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

Bonding Preferences

Organic Chemistry

1. A Review of General Chemistry

Bonding Preferences

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3:26 minutes

Problem 19

Textbook Question

Fill in the blank. Oxygen ionizes to become ― 2 instead of ― 1 because O^2- is more ___________ .

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Understand the context: Oxygen typically forms ions by gaining electrons to achieve a stable electronic configuration, similar to the nearest noble gas (Neon). This is due to its high electronegativity and tendency to complete its octet.

Recall the electronic configuration of oxygen: The neutral oxygen atom has an atomic number of 8, meaning its electronic configuration is 1s² 2s² 2p⁴. It needs 2 more electrons to fill its 2p orbital and achieve a stable octet.

Analyze the charge states: When oxygen gains 1 electron, it forms O⁻ (with a -1 charge). However, this state is less stable because the octet is not yet complete. When oxygen gains 2 electrons, it forms O²⁻ (with a -2 charge), achieving a full octet and a more stable configuration.

Consider the concept of stability: The O²⁻ ion is more stable than O⁻ because it has a complete octet, which minimizes the energy of the system. Atoms and ions tend to adopt configurations that lower their energy and increase stability.

Fill in the blank: The blank should be filled with the word 'stable,' as O²⁻ is more stable than O⁻ due to its complete octet and lower energy state.

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Key Concepts

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

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion. For oxygen, the first ionization energy is relatively high due to its electronegativity and the stability of its electron configuration. However, the second ionization energy is even higher, which explains why oxygen typically forms a -2 charge (O²⁻) rather than a -1 charge (O⁻).

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons. Oxygen is highly electronegative, which means it has a strong tendency to gain electrons to achieve a stable octet configuration. This property contributes to its preference for forming a -2 charge, as it can effectively stabilize the additional electrons.

Stability of Electron Configuration

The stability of an electron configuration refers to how energetically favorable a particular arrangement of electrons is. For oxygen, achieving a full outer shell with eight electrons (octet) by gaining two electrons leads to the formation of the O²⁻ ion, which is more stable than having only one additional electron. This stability drives the ionization process and the resulting charge.

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