Multiple Choice
After drawing the Lewis structure of CHOCl (formyl chloride), what is the ideal bond angle around the central carbon atom?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following correctly describes the bonding in the Lewis dot structure of BF_3 (boron trifluoride)?
A
BF_3 has two triple bonds and one single bond between boron and fluorine atoms.
B
BF_3 has three double bonds between boron and each fluorine atom.
C
BF_3 has three single bonds between boron and each fluorine atom.
D
BF_3 has one double bond and two single bonds between boron and fluorine atoms.
Verified step by step guidance1
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.
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