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Determine the hybridization of the central atom in BF3.
Determine the hybridization of the central atom in BF3.
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Practice Questions
1 question
Q1
Determine the hybridization of the central atom in BF3.
sp
sp2
sp3
dsp3
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Boron in BF3 is sp2 hybridized, forming three equivalent sp2 hybrid orbitals.
Questions & Step-by-step Solutions
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Q
Q: Determine the hybridization of the central atom in BF3.
Solution:
Boron in BF3 is sp2 hybridized, forming three equivalent sp2 hybrid orbitals.
Steps: 6
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Step 1: Identify the central atom in BF3, which is boron (B).
Step 2: Count the number of bonds boron forms with surrounding atoms. In BF3, boron forms three bonds with three fluorine (F) atoms.
Step 3: Determine the number of electron groups around the central atom. Boron has three bonding pairs and no lone pairs.
Step 4: Use the VSEPR theory to determine the geometry. Three bonding pairs result in a trigonal planar shape.
Step 5: Identify the hybridization that corresponds to a trigonal planar shape. This is sp2 hybridization.
Step 6: Conclude that boron in BF3 is sp2 hybridized, forming three equivalent sp2 hybrid orbitals.
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