Domanda del libro di testo
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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Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
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TOC.tableOfContents
- 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 1: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes 2: 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 1: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification 2: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution 1: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution 2: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems 1: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems 2: Pericyclic Reactions54
- Ch. 23 - Benzene 1: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene 2: 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: 9780137566471Non è quello che usi tu?Cambia libro di testo
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Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblema 10a
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblema 10aCapitolo 1, Problema 10a
A chemistry student drew the following incorrect electron configuration for carbon. (a) Correct the diagram.
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Understand the electron configuration of carbon: Carbon has an atomic number of 6, meaning it has 6 electrons. These electrons are distributed in orbitals according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
Recall the order of orbital filling: Electrons fill orbitals in the order of increasing energy levels. For carbon, the order is 1s, 2s, and then 2p. The correct configuration should be written as: .
Apply Hund's rule for the 2p orbitals: When filling the 2p orbitals, electrons are placed in separate orbitals with parallel spins before pairing. This minimizes electron repulsion and stabilizes the atom.
Correct the diagram: Ensure that the 1s and 2s orbitals are fully filled with two electrons each, and the 2p orbitals have one electron in two separate orbitals with parallel spins.
Double-check the corrected diagram: Verify that the total number of electrons is 6, and that the configuration adheres to the principles of electron distribution (Aufbau principle, Hund's rule, and Pauli exclusion principle).
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Electron Configuration
Electron configuration describes the distribution of electrons in an atom's orbitals. For carbon, which has six electrons, the correct configuration is 1s² 2s² 2p². This notation indicates that two electrons occupy the 1s orbital, two occupy the 2s orbital, and two occupy the 2p orbitals, reflecting the principles of quantum mechanics.
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02:14
The Electron Configuration
Aufbau Principle
The Aufbau principle states that electrons fill atomic orbitals in order of increasing energy levels, starting from the lowest. This means that before electrons can occupy higher energy orbitals, such as 2p, the lower energy orbitals (1s and 2s) must be filled first. Understanding this principle is crucial for accurately determining the electron configuration of an element.
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2:38The 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 principle explains why each orbital can hold a maximum of two electrons with opposite spins. It is essential for understanding how electrons are arranged in orbitals and helps prevent incorrect configurations.
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02:54Three rules about orbitals you need to know.
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