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: Electron Affinity (Simplified)

GOB Chemistry

3. Ionic Compounds

Periodic Trend: Electron Affinity (Simplified)

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Multiple Choice

Rank the following elements in order of increasing electron affinity:Cs, Hg, F, S

Hg < S < F < Cs

Hg < F < S < Cs

Cs < S < F < Hg

Cs < S < Hg < F

Cs < Hg < S < F

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Verified step by step guidance

Understand the concept of electron affinity: Electron affinity is the amount of energy released when an electron is added to a neutral atom in the gaseous state to form a negative ion. Generally, elements with higher electron affinity values are more likely to gain electrons.

Recall the periodic trend: Electron affinity generally increases across a period from left to right and decreases down a group in the periodic table. This is because atoms become smaller across a period, allowing them to attract additional electrons more strongly.

Identify the positions of the given elements in the periodic table: Cs (Cesium) is in Group 1, Period 6; Hg (Mercury) is in Group 12, Period 6; S (Sulfur) is in Group 16, Period 3; F (Fluorine) is in Group 17, Period 2.

Apply the periodic trend to the given elements: Since Cs is in Group 1, it has a low electron affinity. Hg, being a transition metal, also has a relatively low electron affinity. S and F, being nonmetals, have higher electron affinities, with F having the highest due to its position in Group 17.

Rank the elements based on the trend: Cs, being in Group 1, has the lowest electron affinity, followed by Hg. S, being a nonmetal, has a higher electron affinity than Hg, and F, being in Group 17, has the highest electron affinity. Therefore, the order is Cs < Hg < S < F.