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Q: Which molecule has bonds that are more polar between PF3 and PCl3?
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PCl3 polar or non polar?

PCl3 has a pyramidal geometry, with three polar P-Cl bonds and one lone pair of electrons. Hence the molecule is polar.

BCl3 H2O NH3 and PCl3 which is non-polar?

BCl3 is non-polar. The B-Cl bonds are polar but the molecule is not. You should review shapes of molecules. Valence Shell Electron Pair Repulsion, VSEPR. Applying VSEPR on BCl3, we can find out that the shape of the molecule is trigonal planar. Due to its geometry, the bonds cancel out.

Is scl4i2 a polar molecule?

Yes, it is polar like PCl3, AsCl3 or NCl3.

Is PCl3 polar?


Is Pcl3 an example of ionic bonding?

No, PCL3 bonds covalently. Hope this helps :)

Is PCl3 polor?

It is polar, not polor.

Is PCl6 polar?

PCl3 is polar because it has a lone pair on the P.

Is PCL3 a molecule?

PCl3 is not an atom, it is a molecule that is comprised of one phosphorus atom and three chlorine atoms. If you wish to learn more about it, this is the link to it's wikipedia article Hope that helps

Why PCl3 has a dipole moment and BCl3 does not have a dipole moment?

B forms 3 bonds (has 3 valence electrons) and is sp2 hybridized, so the molecule is trigonal planar, which is symmetrical. P can form 5 bonds (has 5 valence electrons), and in PCl3 has a free electron pair which makes the molecule non-symmetrical.

Is PCl3 an electrolyte?

No, PCl3 has covalent bonds. The difference in electronegativity between P and Cl is not large enough. The electronegativity of P is 2.19 and for Cl it is 3.16, and so the difference is less than one, making it a polar-covalent bond.For more information, see the Related Questions link about how to determine if a bond is non-polar covalent, polar covalent, or ionic.

What is the molecular geometry or shape of phosphorus trichloride (PCl3)?

The phosphorus trichloride (PCl3) has a molecule with a trigonal pyramidal form.

Why is phosphorus trichloride polar?

PCl3 has a trigonal pyramidal molecular geometry, and is, therefore, polar because the dipoles do not cancel.