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Ch.1 - Structure and Bonding
Wade - Organic Chemistry 9th Edition
Wade9th EditionOrganic ChemistryISBN: 9780135213728Not the one you use?Change textbook
All textbooksWade 9th EditionCh.1 - Structure and BondingProblem 1
Chapter 1, Problem 1

For each of the following compounds,1. Give the hybridization and approximate bond angles around each atom except hydrogen.2. Draw a three-dimensional diagram, including any lone pairs of electrons.d. (CH3)3N e. [CH3NH3]+f. CH3COOH

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1
Identify the central atoms in each compound and determine the number of electron groups (bonds and lone pairs) around them.
For each central atom, use the VSEPR theory to determine the hybridization based on the number of electron groups: sp (2 groups), sp2 (3 groups), sp3 (4 groups), etc.
Estimate the bond angles based on the hybridization: sp (180°), sp2 (120°), sp3 (109.5°), and adjust for lone pairs if necessary.
Draw a three-dimensional structure for each compound, showing the arrangement of atoms and lone pairs around the central atoms.
Label the hybridization and bond angles on the diagram for each central atom, ensuring to include any lone pairs in the depiction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of a molecule. For example, in (CH3)3N, the nitrogen atom undergoes sp3 hybridization, resulting in four equivalent hybrid orbitals that form sigma bonds with three methyl groups and one lone pair.
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Bond Angles

Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the hybridization of the central atom and the presence of lone pairs. In (CH3)3N, the bond angles are approximately 109.5 degrees due to its tetrahedral geometry, while in [CH3NH3]+, the angles are also close to this value, reflecting its sp3 hybridization.
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Three-Dimensional Molecular Geometry

Three-dimensional molecular geometry describes the spatial arrangement of atoms in a molecule, which can be represented using models that show bond angles and lone pairs. For instance, in CH3COOH, the carboxylic acid group has a planar arrangement around the carbon atom, while the overall structure can be depicted using wedge-and-dash notation to indicate the three-dimensional orientation of bonds.
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Related Practice
Textbook Question

Nitrogen has relatively stable isotopes (half-life greater than 1 second) of mass ­numbers 13, 14, 15, 16, and 17. All except 14N and 15N are radioactive.) Calculate how many protons and neutrons are in each of these isotopes of nitrogen.

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Textbook Question

Use your molecular models to make ethane, and compare the model with the preceding structures.

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Textbook Question

Draw Lewis structures for the following compounds.

e. dimethylamine, CH3NHCH3

f. diethyl ether, CH3CH2OCH2CH3

g. 1-chloropropane,CH3CH2CH2Cl

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Textbook Question

Write the electronic configurations of the third-row elements shown in the partial ­periodic table in Figure 1-6.

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