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

Electron Arrangements

GOB Chemistry

2. Atoms and the Periodic Table

Electron Arrangements

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1:55 minutes

Problem 15

Textbook Question

An element has completely filled n = 1 and n = 2 shells and has six electrons in the n = 3 shell. Identify the element and its major group (i.e., main group, transition, etc.). Is it a metal or a nonmetal? Identify the orbital in which the last electron is found.

Verified step by step guidance

Step 1: Determine the total number of electrons in the element. The n = 1 shell can hold a maximum of 2 electrons, and the n = 2 shell can hold a maximum of 8 electrons. Since both shells are completely filled, this accounts for 2 + 8 = 10 electrons. Additionally, the n = 3 shell has 6 electrons, bringing the total to 10 + 6 = 16 electrons.

Step 2: Use the total number of electrons to identify the element. The atomic number of an element corresponds to the number of electrons in a neutral atom. An element with 16 electrons has an atomic number of 16, which corresponds to sulfur (S) on the periodic table.

Step 3: Determine the major group of the element. Sulfur is located in Group 16 (or VIA) of the periodic table, which is part of the main group elements. Group 16 elements are also known as the chalcogens.

Step 4: Classify the element as a metal or nonmetal. Sulfur is a nonmetal because it is located on the right side of the periodic table and exhibits properties typical of nonmetals, such as high electronegativity and the ability to form covalent bonds.

Step 5: Identify the orbital in which the last electron is found. The n = 3 shell consists of the 3s, 3p, and 3d orbitals. Since sulfur has 6 electrons in the n = 3 shell, the first 2 electrons fill the 3s orbital, and the next 4 electrons occupy the 3p orbitals. Therefore, the last electron is found in a 3p orbital.

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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 is represented by a series of numbers and letters indicating the energy levels (n) and types of orbitals (s, p, d, f) occupied by electrons. For the given element, the filled n = 1 and n = 2 shells indicate a stable core, while the six electrons in the n = 3 shell suggest a specific arrangement that helps identify the element.

Periodic Table Groups

Elements are organized in the periodic table into groups based on their electron configurations and chemical properties. The major groups include main group elements (s and p block), transition metals (d block), and inner transition metals (f block). The number of valence electrons, which can be inferred from the outermost shell, helps determine the element's group and its metallic or nonmetallic character.

Metallic vs. Nonmetallic Character

The distinction between metals and nonmetals is based on their physical and chemical properties. Metals are typically good conductors of heat and electricity, malleable, and ductile, while nonmetals are usually poor conductors and more brittle. The element in question, with six electrons in the n = 3 shell, is likely to be a nonmetal, specifically a member of the p block, where elements tend to exhibit nonmetallic characteristics.

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