigonal planar geometry, the bond angles are approximately 120° due to the arrangement of three bonding pairs around a central atom.
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Molecular Shapes and VSEPR

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In the case of hydrocarbons with 120° bond angles, sp² hybridization occurs, where one s orbital and two p orbitals combine to form three equivalent sp² hybrid orbitals. This hybridization explains the planar structure and the specific bond angles observed in such molecules.
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Hybridization
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Consider the following hydrocarbon:

a. What is the hybridization at each carbon atom in the molecule?

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The drawing below shows the overlap of two hybrid orbitals to form a bond in a hydrocarbon. (a) Which of the following types of bonds is being formed: (i) C¬C s, (ii) C¬C p, or (iii) C¬H s?

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The drawing below shows the overlap of two hybrid orbitals to form a bond in a hydrocarbon. (b) Which of the following could be the identity of the hydrocarbon: (i) CH4, (ii) C2H6, (iii) C2H4, or (iv) C2H2?

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The orbital diagram that follows presents the final step in the formation of hybrid orbitals by a silicon atom. (b) What type of hybrid orbital is produced in this hybridization?

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Consider the following hydrocarbon:

b. How many 𝜎 bonds are there in the molecule?

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The molecule shown here is called furan. It is represented in the typical shorthand way for organic molecules, with hydrogen atoms not shown, and each of the four vertices representing a carbon atom. e. The bond angles in furan are much smaller than those in benzene. The likely reason is which of the following? i. The hybridization of the carbon atoms in furan is different from that in benzene. ii. Furan does not have another resonance structure equivalent to the one shown here. iii. The atoms are forced to adopt smaller angles in a five-membered ring than in a six-membered ring. [Section 9.5]