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

3. Ionic Compounds

Periodic Trend: Ionization Energy (Simplified)

GOB Chemistry

3. Ionic Compounds

Periodic Trend: Ionization Energy (Simplified)

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Multiple Choice

Which element from Group 7A has lowest ionization energy.

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Identify the elements in Group 7A (also known as Group 17 or the halogens) from the periodic table: Fluorine (F), Chlorine (Cl), Bromine (Br), and Iodine (I). Note that Neon (Ne) is not part of Group 7A; it is a noble gas in Group 8A.

Understand the concept of ionization energy: it is the energy required to remove an electron from an atom in the gaseous state. Generally, ionization energy decreases as you move down a group in the periodic table.

Recall that as you move down Group 7A from Fluorine to Iodine, the atomic size increases. This is because additional electron shells are added, increasing the distance between the nucleus and the outermost electrons.

Recognize that with increased atomic size, the outermost electrons are less tightly held by the nucleus due to increased electron shielding. This results in a lower ionization energy for elements further down the group.

Conclude that among the halogens listed (F, Cl, Br, I), Iodine (I) has the lowest ionization energy because it is the heaviest and largest atom in Group 7A, making it easier to remove an electron compared to the others.