Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

2. Atoms and the Periodic Table

Electronic Structure: Subshells

GOB Chemistry

2. Atoms and the Periodic Table

Electronic Structure: Subshells

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2:41 minutes

Problem 66

Textbook Question

How many subshells are there in the third shell? The fourth shell? The fifth shell?

Verified step by step guidance

Understand that the number of subshells in a shell is determined by the principal quantum number (n). The principal quantum number corresponds to the shell number.

Recall that the number of subshells in a shell is equal to the value of n. For example, if n = 3 (third shell), there are 3 subshells.

List the subshells for each shell: For n = 3, the subshells are 3s, 3p, and 3d. For n = 4, the subshells are 4s, 4p, 4d, and 4f. For n = 5, the subshells are 5s, 5p, 5d, 5f, and 5g.

Note that the subshells are labeled based on the azimuthal quantum number (l), which ranges from 0 to (n-1). Each value of l corresponds to a specific subshell type: s (l=0), p (l=1), d (l=2), f (l=3), g (l=4), etc.

Conclude that the third shell (n=3) has 3 subshells, the fourth shell (n=4) has 4 subshells, and the fifth shell (n=5) has 5 subshells.

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Key Concepts

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

Electron Shells

Electron shells are the regions around an atom's nucleus where electrons are likely to be found. Each shell is associated with a principal quantum number (n), which indicates its energy level. The first shell (n=1) can hold a maximum of 2 electrons, the second (n=2) can hold 8, and this pattern continues with increasing energy levels.

Subshells

Subshells are divisions within electron shells that define the shape and orientation of the electron cloud. Each shell can contain one or more subshells, designated by the letters s, p, d, and f. The number of subshells in a shell corresponds to the principal quantum number, with n=1 having 1 subshell (s), n=2 having 2 subshells (s and p), and so forth.

Quantum Numbers

Quantum numbers are numerical values that describe the unique quantum state of an electron in an atom. The principal quantum number (n) indicates the shell, while the azimuthal quantum number (l) defines the subshell. For example, in the third shell (n=3), there are three subshells (l=0 for s, l=1 for p, l=2 for d), while the fourth shell (n=4) has four subshells (s, p, d, f).

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