**Educational Content: Molecule Hybridization and Bond Angles**In the displayed molecule, identify the hybridization and approximate bond angle of the labeled atoms:- **a (Oxygen atom)**: Typically, oxygen in this context will exhibit sp³ hybridization, characterized by a bond angle close to 109.5°, due to its two lone pairs.- **b (Carbon atom connected to oxygen and sulfur)**: Demonstrates sp³ hybridization, with a geometrical bond angle around 109.5°, owing to its tetrahedral arrangement.- **c (Carbon atom double-bonded to another carbon)**: This carbon will be sp² hybridized, typical of alkenes, with an approximate bond angle of 120° due to its planar trigonal configuration.- **d (Carbon atom with a lone pair)**: The presence of the lone pair indicates sp hybridization, associated with a linear geometry and a bond angle of approximately 180°.- **e (Phosphorus atom connected to sulfur)**: This phosphorus is likely sp³ hybridized, suggesting a bond angle of about 109.5°, consistent with its tetrahedral shape.- **f (Sulfur atom connected to phosphorus)**: With a similar sp³ hybridization, the sulfur exhibits a bond angle near 109.5°, being part of a different tetrahedral structure.These hybridizations and bond angles are fundamental in predicting molecular geometry and behavior in various chemical environments.

Answered: Determine the hybridization and the…

Determine the hybridization and the approximate bond angle of the labeled atom in the following molecule b a H d f е н SA :O:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

**Educational Content: Molecule Hybridization and Bond Angles**

In the displayed molecule, identify the hybridization and approximate bond angle of the labeled atoms:

- **a (Oxygen atom)**: Typically, oxygen in this context will exhibit sp³ hybridization, characterized by a bond angle close to 109.5°, due to its two lone pairs.

- **b (Carbon atom connected to oxygen and sulfur)**: Demonstrates sp³ hybridization, with a geometrical bond angle around 109.5°, owing to its tetrahedral arrangement.

- **c (Carbon atom double-bonded to another carbon)**: This carbon will be sp² hybridized, typical of alkenes, with an approximate bond angle of 120° due to its planar trigonal configuration.

- **d (Carbon atom with a lone pair)**: The presence of the lone pair indicates sp hybridization, associated with a linear geometry and a bond angle of approximately 180°.

- **e (Phosphorus atom connected to sulfur)**: This phosphorus is likely sp³ hybridized, suggesting a bond angle of about 109.5°, consistent with its tetrahedral shape.

- **f (Sulfur atom connected to phosphorus)**: With a similar sp³ hybridization, the sulfur exhibits a bond angle near 109.5°, being part of a different tetrahedral structure.

These hybridizations and bond angles are fundamental in predicting molecular geometry and behavior in various chemical environments.

Expert Solution

Step 1

Hybridization = Bond pair + Lone pair

By using this formula , we can calculate the hybridization of each atom.

For 2 , hybridization is 'sp' , Bond angle is 180

For 3 , hybridization is 'sp²' , Bond angle is 120

For 4, hybridization is 'sp³', Bond angle is 109.5

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