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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1:44 minutes

Problem 20b

Textbook Question

(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?
(b) N vs. O

Verified step by step guidance

Step 1: Recall the periodic trend for electronegativity. Electronegativity generally increases across a period (left to right) and decreases down a group in the periodic table.

Step 2: Identify the position of nitrogen (N) and oxygen (O) in the periodic table. Both elements are in the same period (Period 2), but oxygen is to the right of nitrogen.

Step 3: Based on the periodic trend, oxygen is expected to be more electronegative than nitrogen because it is further to the right in the same period.

Step 4: To confirm this, look at the actual Pauling electronegativity values. Nitrogen has a value of approximately 3.0, while oxygen has a value of approximately 3.5. This confirms that oxygen is more electronegative.

Step 5: Explain why oxygen is more electronegative. Oxygen has a higher nuclear charge (more protons in the nucleus) compared to nitrogen, which results in a stronger attraction for electrons in a covalent bond.

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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 a key concept in understanding how atoms interact in molecules. The Pauling scale is commonly used to quantify electronegativity values, with higher values indicating a stronger tendency to attract electrons.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Electronegativity generally increases across a period from left to right and decreases down a group. This trend is crucial for comparing the electronegativity of elements like nitrogen (N) and oxygen (O) in the given question.

Pauling Scale

The Pauling scale is a numerical scale for measuring electronegativity, developed by Linus Pauling. It assigns values to elements based on their ability to attract electrons in a bond, with fluorine being the most electronegative at 4.0. For the pair N vs. O, the actual Pauling values (3.0 for N and 3.5 for O) indicate that oxygen is more electronegative, which is essential for answering the question.

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Related Practice

Textbook Question

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

(b)

Textbook Question

Carbon dioxide (CO₂) has no dipole moment (μ = 0 D). The related molecule sulfur dioxide (SO₂) does have a dipole moment (μ = 1.6 D) Explain this observation.

Textbook Question

Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.]

(a) C―C

(b) C―O

(d) C―F

(e) C―Cl

(f) C―S

Textbook Question

Rank the following elements from least electronegative to most electronegative.

Na, Si, F, Mg, C, O, N

Textbook Question

(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?

(d) B vs. Si

Textbook Question

In each pair of atoms, which has the larger atomic radius? Which is more electronegative?

Textbook Question

In each pair of atoms, which has the larger atomic radius? Which is more electronegative?

(b) C vs. O

Textbook Question

Which bond is stronger? Briefly explain why.

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(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why? (b) N vs. O

Key Concepts

Electronegativity

Periodic Trends

Pauling Scale

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(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?
(b) N vs. O