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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 51m
7. Gases3h 49m
8. Thermochemistry2h 35m
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 34m
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

Which element within the thiocyanate ion possesses a negative charge?

All of them.

None of them.

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Verified step by step guidance

Examine the Lewis structure of the thiocyanate ion (SCN⁻) provided in the image. Notice the arrangement of atoms: nitrogen (N), carbon (C), and sulfur (S).

Identify the formal charges on each atom in the thiocyanate ion. Formal charge is calculated using the formula: Formal Charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons/2).

Calculate the formal charge for nitrogen (N). Nitrogen typically has 5 valence electrons. In the structure, it has 2 non-bonding electrons and is involved in 3 bonds (6 bonding electrons).

Calculate the formal charge for carbon (C). Carbon typically has 4 valence electrons. In the structure, it has no non-bonding electrons and is involved in 4 bonds (8 bonding electrons).

Calculate the formal charge for sulfur (S). Sulfur typically has 6 valence electrons. In the structure, it has 6 non-bonding electrons and is involved in 1 bond (2 bonding electrons).

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