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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 36m
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

11. Bonding & Molecular Structure

Formal Charge

General Chemistry

11. Bonding & Molecular Structure

Formal Charge

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Multiple Choice

Calculate the formal charges for each of the oxygen atoms within the nitrite ion, NO₂^–.

0, -1

+1, 0

-1, -1

+1, +1

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Verified step by step guidance

Identify the number of valence electrons for a neutral oxygen atom, which is 6.

For oxygen atom A, count the number of electrons in lone pairs and bonds. Oxygen A has 4 electrons in lone pairs and 2 electrons in a double bond with nitrogen.

Calculate the formal charge for oxygen A using the formula: Formal Charge = Valence Electrons - (Lone Pair Electrons + 1/2 Bonding Electrons). Substitute the values: 6 - (4 + 2) = 0.

For oxygen atom B, count the number of electrons in lone pairs and bonds. Oxygen B has 6 electrons in lone pairs and 1 electron in a single bond with nitrogen.

Calculate the formal charge for oxygen B using the same formula: Formal Charge = Valence Electrons - (Lone Pair Electrons + 1/2 Bonding Electrons). Substitute the values: 6 - (6 + 1) = -1.