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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3:20 minutes

Problem 3a

Textbook Question

Rank the following elements from least electronegative to most electronegative.
Na, Si, F, Mg, C, O, N

Verified step by step guidance

Understand the concept of electronegativity: Electronegativity is the ability of an atom to attract electrons in a chemical bond. It generally increases across a period (left to right) in the periodic table and decreases down a group (top to bottom).

Locate the elements on the periodic table: Identify the positions of Na, Si, F, Mg, C, O, and N in the periodic table. Note their group and period numbers.

Compare trends across periods: Within the same period, electronegativity increases as you move from left to right. For example, Na (Group 1) will have lower electronegativity than Si (Group 14), and Si will have lower electronegativity than F (Group 17).

Compare trends within groups: Electronegativity decreases as you move down a group. For example, Mg (Group 2, Period 3) will have lower electronegativity than elements like C, N, O, and F, which are in higher periods.

Rank the elements: Based on their positions in the periodic table and the trends in electronegativity, arrange the elements from least electronegative to most electronegative. Use the general rule that metals (e.g., Na, Mg) are less electronegative than nonmetals (e.g., C, N, O, F).

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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 factor in determining the nature of bonds between atoms, influencing whether they will form ionic or covalent bonds. The Pauling scale is commonly used to quantify electronegativity, with higher values indicating greater ability to attract electrons.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements across the periodic table. Electronegativity generally increases from left to right across a period and decreases from top to bottom within a group. Understanding these trends helps in predicting the behavior of elements in chemical reactions and their bonding characteristics.

Comparison of Elements

When ranking elements by electronegativity, it is essential to compare their positions in the periodic table. For example, fluorine (F) is the most electronegative element, while sodium (Na) and magnesium (Mg) are less electronegative due to their positions in groups 1 and 2. This comparison allows for a systematic ranking of the elements based on their electronegativity values.

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Related Practice

Textbook Question

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

(a)

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

(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

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

(b) C vs. O

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Rank the following elements from least electronegative to most electronegative. Na, Si, F, Mg, C, O, N

Key Concepts

Electronegativity

Periodic Trends

Comparison of Elements

Watch next

Rank the following elements from least electronegative to most electronegative.
Na, Si, F, Mg, C, O, N