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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following best represents the correct Lewis dot structure for a neutral molecule of hypofluorous acid (HOF)?

H is bonded to O, which is bonded to F; O has two lone pairs, F has three lone pairs, and all atoms have complete octets except H.

H is bonded to F, which is bonded to O; O has three lone pairs, F has two lone pairs.

H is bonded to F, which is double-bonded to O; O has two lone pairs, F has two lone pairs.

H is bonded to O, which is double-bonded to F; O has one lone pair, F has three lone pairs.

Previous problemNext problem

Verified step by step guidance

Identify the atoms involved in hypofluorous acid (HOF): hydrogen (H), oxygen (O), and fluorine (F). Consider their typical bonding patterns and electronegativities.

Determine the central atom: oxygen is less electronegative than fluorine and can form two bonds, so it is the central atom bonded to both H and F.

Draw single bonds connecting H to O and O to F, since hydrogen forms only one bond and fluorine typically forms one bond with three lone pairs.

Assign lone pairs to complete the octets: oxygen should have two lone pairs to complete its octet, fluorine should have three lone pairs, and hydrogen has only one bond (duet).

Verify that all atoms have complete octets (or duet for hydrogen) and that the molecule is neutral, confirming the correct Lewis structure is H bonded to O, which is bonded to F; O has two lone pairs, F has three lone pairs.