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 represents the correct Lewis structure for the neutral compound NOF?

N with a single bond to O and a double bond to F, with one lone pair on N

N with a triple bond to O and a single bond to F, with no lone pairs on N

N with a double bond to O and a single bond to F, with one lone pair on N

N with a single bond to O and a single bond to F, with one lone pair on N

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the compound NOF. Nitrogen (N) has 5 valence electrons, oxygen (O) has 6, and fluorine (F) has 7. Add these together to get the total number of valence electrons.

Step 2: Identify the central atom. In this case, nitrogen (N) is the central atom because it is less electronegative than oxygen and fluorine.

Step 3: Arrange the atoms around the central atom and draw single bonds initially. Connect N to O and N to F with single bonds. This uses up 4 valence electrons (2 for each bond).

Step 4: Distribute the remaining valence electrons to satisfy the octet rule, starting with the most electronegative atoms. Place lone pairs on O and F to complete their octets, then place any remaining electrons on N.

Step 5: Adjust the bonding to ensure all atoms have a complete octet. If necessary, convert lone pairs on adjacent atoms into double or triple bonds with the central atom. In this case, form a double bond between N and O to satisfy the octet rule for all atoms, leaving one lone pair on N.