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

Lewis Structure

Organic Chemistry

1. A Review of General Chemistry

Lewis Structure

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3:27 minutes

Problem 17f

Textbook Question

Draw the Lewis structure for each of the following:
f. NaOH

Verified step by step guidance

Step 1: Identify the elements in the compound NaOH. Sodium (Na) is a metal, oxygen (O) is a nonmetal, and hydrogen (H) is also a nonmetal. This compound is ionic in nature, with Na+ as the cation and OH⁻ as the anion.

Step 2: Begin by drawing the Lewis structure for the hydroxide ion (OH⁻). Oxygen has six valence electrons, and hydrogen has one valence electron. Since OH⁻ has a negative charge, add one extra electron to the oxygen atom, making a total of seven valence electrons for oxygen.

Step 3: Place the hydrogen atom bonded to the oxygen atom via a single covalent bond. Represent the bond as a line between the oxygen and hydrogen atoms. Distribute the remaining electrons around the oxygen atom to satisfy the octet rule. Oxygen will have three lone pairs of electrons.

Step 4: Represent the sodium ion (Na⁺) separately. Sodium loses one electron to form a positive charge, so it does not have any valence electrons in its Lewis structure. Write Na⁺ next to the hydroxide ion to indicate the ionic bond between Na⁺ and OH⁻.

Step 5: Combine the structures to show the complete Lewis structure of NaOH. The sodium ion (Na⁺) is adjacent to the hydroxide ion (OH⁻), with the ionic bond implied by their charges. Ensure the negative charge on OH⁻ and the positive charge on Na⁺ are clearly indicated.

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Key Concepts

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

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of charged ions. In the case of NaOH, sodium (Na) donates an electron to become Na+, while hydroxide (OH-) is formed from oxygen and hydrogen. Recognizing the ionic nature of compounds helps in understanding their properties and behavior in chemical reactions.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how an atom bonds with others. The number of valence electrons influences the atom's reactivity and the type of bonds it can form. For NaOH, knowing the valence electrons of sodium, oxygen, and hydrogen is key to accurately drawing its Lewis structure.

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Related Practice

Textbook Question

Draw Lewis structures for the following compounds and ions, showing appropriate formal charges.

(i) (CH₃)₂O—BF₃

(j) [HONH₃]⁺

(k) KOC(CH₃)₃

(l) [H₂C=OH]⁺

Textbook Question

Draw Lewis structures for the following compounds and ions, showing appropriate formal charges.

(e) ⁺CH₃

(f) ^–CH₃

(g) NaBH₄

(h) NaBH₃CN

Textbook Question

Write Lewis structures for the following molecular formulas. Circle any lone pairs (pairs of nonbonding electrons) in the structures.

i. C₃H₆ (one double bond)

j. C₃H₄ (two double bonds)

k. C₃H₄ (one triple bond)

Textbook Question

Dimethyl sulfoxide (DMSO) has been used as an anti-inflammatory rub for race horses. DMSO and acetone appear to have similar structures, but the C=O carbon atom in acetone is planar, while the S=O sulfur atom in DMSO is pyramidal. Draw Lewis structures for DMSO and acetone, predict the hybridizations, and explain these observations.

Textbook Question

Draw two Lewis structures for C₂H₆O.

Textbook Question

Draw three Lewis structures for C₃H₈O.

Textbook Question

For each of the given species:

a. Draw its Lewis structure.

b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.

1. H₂CO₂

Textbook Question

For each of the given species:

a. Draw its Lewis structure.