Account for the differences in the shapes of the ammonia (NH₃) and boron trifluoride (BF₃) molecules. - Leaving Cert Chemistry - Question b - 2004
Question b
Account for the differences in the shapes of the ammonia (NH₃) and boron trifluoride (BF₃) molecules.
Worked Solution & Example Answer:Account for the differences in the shapes of the ammonia (NH₃) and boron trifluoride (BF₃) molecules. - Leaving Cert Chemistry - Question b - 2004
Step 1
Ammonia (NH₃) Shape
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Answer
Ammonia (NH₃) has three bond pairs and one lone pair of electrons. The presence of the lone pair repels the bond pairs, resulting in a trigonal pyramidal shape. The bond angle in ammonia is approximately 107 degrees.
Step 2
Boron Trifluoride (BF₃) Shape
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Answer
Boron trifluoride (BF₃) has three bond pairs and no lone pairs. This arrangement leads to a trigonal planar shape with bond angles of approximately 120 degrees. The lack of a lone pair allows for a more symmetrical shape compared to ammonia.
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