Account for the difference in the shapes of the boron trifluoride (BF₃) molecule and the ammonia (NH₃) molecule. - Leaving Cert Chemistry - Question d - 2015
Question d
Account for the difference in the shapes of the boron trifluoride (BF₃) molecule and the ammonia (NH₃) molecule.
Worked Solution & Example Answer:Account for the difference in the shapes of the boron trifluoride (BF₃) molecule and the ammonia (NH₃) molecule. - Leaving Cert Chemistry - Question d - 2015
Step 1
Boron trifluoride (BF₃)
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Answer
The central atom of boron trifluoride (BF₃) has three bond pairs of electrons. It does not have any lone pairs on the boron atom, resulting in a trigonal planar shape. The bond angle is approximately 120°.
Step 2
Ammonia (NH₃)
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Answer
In ammonia (NH₃), the central nitrogen atom has three bond pairs and one lone pair of electrons. The presence of the lone pair repels the bonding pairs more strongly, resulting in a pyramidal shape with a bond angle of approximately 107°.
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