The Dipole Moment of Barium Floride is zero but Dipole Moment of Nitrogen Floride is not zero.Why?
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Answers
Molecules that are polar have two attributes:
They contain polar bonds (ie. electronegativity difference between the atoms in the bond of about >0.4 depending on your source)They are asymmetrical in geometry
NF3 is trigonal pyramidal in shape. This is because N requires 4 electron pairs to fulfil its octet.
BF3 is different. It is trigonal planar in shape, because it only requires 3 electron pairs to fulfil its octet. This is because there are only three electrons available for bonding (one unpaired electron per fluoride and three valence electrons total on the boron). In the case of NF3, nitrogen has 5 valence electrons, so when it forms bonds three bonds with the fluorides, a lone pair occupies another space, causing the bonds to bend onwards and resulting in a trigonal pyramidal shape.
The bonds in NF3 are polar, because there in a difference in electronegativity of 1.0. Although the bonds in BF3 are more polar, with a difference of 2.0, the trigonal planar shape is symmetrical, and the electronegativity differences cancel out. Because BF3 doesn't meet both requirements of polar molecules, it is considered non-polar.
Answer:
NF3 (nitrogen trifluoride) is the polar molecule in this case. BF3 (boron trifluoride) is non-polar.
Molecules that are polar have two attributes:
They contain polar bonds (ie. electronegativity difference between the atoms in the bond of about >0.4 depending on your source)They are asymmetrical in geometry
NF3 is trigonal pyramidal in shape. This is because N requires 4 electron pairs to fulfil its octet.
BF3 is different. It is trigonal planar in shape, because it only requires 3 electron pairs to fulfil its octet. This is because there are only three electrons available for bonding (one unpaired electron per fluoride and three valence electrons total on the boron). In the case of NF3, nitrogen has 5 valence electrons, so when it forms bonds three bonds with the fluorides, a lone pair occupies another space, causing the bonds to bend onwards and resulting in a trigonal pyramidal shape.
The bonds in NF3 are polar, because there in a difference in electronegativity of 1.0. Although the bonds in BF3 are more polar, with a difference of 2.0, the trigonal planar shape is symmetrical, and the electronegativity differences cancel out. Because BF3 doesn't meet both requirements of polar molecules, it is considered non-polar.
Explanation:
NF3 (nitrogen trifluoride) is the polar molecule in this case. BF3 (boron trifluoride) is non-polar.
Molecules that are polar have two attributes:
They contain polar bonds (ie. electronegativity difference between the atoms in the bond of about >0.4 depending on your source)They are asymmetrical in geometry
NF3 is trigonal pyramidal in shape. This is because N requires 4 electron pairs to fulfil its octet.
BF3 is different. It is trigonal planar in shape, because it only requires 3 electron pairs to fulfil its octet. This is because there are only three electrons available for bonding (one unpaired electron per fluoride and three valence electrons total on the boron). In the case of NF3, nitrogen has 5 valence electrons, so when it forms bonds three bonds with the fluorides, a lone pair occupies another space, causing the bonds to bend onwards and resulting in a trigonal pyramidal shape.
The bonds in NF3 are polar, because there in a difference in electronegativity of 1.0. Although the bonds in BF3 are more polar, with a difference of 2.0, the trigonal planar shape is symmetrical, and the electronegativity differences cancel out. Because BF3 doesn't meet both requirements of polar molecules, it is considered non-polar.