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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblema 61a
Capitolo 9, Problema 61a

Consider the Lewis structure for acetic acid, which is known as vinegar:
Lewis structure of propyne showing carbon atoms A and B with hydrogen atoms.
(a) What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each of them?

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Identify the hybridization of carbon atom A. Since carbon atom A is involved in a triple bond (one sigma bond and two pi bonds) and one single bond, it is sp-hybridized.
Determine the bond angles around carbon atom A. In sp-hybridization, the bond angles are approximately 180 degrees.
Identify the hybridization of carbon atom B. Carbon atom B is involved in four single bonds, which means it is sp3-hybridized.
Determine the bond angles around carbon atom B. In sp3-hybridization, the bond angles are approximately 109.5 degrees.
Summarize the findings: Carbon atom A has sp hybridization with bond angles of approximately 180 degrees, and carbon atom B has sp3 hybridization with bond angles of approximately 109.5 degrees.

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Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In the case of carbon atoms, sp, sp², and sp³ hybridizations correspond to different types of bonding and geometry. For example, sp hybridization involves the mixing of one s and one p orbital, resulting in two equivalent sp hybrid orbitals, which are oriented linearly at 180°.
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Hybridization

Bond Angles

Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the hybridization of the central atom. For sp hybridized carbon atoms, the bond angles are approximately 180°, while sp² hybridized carbons have bond angles of about 120°, and sp³ hybridized carbons have angles close to 109.5°. Understanding these angles helps predict molecular geometry.
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Bond Angles

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons. They provide a visual representation of how atoms are connected and help in determining the hybridization and bond angles. In acetic acid, the Lewis structure reveals the arrangement of atoms and the types of bonds, which are essential for analyzing the molecular geometry.
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Lewis Dot Structures: Ions
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Consider the Lewis structure for acetic acid, which is known as vinegar: (b) What are the hybridizations of the orbitals on the two oxygen atoms, and what are the approximate bond angles at the oxygen that is connected to carbon and hydrogen? What are the hybridizations of the orbitals on the two oxygen atoms?

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(e) How many valence electrons remain in nonbonding pairs in the molecule?

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Consider the Lewis structure for glycine, the simplest amino acid:


(b) What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom, and what are the approximate bond angles at the nitrogen?

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Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is

(c) How many of the valence electrons are used to make s bonds in the molecule?

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Consider the Lewis structure for glycine, the simplest amino acid:

(c) What is the total number of s bonds in the entire molecule, and what is the total number of p bonds?

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(a) What is the hybridization at each of the carbon atoms of the molecule?

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