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 correctly describes the bonding in the Lewis dot structure of BF_3 (boron trifluoride)?

BF_3 has two triple bonds and one single bond between boron and fluorine atoms.

BF_3 has three double bonds between boron and each fluorine atom.

BF_3 has three single bonds between boron and each fluorine atom.

BF_3 has one double bond and two single bonds between boron and fluorine atoms.

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Verified step by step guidance

Step 1: Identify the total number of valence electrons available for bonding in BF_3. Boron (B) has 3 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are three fluorine atoms, calculate the total valence electrons as: $3 + 3 \times 7$.

Step 2: Draw a skeletal structure with boron as the central atom bonded to three fluorine atoms. Connect each fluorine atom to boron with a single bond initially.

Step 3: Distribute the remaining valence electrons to complete the octets of the fluorine atoms. Each fluorine needs 8 electrons total (including bonding electrons), so add lone pairs around fluorine atoms accordingly.

Step 4: Check the octet rule for boron. Boron is an exception and often forms stable compounds with only 6 electrons around it. Confirm if boron has 6 electrons (three single bonds) or if double or triple bonds are necessary to complete its octet.

Step 5: Conclude the bonding type based on the electron count and octet rule. Since boron is stable with 6 electrons, the structure with three single bonds between boron and each fluorine atom correctly describes the bonding in BF_3.