Textbook Question
Draw the Lewis structure for the following molecules. Be sure to calculate the formal charge of each atom as a way of confirming your structure is correct.
(b) HOBr
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Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
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Table of contents
- Ch. 2 - General Chemistry Translated: Finding the Electrons114
- Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis109
- Ch. 4 - Acids and Bases: Electron Flow144
- Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics118
- Ch. 6 - Stereoisomerism: Arrangement of Atoms in Space112
- Ch. 7 - Principles of Green (Organic) Chemistry3
- Ch. 8 - Alkenes I: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes II: Oxidation and Reduction150
- Ch. 10 - Alkynes: Electrophilic Addition and Redox Reactions101
- Ch. 11 - Properties and Synthesis of Alkyl Halides: Radical Reactions108
- Ch. 12 - Substitution and Elimination: Reactions of Haloalkanes172
- Ch. 13 - Alcohols, Ethers and Related Compounds: Substitution and Elimination239
- Ch. 14 - Structural Identification I: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification II: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution I: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution II: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems I: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems II: Pericyclic Reactions54
- Ch. 23 - Benzene I: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene II: Reactions Influenced by the Aromatic Ring62
- Ch. 25 - Amines: Structure, Reactions, and Synthesis27
- Ch. 26 - Amino Acids, Proteins, and Peptide Synthesis9
- Ch. 27 - Carbohydrates, Nucleic Acids, and Lipids54
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471Not the one you use?Change textbook
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Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 24a
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 24aChapter 1, Problem 24a
Without looking at Figure 2.20, use your intuition to estimate whether a bond is ionic, polar covalent, or covalent.
(a) Na―Cl
Verified step by step guidance1
Step 1: Begin by considering the electronegativity difference between the two atoms involved in the bond. Sodium (Na) is a metal with low electronegativity, while chlorine (Cl) is a nonmetal with high electronegativity.
Step 2: Recall the general rule for bond types: If the electronegativity difference is large (greater than 2.0), the bond is likely ionic. If the difference is moderate (between 0.5 and 2.0), the bond is polar covalent. If the difference is small (less than 0.5), the bond is nonpolar covalent.
Step 3: Use your intuition to estimate the electronegativity difference between Na and Cl. Sodium has an electronegativity of approximately 0.9, and chlorine has an electronegativity of approximately 3.0. The difference is significant.
Step 4: Based on the large electronegativity difference, predict that the bond between Na and Cl is ionic. This is because the electron from Na is likely to be completely transferred to Cl, forming ions.
Step 5: After making your prediction, consult Figure 2.20 to confirm whether your estimation aligns with the classification provided in the figure.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ionic Bonds
Ionic bonds form when there is a complete transfer of electrons from one atom to another, resulting in the formation of charged ions. This typically occurs between metals and nonmetals, where the metal loses electrons to become a positively charged cation, and the nonmetal gains electrons to become a negatively charged anion. The electrostatic attraction between these oppositely charged ions holds them together.
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Differences between ionic, polar and covalent bonds
Polar Covalent Bonds
Polar covalent bonds occur when two atoms share electrons unequally due to a difference in their electronegativities. In this type of bond, the atom with higher electronegativity attracts the shared electrons more strongly, resulting in a partial negative charge on that atom and a partial positive charge on the other. This creates a dipole moment, which is crucial for understanding molecular polarity and interactions.
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Covalent Bonds
Covalent bonds are formed when two atoms share one or more pairs of electrons, typically between nonmetals. This sharing allows each atom to attain a stable electron configuration, often resembling that of noble gases. Covalent bonds can be single, double, or triple, depending on the number of shared electron pairs, and they play a fundamental role in the structure and function of organic molecules.
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Related Practice
Textbook Question
Using only your intuition, rank the following covalent bonds in terms of their polarity (1 = most polar; 6 = least polar). [You can use the periodic trend of electronegativity, but don't use actual numbers.]
(a) C―C
(b) C―O
(c) C―H
(d) C―F
(e) C―Cl
(f) C―S
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Textbook Question
Based on your answer to Assessment 2.22, would you expect a larger atom to be more or less electronegative than a smaller atom?
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Textbook Question
(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?
(b) N vs. O
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Textbook Question
Draw the Lewis structure for the following molecules. Be sure to calculate the formal charge of each atom as a way of confirming your structure is correct.
(c) CF4
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Textbook Question
(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?
(d) B vs. Si
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