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 is the correct Lewis dot structure for the neutral compound HNCO (isocyanic acid)?

H–N≡C–O, with a triple bond between N and C and a single bond between C and O.

H–N=C=O, with all atoms having a complete octet and no formal charges.

H–N–C–O, with single bonds between all atoms and no lone pairs.

H–N–C=O, with a single bond between N and C and a double bond between C and O.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the molecule HNCO. Sum the valence electrons from each atom: Hydrogen (H) has 1, Nitrogen (N) has 5, Carbon (C) has 4, and Oxygen (O) has 6 valence electrons.

Step 2: Arrange the atoms in a plausible connectivity. Since the formula is HNCO, a common arrangement is H bonded to N, which is bonded to C, which is bonded to O. This reflects the sequence H–N–C–O.

Step 3: Draw single bonds between the atoms initially, and then distribute the remaining valence electrons as lone pairs to satisfy the octet rule (or duet for hydrogen) for each atom. Remember that hydrogen only needs 2 electrons, while N, C, and O aim for 8 electrons.

Step 4: Adjust the bonding by forming double or triple bonds if necessary to ensure all atoms (except hydrogen) have a complete octet and to minimize formal charges. Calculate formal charges for each atom using the formula: $\text{Formal Charge} = \text{Valence Electrons} - \text{Nonbonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons}$.

Step 5: Compare the possible Lewis structures by checking which one has all atoms with complete octets and the lowest formal charges. The correct structure will have nitrogen double bonded to carbon and carbon double bonded to oxygen (H–N=C=O), with all atoms having complete octets and minimal formal charges.