Table of contents

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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

3. Chemical Reactions

Naming Ionic Compounds

General Chemistry

3. Chemical Reactions

Naming Ionic Compounds

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Multiple Choice

Which of the following is the correct chemical formula for ammonium sulfide?

NH_4S

NH_4SO_3

(NH_4)_2SO_4

(NH_4)_2S

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Verified step by step guidance

Identify the ions involved: ammonium is the polyatomic ion NH_4^+ and sulfide is the anion S^{2-}.

Determine the charges on each ion: ammonium (NH_4^+) has a charge of +1, and sulfide (S^{2-}) has a charge of -2.

Balance the total positive and negative charges to make a neutral compound. Since sulfide has a charge of -2, you need two ammonium ions (each +1) to balance it.

Write the formula by placing the ammonium ion in parentheses with a subscript 2 to indicate two ammonium ions, followed by the sulfide ion: (NH_4)_2S.

Verify that the formula is neutral by confirming the total positive charge (+2 from two NH_4^+) balances the total negative charge (-2 from S^{2-}).