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Of the following molecules, which do not have permanent dipole moment?
- a)SiF4
- b)BF3
- c)PF3
- d)PF5
Correct answer is option 'A,B,D'. Can you explain this answer?
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Most Upvoted Answer
Of the following molecules, which do not have permanent dipole moment?...
Permanent dipole means basically polar molecule.. one end has partial negative and other has partial negative kind of thing... except option 3 all other molecules dipole are exactly balanced by Oppositively bonded atom... so it basically act as non polar (non permanent dipole) , in PF3 it has unequal distribution of electron density...so it is polar (permanent dipole molecule)
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Community Answer
Of the following molecules, which do not have permanent dipole moment?...
Explanation:
Permanent dipole moment:
A permanent dipole moment occurs when a molecule has a separation of positive and negative charges, creating a permanent imbalance of electron density. This imbalance results in a polar molecule with a dipole moment.
SiF4:
Silicon tetrafluoride (SiF4) has a tetrahedral molecular geometry. In this molecule, the Si-F bonds are polar due to the difference in electronegativity between silicon and fluorine. However, the dipole moments of the individual bonds cancel out each other due to the symmetric arrangement of the four fluorine atoms around the central silicon atom. As a result, the molecule as a whole has no net dipole moment and is nonpolar.
BF3:
Boron trifluoride (BF3) has a trigonal planar molecular geometry. The boron-fluorine bonds are polar due to the difference in electronegativity between boron and fluorine. However, the three polar bonds are symmetrically arranged around the central boron atom, resulting in the cancellation of dipole moments. Therefore, BF3 has no net dipole moment and is nonpolar.
PF3:
Phosphorus trifluoride (PF3) has a trigonal pyramidal molecular geometry. The phosphorus-fluorine bonds are polar due to the difference in electronegativity between phosphorus and fluorine. The molecule has a net dipole moment because the three polar bonds do not cancel out each other. Therefore, PF3 is a polar molecule with a permanent dipole moment.
PF5:
Phosphorus pentafluoride (PF5) has a trigonal bipyramidal molecular geometry. The five phosphorus-fluorine bonds are polar due to the difference in electronegativity between phosphorus and fluorine. However, the molecule has a symmetric arrangement, and the dipole moments of the five bonds cancel out each other. Therefore, PF5 has no net dipole moment and is nonpolar.
Summary:
- SiF4, BF3, and PF5 do not have a permanent dipole moment because the dipole moments of the polar bonds cancel out each other due to the symmetric arrangement of the atoms.
- PF3 has a permanent dipole moment because the dipole moments of the polar bonds do not cancel out, resulting in a net dipole moment.
Permanent dipole moment:
A permanent dipole moment occurs when a molecule has a separation of positive and negative charges, creating a permanent imbalance of electron density. This imbalance results in a polar molecule with a dipole moment.
SiF4:
Silicon tetrafluoride (SiF4) has a tetrahedral molecular geometry. In this molecule, the Si-F bonds are polar due to the difference in electronegativity between silicon and fluorine. However, the dipole moments of the individual bonds cancel out each other due to the symmetric arrangement of the four fluorine atoms around the central silicon atom. As a result, the molecule as a whole has no net dipole moment and is nonpolar.
BF3:
Boron trifluoride (BF3) has a trigonal planar molecular geometry. The boron-fluorine bonds are polar due to the difference in electronegativity between boron and fluorine. However, the three polar bonds are symmetrically arranged around the central boron atom, resulting in the cancellation of dipole moments. Therefore, BF3 has no net dipole moment and is nonpolar.
PF3:
Phosphorus trifluoride (PF3) has a trigonal pyramidal molecular geometry. The phosphorus-fluorine bonds are polar due to the difference in electronegativity between phosphorus and fluorine. The molecule has a net dipole moment because the three polar bonds do not cancel out each other. Therefore, PF3 is a polar molecule with a permanent dipole moment.
PF5:
Phosphorus pentafluoride (PF5) has a trigonal bipyramidal molecular geometry. The five phosphorus-fluorine bonds are polar due to the difference in electronegativity between phosphorus and fluorine. However, the molecule has a symmetric arrangement, and the dipole moments of the five bonds cancel out each other. Therefore, PF5 has no net dipole moment and is nonpolar.
Summary:
- SiF4, BF3, and PF5 do not have a permanent dipole moment because the dipole moments of the polar bonds cancel out each other due to the symmetric arrangement of the atoms.
- PF3 has a permanent dipole moment because the dipole moments of the polar bonds do not cancel out, resulting in a net dipole moment.
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Of the following molecules, which do not have permanent dipole moment?a)SiF4b)BF3c)PF3d)PF5Correct answer is option 'A,B,D'. Can you explain this answer?
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