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 best represents the Lewis dot structure of HF, with the elements in the order H–F?

H–F

H :F:

:H–F:

H::F

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Verified step by step guidance

Step 1: Identify the total number of valence electrons for the molecule HF. Hydrogen (H) has 1 valence electron, and fluorine (F) has 7 valence electrons, so the total is 1 + 7 = 8 valence electrons.

Step 2: Determine the bonding between the atoms. Since HF is a diatomic molecule, hydrogen and fluorine will share a pair of electrons to form a single covalent bond, represented as H–F.

Step 3: Assign the remaining valence electrons as lone pairs. After forming the single bond (2 electrons), fluorine will have 6 electrons left, which are placed as three lone pairs around fluorine.

Step 4: Represent the Lewis structure by showing the single bond between H and F, with fluorine having three lone pairs (six dots) around it, and hydrogen having no lone pairs since it only needs 2 electrons to complete its shell.

Step 5: Confirm that the Lewis structure satisfies the octet rule for fluorine (8 electrons total) and the duet rule for hydrogen (2 electrons total), ensuring the structure is stable and correctly represents HF.