Textbook Question
Sodium amide (NaNH₂) dissociates to give a sodium cation (Na+) and amide ion (NH2–) a very strong base. In the following three equations, identify which definition of base is being exemplified.
(b)
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Ch. 4 - Acids and Bases: Electron Flow
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
Chapter 3, Problem 6c
In each pair of atoms, which has the larger atomic radius? Which is more electronegative?
(c) O vs. S
Verified step by step guidance1
Step 1: Understand the periodic trends for atomic radius. Atomic radius increases as you move down a group in the periodic table because additional electron shells are added, increasing the distance between the nucleus and the outermost electrons.
Step 2: Compare the positions of oxygen (O) and sulfur (S) in the periodic table. Both elements are in Group 16 (chalcogens), but sulfur is located below oxygen, meaning sulfur has a larger atomic radius due to having more electron shells.
Step 3: Understand the periodic trends for electronegativity. Electronegativity increases as you move across a period from left to right and decreases as you move down a group. This is because atoms higher in a group have fewer electron shells, resulting in a stronger attraction between the nucleus and bonding electrons.
Step 4: Compare the electronegativity of oxygen and sulfur. Since oxygen is above sulfur in Group 16, it is more electronegative because it has fewer electron shells, leading to a stronger pull on bonding electrons.
Step 5: Summarize the findings. Sulfur has the larger atomic radius, while oxygen is more electronegative. These trends are consistent with periodic table principles.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Atomic Radius
Atomic radius refers to the size of an atom, typically measured from the nucleus to the outermost electron shell. As you move down a group in the periodic table, atomic radius increases due to the addition of electron shells, which outweighs the increase in nuclear charge. Therefore, sulfur (S), being below oxygen (O) in the periodic table, has a larger atomic radius.
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The difference between atomic numbers and atomic mass.
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It generally increases across a period from left to right and decreases down a group. Oxygen, being higher in the periodic table than sulfur, has a greater electronegativity, meaning it is more effective at attracting electrons compared to sulfur.
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Periodic Trends
Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change across periods and down groups. Key trends include atomic radius, electronegativity, ionization energy, and electron affinity. Understanding these trends helps predict the behavior of elements, such as why oxygen is more electronegative than sulfur and why sulfur has a larger atomic radius.
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03:43The radical stability trend.
Related Practice
Textbook Question
Sodium amide (NaNH2) dissociates to give a sodium cation (Na+) and amide ion (NH2-) a very strong base. In the following three equations, identify which definition of base is being exemplified.
(c)
Textbook Question
Sodium amide (NaNH2) dissociates to give a sodium cation (Na+) and amide ion (NH2-) a very strong base. In the following three equations, identify which definition of base is being exemplified.
(a)
Textbook Question
In each pair of atoms, which has the larger atomic radius? Which is more electronegative?
(b) C vs. O
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Textbook Question
Draw the molecular orbital picture of the following molecules and ions. In each, how many electrons are in the p orbital on the central atom? (b) BH3
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Textbook Question
Draw the molecular orbital picture of the following molecules and ions. In each, how many electrons are in the p orbital on the central atom? (c) AlCl3
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