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 magnesium nitrate?

Mg2N3O6

MgNO3

Mg2(NO3)3

Mg(NO3)2

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Verified step by step guidance

Step 1: Identify the ions involved. Magnesium typically forms a Mg^{2+} ion, and the nitrate ion is NO_3^{-}.

Step 2: Determine the charges of the ions. Magnesium has a charge of +2, and nitrate has a charge of -1.

Step 3: Balance the total positive and negative charges to form a neutral compound. Since Mg^{2+} has a +2 charge, you need two NO_3^{-} ions to balance the charge (2 × -1 = -2).

Step 4: Write the chemical formula by placing the magnesium ion first, followed by the nitrate ion with a subscript indicating the number of nitrate ions needed to balance the charge: Mg(NO_3)_2.

Step 5: Verify that the formula is electrically neutral and correctly represents the ratio of ions.