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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Problem 23

Textbook Question

Based on your answer to Assessment 2.22, would you expect a larger atom to be more or less electronegative than a smaller atom?

Verified step by step guidance

Understand the concept of electronegativity: Electronegativity is the ability of an atom to attract electrons towards itself in a chemical bond.

Consider the size of the atom: Larger atoms have their valence electrons farther from the nucleus, which means the nucleus has less pull on the electrons.

Compare with smaller atoms: Smaller atoms have their valence electrons closer to the nucleus, resulting in a stronger attraction between the nucleus and the electrons.

Relate size to electronegativity: Generally, as atomic size increases, electronegativity decreases because the increased distance reduces the nucleus's ability to attract electrons.

Conclude the relationship: Therefore, a larger atom is typically less electronegative than a smaller atom.

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Key Concepts

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

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It is influenced by the atom's atomic number and the distance of the valence electrons from the nucleus. Generally, higher electronegativity indicates a stronger pull on electrons, which is crucial for understanding bonding behavior in molecules.

Atomic Size

Atomic size refers to the physical size of an atom, typically measured by the atomic radius. As you move down a group in the periodic table, atomic size increases due to the addition of electron shells. Larger atoms have their valence electrons further from the nucleus, which can affect their electronegativity and ability to attract electrons.

Trends in the Periodic Table

Trends in the periodic table, such as electronegativity and atomic size, help predict the behavior of elements. Generally, electronegativity increases across a period (left to right) and decreases down a group (top to bottom). Understanding these trends is essential for predicting how different atoms will interact in chemical reactions.

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Related Practice

Textbook Question

Refer to the electrostatic potential maps <IMAGE> to answer the following questions:

c. Why is the center of the electrostatic potential map of benzene more red than the center of the electrostatic potential map of pyridine?

Textbook Question

Which is more reactive, an organolithium compound or an organosodium compound? Explain your answer.

Textbook Question

(a) Rank the following bonds in terms of the strength of their bond dipole (1 = weakest, 6 = strongest).

(b) Which carbon has the largest δ⁺ ?

C―F, C―Br, C―I, C―H, C―C, C―Cl

Textbook Question

A mixture of seven amino acids (glycine, glutamate, leucine, lysine, alanine, isoleucine, and aspartate) is separated by chromatography. Explain why only six spots show up when the chromatographic plate is coated with ninhydrin and heated.

Textbook Question

Given the Lewis structures, indicate the direction of the dipole moment, if there is one.

(e)

Textbook Question

Use the symbols δ⁺ and δ⁻ to show the direction of the polarity of the indicated bond in each of the following compounds:

e. HO—Br

f. H₃C—Li

Textbook Question

After examining the potential maps for LiH, HF, and H₂, answer the following questions:

<IMAGE>

a. Which compounds are polar?

b. Why does LiH have the largest hydrogen?

c. Which compound has the hydrogen that would be most apt to attract a negatively charged molecule?

Textbook Question

Rank the following compounds from highest dipole moment to lowest dipole moment:

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