Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Molecular Geometry

Organic Chemistry

1. A Review of General Chemistry

Molecular Geometry

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6:41 minutes

Problem 32(3)

Textbook Question

For each of the given species:
a. Draw its Lewis structure.
b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.
3. CCl₄

Verified step by step guidance

Step 1: Draw the Lewis structure for CCl₄. Start by identifying the total number of valence electrons. Carbon (C) has 4 valence electrons, and each chlorine (Cl) atom has 7 valence electrons. Since there are 4 chlorine atoms, the total number of valence electrons is 4 + (7 × 4) = 32.

Step 2: Place the carbon atom in the center as it is less electronegative than chlorine. Surround the carbon atom with four chlorine atoms. Form single bonds between the carbon and each chlorine atom. Each single bond consists of 2 electrons, so 8 electrons are used for bonding.

Step 3: Distribute the remaining electrons (32 - 8 = 24) as lone pairs around the chlorine atoms to satisfy the octet rule. Each chlorine atom will have 6 electrons as lone pairs, in addition to the 2 electrons in the C-Cl bond, completing their octets.

Step 4: Describe the orbitals used by the carbon atom in bonding. Carbon in CCl₄ undergoes sp³ hybridization. This means that one s orbital and three p orbitals mix to form four equivalent sp³ hybrid orbitals. Each of these orbitals overlaps with a p orbital of a chlorine atom to form a sigma bond.

Step 5: Indicate the approximate bond angles. Since the carbon atom is sp³ hybridized, the geometry of CCl₄ is tetrahedral, and the bond angles are approximately 109.5°.

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Key Concepts

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

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of CCl4, the carbon atom undergoes sp3 hybridization, resulting in four equivalent sp3 hybrid orbitals that form sigma bonds with chlorine atoms. This concept is crucial for understanding the geometry and bond angles in molecules.

Molecular Geometry and Bond Angles

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule, which is influenced by the repulsion between electron pairs. In CCl4, the tetrahedral geometry leads to bond angles of approximately 109.5 degrees. Recognizing the relationship between hybridization, molecular shape, and bond angles is vital for predicting the physical and chemical properties of compounds.

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Related Practice

Textbook Question

Predict the approximate bond angles for

c. the H—C—N bond angle in (CH₃)₂NH.

d. the H—C—O bond angle in CH₃OCH₃

Textbook Question

Predict the approximate bond angles:

c. the C—N—H bond angle in (CH₃)₂NH

d. the C—N—C bond angle in (CH₃)₂NH

Textbook Question

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

Textbook Question

For each of the following compounds and ions,

1. Draw a Lewis structure.

2. Show the kinds of orbitals that overlap to form each bond.

3. Give approximate bond angles around each atom except hydrogen.

a. [NH₂]^–

Textbook Question

Predict the hybridization of the oxygen atom in water, H₂O. Draw a picture of its three-dimensional structure, and explain why its bond angle is 104.5°.

Multiple Choice

Determine the hybridizationof the following selected atoms:

Multiple Choice

PRACTICE:Determine the hybridization and molecular geometry of the following selected atoms:

Multiple Choice

Which atom in the following structure has trigonal planar geometry?

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