Textbook Question
Fill in the blank. Oxygen ionizes to become ― 2 instead of ― 1 because O2- is more ___________ .
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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 20b
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 20bChapter 1, Problem 20b
(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
Verified step by step guidance1
Step 1: Recall the periodic trend for electronegativity. Electronegativity generally increases across a period (left to right) and decreases down a group in the periodic table.
Step 2: Identify the position of nitrogen (N) and oxygen (O) in the periodic table. Both elements are in the same period (Period 2), but oxygen is to the right of nitrogen.
Step 3: Based on the periodic trend, oxygen is expected to be more electronegative than nitrogen because it is further to the right in the same period.
Step 4: To confirm this, look at the actual Pauling electronegativity values. Nitrogen has a value of approximately 3.0, while oxygen has a value of approximately 3.5. This confirms that oxygen is more electronegative.
Step 5: Explain why oxygen is more electronegative. Oxygen has a higher nuclear charge (more protons in the nucleus) compared to nitrogen, which results in a stronger attraction for electrons in a covalent bond.
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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. It is a key concept in understanding how atoms interact in molecules. The Pauling scale is commonly used to quantify electronegativity values, with higher values indicating a stronger tendency to attract electrons.
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Electronegativity
Periodic Trends
Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Electronegativity generally increases across a period from left to right and decreases down a group. This trend is crucial for comparing the electronegativity of elements like nitrogen (N) and oxygen (O) in the given question.
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Pauling Scale
The Pauling scale is a numerical scale for measuring electronegativity, developed by Linus Pauling. It assigns values to elements based on their ability to attract electrons in a bond, with fluorine being the most electronegative at 4.0. For the pair N vs. O, the actual Pauling values (3.0 for N and 3.5 for O) indicate that oxygen is more electronegative, which is essential for answering the question.
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Related Practice
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
Show the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species.
(a) Al and F
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Textbook Question
Show the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species.
(b) Mg and Br
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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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Textbook Question
Without looking at Figure 2.20, use your intuition to estimate whether a bond is ionic, polar covalent, or covalent.
(a) Na―Cl
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