Textbook Question
Choose the larger atom in each pair.
(d) N or S
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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 10b
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 10bChapter 1, Problem 10b
A chemistry student drew the following incorrect electron configuration for carbon. (b) Which rule wasn't followed by the student?
Verified step by step guidance1
Step 1: Analyze the electron configuration provided in the image. The configuration shows the 1s and 2s orbitals filled correctly, but the 2p orbitals have two electrons paired in one box and the other two boxes are empty.
Step 2: Recall Hund's Rule, which states that electrons must occupy degenerate orbitals (orbitals of the same energy level) singly before pairing occurs. This minimizes electron repulsion and stabilizes the atom.
Step 3: Identify the mistake in the student's drawing. The student paired two electrons in one 2p orbital without first placing one electron in each of the three 2p orbitals.
Step 4: Explain the correct approach. According to Hund's Rule, the correct electron configuration for carbon's 2p orbitals should have one electron in each of the three 2p orbitals before any pairing occurs.
Step 5: Conclude that the rule violated by the student is Hund's Rule, and emphasize the importance of following this rule for accurate electron configurations.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Aufbau Principle
The Aufbau Principle states that electrons occupy the lowest energy orbitals first before filling higher energy levels. For carbon, which has six electrons, the correct order of filling is 1s², 2s², and then 2p². This principle is fundamental in determining the electron configuration of elements.
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2:38
The Electron Configuration
Pauli Exclusion Principle
The Pauli Exclusion Principle asserts that no two electrons in an atom can have the same set of four quantum numbers. This means that an orbital can hold a maximum of two electrons, which must have opposite spins. In the provided configuration, if the same orbital is shown with two electrons having the same spin, this principle is violated.
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02:54Three rules about orbitals you need to know.
Hund's Rule
Hund's Rule states that electrons will fill degenerate orbitals (orbitals of the same energy) singly before pairing up. In the case of the 2p orbitals for carbon, the correct configuration should show one electron in each of the three 2p orbitals before any pairing occurs. This rule helps minimize electron-electron repulsion and stabilizes the atom.
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Related Practice
Textbook Question
Chlorine exists as one of two isotopes with atomic masses of 34.969 amu (35Cl) and 36.966 amu (37Cl) . Calculate the relative abundance of 35Cl and 37Cl based on the average atomic mass of 35.453 amu.
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Textbook Question
Choose the larger atom in each pair.
(b) O or F
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Textbook Question
A chemistry student drew the following incorrect electron configuration for carbon. (a) Correct the diagram.
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Textbook Question
Would you expect electrons in the 2s or 3s orbital to be more reactive? Why?
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Textbook Question
Bromine-79 (50.7% abundance) has an atomic mass of 78.918 amu, whereas bromine-81 (49.3% abundance) has an atomic mass of 80.916 amu. From these data, calculate the average atomic mass of bromine that you would expect to see in the periodic table.
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