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

4. Molecular Compounds

Lewis Dot Structures: Exceptions (Simplified)

GOB Chemistry

4. Molecular Compounds

Lewis Dot Structures: Exceptions (Simplified)

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Multiple Choice

Determine the Lewis Dot Structure for the following compound:SOCl₂

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Identify the total number of valence electrons in the compound SOCl2. Sulfur (S) has 6 valence electrons, oxygen (O) has 6, and each chlorine (Cl) has 7. Therefore, the total is 6 (S) + 6 (O) + 2*7 (Cl) = 26 valence electrons.

Determine the central atom. Sulfur is less electronegative than oxygen and chlorine, making it the central atom.

Arrange the atoms around the central sulfur atom. Connect the sulfur atom to the oxygen atom and the two chlorine atoms with single bonds initially.

Distribute the remaining valence electrons to satisfy the octet rule. Start by completing the octets of the outer atoms (oxygen and chlorine). Oxygen will form a double bond with sulfur to satisfy its octet, and each chlorine will have three lone pairs.

Check the formal charges to ensure the most stable structure. The formal charge is calculated as: Formal Charge = (Valence electrons) - (Non-bonding electrons) - 0.5*(Bonding electrons). Adjust the structure if necessary to minimize formal charges, ensuring the most stable Lewis structure.