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 neutral NOCl?

Nitrogen is bonded to oxygen by a double bond and to chlorine by a single bond, with one lone pair on nitrogen.

Nitrogen is bonded to both oxygen and chlorine by single bonds, with three lone pairs on nitrogen.

Nitrogen is bonded to oxygen by a triple bond and to chlorine by a single bond, with no lone pairs on nitrogen.

Nitrogen is bonded to oxygen by a single bond and to chlorine by a double bond, with two lone pairs on nitrogen.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for NOCl by adding the valence electrons of nitrogen (N), oxygen (O), and chlorine (Cl). Nitrogen has 5, oxygen has 6, and chlorine has 7 valence electrons, so total valence electrons = 5 + 6 + 7.

Step 2: Arrange the atoms with nitrogen as the central atom because it is less electronegative than oxygen and chlorine. Connect nitrogen to oxygen and chlorine with single bonds initially.

Step 3: Distribute the remaining valence electrons to satisfy the octet rule for the outer atoms (oxygen and chlorine) first by adding lone pairs around them.

Step 4: Check the octet of the central nitrogen atom. If nitrogen does not have a complete octet, form double or triple bonds by converting lone pairs from oxygen or chlorine into bonding pairs with nitrogen.

Step 5: Confirm the final Lewis structure by ensuring all atoms have complete octets (except hydrogen if present), the total number of electrons matches the total valence electrons, and the formal charges are minimized, which will help identify the correct bonding pattern (double bond between N and O, single bond between N and Cl, and one lone pair on nitrogen).