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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5:30 minutes

Problem 22

Textbook Question

Why are Na⁺ and K⁺ unable to form covalent bonds?

Verified step by step guidance

Understand the nature of Na+ and K+: Sodium (Na) and Potassium (K) are alkali metals located in Group 1 of the periodic table. When they lose one electron, they form Na+ and K+ cations, respectively, achieving a stable noble gas electron configuration.

Recognize the electronic configuration of Na+ and K+: Na+ has the electron configuration of [Ne], and K+ has the electron configuration of [Ar]. Both ions have a full outer shell, making them highly stable and unlikely to share electrons.

Recall the definition of covalent bonds: Covalent bonds are formed when two atoms share electrons to achieve a stable electron configuration. This typically occurs between nonmetals with similar electronegativities.

Analyze the properties of Na+ and K+: Since Na+ and K+ are positively charged ions, they lack valence electrons to share with other atoms. This absence of valence electrons makes it impossible for them to participate in covalent bonding.

Conclude why Na+ and K+ cannot form covalent bonds: The inability of Na+ and K+ to share electrons, combined with their stable noble gas configurations, means they are restricted to forming ionic bonds rather than covalent bonds.

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Key Concepts

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

Ionic vs. Covalent Bonds

Ionic bonds form between atoms with significantly different electronegativities, where one atom donates an electron to another, resulting in charged ions. In contrast, covalent bonds involve the sharing of electrons between atoms with similar electronegativities. Understanding this distinction is crucial for explaining why certain elements, like Na+ and K+, do not form covalent bonds.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons. Sodium (Na) and potassium (K) have low electronegativities, which means they tend to lose electrons rather than share them. This property makes them more likely to form ionic bonds with electronegative elements rather than covalent bonds with other metals or nonmetals.

Ion Formation

Na+ and K+ are cations formed when sodium and potassium atoms lose one electron, respectively. This loss results in a stable electron configuration similar to noble gases. Since these ions are already stable in their ionic form, they do not seek to share electrons through covalent bonding, which is typically a characteristic of neutral atoms.

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Related Practice

Textbook Question

The N—F bond is more polar than the N—H bond, but NF₃ has a smaller dipole moment than NH₃. Explain this curious result.

NF₃

μ= 0.2 D

NH₃

μ = 1.5 D

Textbook Question

For each of the following compounds,

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.

Textbook Question

For each of the following compounds,

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.

Textbook Question

The electrostatic potential maps for ammonia and water are shown here. The structure of ammonia is shown within its EPM. Note how the lone pair creates a region of high electron potential (red), and the hydrogens are in regions of low electron potential (blue). Show how your three-dimensional structure of water corresponds with its EPM.

Textbook Question

Show the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species.

(b) Mg and Br

Textbook Question

Give the charge most likely to result from ionization of the following metals.

(b) Aluminum

Textbook Question

Without looking at Figure 2.20, use your intuition to estimate whether a bond is ionic, polar covalent, or covalent.

(a) Na―Cl

Textbook Question

Show the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species.

(a) Al and F