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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2:32 minutes

Problem 6b

Textbook Question

In each pair of atoms, which has the larger atomic radius? Which is more electronegative?
(b) C vs. O

Verified step by step guidance

Step 1: Understand the periodic trends for atomic radius and electronegativity. Atomic radius generally decreases across a period (left to right) in the periodic table, while electronegativity increases across a period.

Step 2: Locate the elements Carbon (C) and Oxygen (O) on the periodic table. Both are in the same period (Period 2), with Carbon in Group 14 and Oxygen in Group 16.

Step 3: Compare atomic radii. Since atomic radius decreases across a period, Carbon (C), being to the left of Oxygen (O), will have a larger atomic radius.

Step 4: Compare electronegativity. Electronegativity increases across a period, so Oxygen (O), being to the right of Carbon (C), will be more electronegative.

Step 5: Summarize the findings. Carbon has the larger atomic radius, while Oxygen is more electronegative. These trends are consistent with periodic table properties.

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Key Concepts

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

Atomic Radius

Atomic radius refers to the size of an atom, typically measured from the nucleus to the outermost electron shell. Generally, atomic radius increases down a group in the periodic table due to the addition of electron shells, while it decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It generally increases across a period from left to right and decreases down a group. This trend is important for predicting how atoms will interact in chemical reactions, particularly in determining bond polarity.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Key trends include atomic radius, electronegativity, ionization energy, and electron affinity. Understanding these trends helps in comparing elements and predicting their chemical behavior.

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Related Practice

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?

(b) N vs. O

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

Which bond is stronger? Briefly explain why.

Textbook Question

Which bond is stronger? Briefly explain why.

Textbook Question

For each pair of compounds, predict which one has the higher molecular dipole moment, and explain your reasoning.

a. ethyl chloride or ethyl iodide

b. 1-bromopropane or cyclopropane

Textbook Question

For each alkene, indicate the direction of the dipole moment. For each pair, determine which compound has the larger dipole moment.

a. cis-1,2-difluoroethene or trans-1,2-difluoroethene

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In each pair of atoms, which has the larger atomic radius? Which is more electronegative? (b) C vs. O

Key Concepts

Atomic Radius

Electronegativity

Periodic Trends

Watch next

In each pair of atoms, which has the larger atomic radius? Which is more electronegative?
(b) C vs. O