Table of contents

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

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

General Chemistry

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

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Multiple Choice

Which of the following statements correctly describes the Lewis dot structure of the neutral compound NCS-?

The structure has a linear arrangement with nitrogen triple-bonded to carbon and carbon single-bonded to sulfur, with a negative charge on sulfur.

The structure has a bent arrangement with nitrogen single-bonded to carbon and carbon double-bonded to sulfur, with a negative charge on nitrogen.

The structure has a trigonal planar arrangement with nitrogen, carbon, and sulfur all single-bonded to each other, with no formal charges.

The structure has a linear arrangement with nitrogen double-bonded to carbon and carbon double-bonded to sulfur, with a negative charge on carbon.

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Verified step by step guidance

Identify the atoms involved in the NCS⁻ ion: nitrogen (N), carbon (C), and sulfur (S), and note that the overall charge is -1.

Determine the total number of valence electrons by adding the valence electrons of each atom and including the extra electron for the negative charge: N has 5, C has 4, S has 6, plus 1 extra electron for the charge.

Consider possible bonding arrangements and electron distributions that satisfy the octet rule for each atom while accounting for the total valence electrons and the negative charge.

Evaluate the formal charges for each atom in different Lewis structures to find the most stable arrangement, aiming for the lowest formal charges and placing the negative charge on the most electronegative atom.

Conclude that the most stable Lewis structure is linear with nitrogen triple-bonded to carbon and carbon single-bonded to sulfur, placing the negative charge on sulfur, which matches the correct description.