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 aluminum sulfide?

AlS3

Al2S3

AlS

Al3S2

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Verified step by step guidance

Step 1: Identify the charges of the ions involved. Aluminum typically forms a +3 charge (Al^{3+}), and sulfide forms a -2 charge (S^{2-}).

Step 2: To write the correct formula, balance the total positive and negative charges so that the compound is electrically neutral.

Step 3: Find the least common multiple (LCM) of the charges 3 and 2, which is 6. This means the total positive charge should be +6 and the total negative charge should be -6.

Step 4: Determine the number of aluminum and sulfide ions needed to reach these charges. For aluminum: 2 ions \times +3 = +6; for sulfide: 3 ions \times -2 = -6.

Step 5: Write the formula using the number of ions found: Al_{2}S_{3}.