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 a neutral molecule of ArF_2?

Argon is the central atom, bonded to two fluorine atoms, with no lone pairs on argon.

Argon is the central atom, bonded to two fluorine atoms, with one lone pair on argon.

Fluorine is the central atom, bonded to two argon atoms, with two lone pairs on fluorine.

Argon is the central atom, bonded to two fluorine atoms, with three lone pairs on argon.

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Verified step by step guidance

Step 1: Identify the central atom in the molecule ArF_2. Typically, the least electronegative atom (excluding hydrogen) is the central atom. Argon (Ar) is a noble gas and less electronegative than fluorine (F), so Ar is the central atom.

Step 2: Determine the total number of valence electrons available. Argon has 8 valence electrons, and each fluorine has 7 valence electrons. For ArF_2, total valence electrons = 8 (Ar) + 2 × 7 (F) = 22 electrons.

Step 3: Draw single bonds between the central atom (Ar) and each fluorine atom. Each bond uses 2 electrons, so 2 bonds use 4 electrons. Subtract these from the total valence electrons to find remaining electrons: 22 - 4 = 18 electrons left.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule for the fluorine atoms first. Each fluorine needs 6 more electrons (3 lone pairs) to complete its octet, so 2 fluorines require 12 electrons. Subtract these from the remaining electrons: 18 - 12 = 6 electrons left.

Step 5: Assign the remaining 6 electrons as lone pairs on the central argon atom. Since each lone pair consists of 2 electrons, 6 electrons correspond to 3 lone pairs on argon. This completes the Lewis structure with argon bonded to two fluorines and three lone pairs on argon.