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

Electronegativity

Organic Chemistry

1. A Review of General Chemistry

Electronegativity

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1:35 minutes

Problem 34

Textbook Question

According to the potential map for the ammonium ion <IMAGE>, which atom has the greatest electron density?

Verified step by step guidance

Examine the potential map provided for the ammonium ion (NH₄⁺). The map uses color coding to represent electron density, where blue typically indicates regions of high electron density and red indicates regions of low electron density.

Identify the atoms in the ammonium ion structure. The central atom is nitrogen (N), and it is surrounded by four hydrogen (H) atoms.

Observe the color distribution around the atoms. In the image, the nitrogen atom is surrounded by blue, indicating higher electron density, while the hydrogen atoms are surrounded by red or orange, indicating lower electron density.

Recall that nitrogen is more electronegative than hydrogen, meaning it attracts electrons more strongly. This aligns with the observation that nitrogen has the greatest electron density in the ammonium ion.

Conclude that the atom with the greatest electron density in the ammonium ion is the nitrogen atom, based on the potential map and the electronegativity of nitrogen compared to hydrogen.

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Key Concepts

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

Electron Density

Electron density refers to the probability of finding electrons in a particular region around an atom or molecule. It is often visualized using electron density maps, which represent areas of high and low electron concentration. In the context of the ammonium ion, understanding electron density helps identify which atom has the greatest electron presence, influencing its reactivity and bonding characteristics.

Ammonium Ion Structure

The ammonium ion (NH4+) consists of a nitrogen atom bonded to four hydrogen atoms, forming a tetrahedral geometry. This structure is crucial for understanding the distribution of electron density within the ion. The nitrogen atom, being more electronegative than hydrogen, attracts electron density towards itself, which can be visualized in the potential map provided.

Potential Maps

Potential maps are graphical representations that illustrate the distribution of electron density around a molecule. They use color gradients to indicate areas of high and low electron density, helping to visualize molecular properties. In the case of the ammonium ion, the potential map allows us to determine which atom has the highest electron density, providing insights into its chemical behavior.

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Related Practice

Textbook Question

Rank the bonds from most polar to least polar.

d. C—H, C—C, C—N

Textbook Question

Rank the bonds from most polar to least polar.

c. H—O, H—N, H—C

Textbook Question

Rank the bonds from most polar to least polar.

b. C—Cl, C—I, C—Br

Textbook Question

Which of the following molecules would you expect to have a dipole moment of zero?

d. NH₃

e. H₂C═CH₂

f. H₂C═CHBr

Textbook Question

Two isomers of 1,2-dichloroethene are known. One has a dipole moment of 2.4 D; the other has zero dipole moment. Draw the two isomers, and explain why one has zero dipole moment.

CHCl=CHCl 1,2-dichloroethene

Textbook Question

1. Draw the Lewis structure.

2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

3. Estimate whether the compound will have a large, small, or zero dipole moment.

g. HCN

h. CH₃CHO

i. H₂C=NH

Textbook Question

1. Draw the Lewis structure.

2. Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.

3. Estimate whether the compound will have a large, small, or zero dipole moment.

d. CH₃F

e. CF₄

f. CH₃OH

Textbook Question

Sulfur dioxide has a dipole moment of 1.60 D. Carbon dioxide has a dipole moment of zero, even though C―O bonds are more polar than S―O bonds. Explain this apparent contradiction.

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