Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Atomic Structure

Organic Chemistry

1. A Review of General Chemistry

Atomic Structure

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5:39 minutes

Problem 5a

Textbook Question

Write the ground-state electronic configuration for chlorine (atomic number 17), bromine (atomic number 35), and iodine (atomic number 53).

Verified step by step guidance

Determine the total number of electrons for each element based on their atomic numbers: Chlorine (17 electrons), Bromine (35 electrons), and Iodine (53 electrons).

Recall the order of orbital filling based on the Aufbau principle: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, etc.

For chlorine (atomic number 17), distribute the electrons into orbitals following the Aufbau principle and Hund's rule:

1s^2 2s^2 2p^6 3s^2 3p^5

For bromine (atomic number 35), distribute the electrons into orbitals:

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^5

For iodine (atomic number 53), distribute the electrons into orbitals:

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^5

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It follows the Aufbau principle, which states that electrons fill the lowest energy orbitals first, and is represented using a notation that indicates the energy levels and sublevels occupied by electrons. Understanding this concept is crucial for determining the ground-state configurations of elements.

Periodic Table and Atomic Number

The periodic table organizes elements based on their atomic number, which is the number of protons in the nucleus. This number also indicates the number of electrons in a neutral atom, allowing for the determination of electron configurations. Recognizing the position of elements like chlorine, bromine, and iodine in the periodic table helps in predicting their electron arrangements.

Valence Electrons

Valence electrons are the outermost electrons of an atom and play a key role in chemical bonding and reactivity. The number of valence electrons can be inferred from the electron configuration and is particularly important for understanding the chemical properties of elements in the same group of the periodic table, such as halogens like chlorine, bromine, and iodine.

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Related Practice

Textbook Question

Draw the ground-state electronic configuration for each of the following:

b. Ca²⁺

Textbook Question

Draw the ground-state electronic configuration for each of the following:

a. Mg

Textbook Question

Chlorine has two isotopes, ³⁵Cl and ³⁷Cl; 75.77% of chlorine is ³⁵Cl, and 24.23% is ³⁷Cl. The atomic mass of ³⁵Cl is 34.969 amu, and the atomic mass of ³⁷Cl is 36.966 amu. What is the atomic mass of chlorine?

Textbook Question

Name the element that corresponds to each electronic configuration.

a. 1s² 2s² 2p²

b. 1s² 2s² 2p⁴

c. 1s² 2s² 2p⁶ 3s² 3p³

d. 1s² 2s² 2p⁶ 3s² 3p⁵

Textbook Question

Oxygen has three isotopes, ¹⁶O, ¹⁷O, and ¹⁸O. The atomic number of oxygen is 8. How many protons and neutrons does each of the isotopes have?

Textbook Question

a. How many protons do the following species have?

b. How many electrons does each have?

Na⁺
Ar
Cl^-

Textbook Question

Write the electronic configurations of the third-row elements shown in the partial periodic table in Figure 1-6.

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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