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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 7a
Capitolo 9, Problema 7a

In the hydrocarbon
Structural formula of a hydrocarbon with numbered carbon atoms for hybridization analysis.
(a) What is the hybridization at each carbon atom in the molecule?

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Identify the number of regions of electron density (bonds and lone pairs) around each carbon atom.
Determine the hybridization based on the number of regions of electron density: 2 regions = sp, 3 regions = sp2, 4 regions = sp3.
For Carbon 1: It has 3 regions of electron density (1 double bond and 2 single bonds), so it is sp2 hybridized.
For Carbon 2: It has 3 regions of electron density (1 double bond and 2 single bonds), so it is sp2 hybridized.
For Carbon 3: It has 4 regions of electron density (4 single bonds), so it is sp3 hybridized.

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Hybridization

Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are used to form covalent bonds in molecules. The type of hybridization (sp, sp2, sp3, etc.) depends on the number of bonds and lone pairs around the central atom, influencing the geometry and bond angles of the molecule.
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Hybridization

Carbon Atom Hybridization

In organic chemistry, carbon atoms can undergo different types of hybridization based on their bonding. For example, sp hybridization occurs when a carbon atom forms two double bonds or one triple bond, resulting in a linear geometry. In contrast, sp2 hybridization is seen in carbon atoms with one double bond and two single bonds, leading to a trigonal planar shape, while sp3 hybridization involves four single bonds, resulting in a tetrahedral geometry.
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Hybridization

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the hybridization of the central atom and the presence of lone pairs. Understanding molecular geometry is crucial for predicting the shape and reactivity of molecules, as it influences properties such as polarity, phase of matter, and biological activity.
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Molecular Geometry with Two Electron Groups
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In the hydrocarbon

(d) Identify all the 120° bond angles in the molecule.

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In the hydrocarbon (b) How many s bonds are there 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 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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