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 NH2F?

Nitrogen is bonded to one hydrogen atom and two fluorine atoms, with one lone pair on nitrogen.

Nitrogen is bonded to two hydrogen atoms and one fluorine atom, with no lone pairs on nitrogen.

Nitrogen is bonded to two hydrogen atoms and one fluorine atom, with one lone pair on nitrogen.

Nitrogen is bonded to three hydrogen atoms and one fluorine atom, with no lone pairs on nitrogen.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the molecule NH2F. Nitrogen has 5 valence electrons, each hydrogen has 1, and fluorine has 7. Add these together to find the total valence electrons available for bonding and lone pairs.

Step 2: Identify the central atom, which is usually the least electronegative element that is not hydrogen. In NH2F, nitrogen is the central atom bonded to two hydrogens and one fluorine atom.

Step 3: Draw single bonds between the nitrogen and each of the attached atoms (two hydrogens and one fluorine). Each single bond represents 2 electrons shared between atoms.

Step 4: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom, starting with the most electronegative atom (fluorine) and then placing any leftover electrons on nitrogen.

Step 5: Check the Lewis structure to ensure nitrogen has a total of 8 electrons around it (including bonding and lone pairs). This will confirm that nitrogen has one lone pair and is bonded to two hydrogens and one fluorine, matching the correct description.