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

How many lone pairs of electrons are on the As atom in the Lewis dot structure of AsF₃?

3 lone pairs

1 lone pair

0 lone pairs

2 lone pairs

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Verified step by step guidance

Step 1: Begin by identifying the total number of valence electrons available for the molecule AsF₃. Arsenic (As) is in group 15 of the periodic table, which means it has 5 valence electrons. Fluorine (F) is in group 17, so each fluorine atom has 7 valence electrons. Since there are three fluorine atoms, the total number of valence electrons from fluorine is 3 × 7 = 21.

Step 2: Add the valence electrons from arsenic and fluorine to find the total number of valence electrons in AsF₃. This is 5 (from As) + 21 (from 3 F atoms) = 26 valence electrons.

Step 3: Construct the Lewis structure by placing the arsenic atom in the center and arranging the three fluorine atoms around it. Connect each fluorine atom to the arsenic atom with a single bond. Each bond uses 2 electrons, so 3 bonds use 6 electrons.

Step 4: Distribute the remaining electrons to satisfy the octet rule for each atom. Start by completing the octets for the fluorine atoms. Each fluorine atom needs 8 electrons, including the bonding pair. Since each fluorine already has 2 electrons from the bond, place 6 more electrons (3 lone pairs) around each fluorine atom.

Step 5: After placing electrons around the fluorine atoms, check the number of electrons used. You have used 6 electrons for bonds and 18 electrons for the lone pairs on fluorine, totaling 24 electrons. The remaining 2 electrons are placed as a lone pair on the arsenic atom, completing its octet.