Textbook Question
Draw a Lewis structure for each of the following:
d. NH2O−
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 57c
Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)Problem 57cChapter 2, Problem 57c
Rank the bonds from most polar to least polar.
c. H—O, H—N, H—C
Verified step by step guidance1
Determine the concept of bond polarity: Bond polarity arises due to the difference in electronegativity between the two atoms in a bond. The greater the difference in electronegativity, the more polar the bond.
Identify the electronegativity values of the atoms involved: Use the Pauling scale to find the electronegativity values. For reference: H = 2.1, O = 3.5, N = 3.0, C = 2.5.
Calculate the electronegativity differences for each bond: Subtract the electronegativity of hydrogen (H) from the electronegativity of the other atom in the bond. For example, for H—O, the difference is |3.5 - 2.1|.
Compare the electronegativity differences: Rank the bonds based on the magnitude of the electronegativity differences. A larger difference indicates a more polar bond.
List the bonds in order from most polar to least polar based on the calculated differences: This will provide the ranking of H—O, H—N, and H—C in terms of bond polarity.
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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. The greater the difference in electronegativity between two bonded atoms, the more polar the bond becomes. For example, oxygen is more electronegative than hydrogen, leading to a polar bond in H—O.
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Electronegativity
Polarity of Bonds
The polarity of a bond is determined by the distribution of electrical charge across the bond. A polar bond occurs when there is a significant difference in electronegativity between the two atoms, resulting in a dipole moment. In the context of the question, H—O is the most polar due to the high electronegativity of oxygen compared to hydrogen.
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Comparison of Bond Polarities
To rank bond polarities, one must compare the electronegativity values of the atoms involved. In the given bonds, H—O is the most polar, followed by H—N, and then H—C, as carbon has a lower electronegativity than nitrogen and oxygen. This ranking reflects the increasing ability of the atoms to attract shared electrons.
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Related Practice
Textbook Question
Rank the bonds from most polar to least polar.
b. C—Cl, C—I, C—Br
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Textbook Question
Draw a Lewis structure for each of the following:
b. CH3OCH3
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Rank the bonds from most polar to least polar.
d. C—H, C—C, C—N
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Draw a Lewis structure for each of the following:
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Textbook Question
Draw a skeletal structure for each of the compounds.
a. CH3CHO
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