Textbook Question
Draw three Lewis structures for C3H8O.
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Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)
Bruice8th EditionOrganic ChemistryISBN: 9780135213711
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Table of contents
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 1)31
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)65
- Ch. 2 - Acids and Bases: Central to Understanding Organic Chemistry84
- Ch. 3 - An Introduction to Organic Compounds:Nomenclature, Physical Properties, and Structure183
- Ch. 4 - Isomers: The Arrangement of Atoms in Space121
- Ch. 5 - Alkenes: Structure, Nomenclature, and an Introduction to Reactivity • Thermodynamics and Kinetics83
- Ch. 6 - The Reactions of Alkenes • The Stereochemistry of Addition Reactions175
- Ch. 7 - The Reactions of Alkynes • An Introduction to Multistep Synthesis119
- Ch. 8 - Delocalized Electrons: Their Effect on Stability, pKa, and the Products of a Reaction • Aromaticity and Electronic Effects: An Introduction to the Reactions of Benzene148
- Ch. 9 - Substitution and Elimination Reactions of Alkyl Halides212
- Ch. 10 - Reactions of Alcohols, Ethers, Epoxides, Amines, and Sulfur-Containing Compounds131
- Ch. 11 - Organometallic Compounds60
- Ch. 12 - Radicals90
- Ch. 13 - Mass Spectrometry; Infrared Spectroscopy; UV/Vis Spectroscopy62
- Ch. 14 - NMR Spectroscopy95
- Ch. 15 - Reactions of Carboxylic Acids and Carboxylic Acid Derivatives123
- Ch. 16 - Reactions of Aldehydes and Ketones • More Reactions of Carboxylic Acid Derivatives141
- Ch. 17 - Reactions at the Alpha-Carbon101
- Ch. 18 - Reactions of Benzene and Substituted Benzenes144
- Ch. 19 - More About Amines • Reactions of Heterocyclic Compounds49
- Ch. 20 - The Organic Chemistry of Carbohydrates80
- Ch. 21 - Amino Acids, Peptides, and Proteins57
- Ch. 22 - Catalysis in Organic Reactions and in Enzymatic Reactions35
- Ch. 23 - The Organic Chemistry of the Coenzymes—Compounds Derived from Vitamins1
- Ch. 28 - Pericyclic Reactions58
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Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)Problem 17f
Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)Problem 17fChapter 2, Problem 17f
Draw the Lewis structure for each of the following:
f. NaOH
Verified step by step guidance1
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.
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Drawing the Lewis Structure for N2H4.
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.
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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
Use the symbols δ+ and δ− to show the direction of the polarity of the indicated bond in each of the following compounds:
g. I—Cl
h. H2N—OH
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Textbook Question
Draw the lone-pair electrons that are not shown in the following condensed structures:
a. CH3CH2NH2
b. CH3NHCH3
c. CH3CH2OH
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Textbook Question
Draw two Lewis structures for C2H6O.
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Textbook Question
After examining the potential maps for LiH, HF, and H2, answer the following questions:
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a. Which compounds are polar?
b. Why does LiH have the largest hydrogen?
c. Which compound has the hydrogen that would be most apt to attract a negatively charged molecule?
Textbook Question
Explain why HCl has a smaller dipole moment than HF, even though the H—Cl bond is longer than the H—F bond.
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