Is SCl4 polar or non polar?

Answer 1

SCl4 is a polar molecule because when the shape is taken into consideration it is a tetrahedral electron shape, with two lone pairs, making it a trigonal pyramidal. You then know the dipoles do not cancel out because they work together to pull in a direction, not aqgainst each other, and since Cl and S are different electronegativities, they do not cancel out, if it were a F-F type bond electronegativity would cancel out, causing it to be nonplar.

Answer 2

It is polar.

Polarity suggests a net-density of electrons existing more toward one side of a molecule than the other.

For example, CO2. The structure exists like O=C=O. Where are the electrons? Well Oxygen is more electronegative than Carbon so more electron density will be on the Oxygens. However the molecule is symmetrical, we have an Oxygen on each side. No point on this molecule has more electron density than the point opposite to it. So it is not polar.

Another way to look at it is that it is polar but only equally polar in opposing directions, meaning it cancels out. It has a net dipole moment of zero.

Meanwhile, SiHCl3 is Silicon with 4 substituents. Silicon has 4 valence electrons and so our chemistry knowledge tells us this molecule is tetrahedral. But not all of the substituents are equal. Chlorine is far more electronegative than Hydrogen is, so the electron density will be higher on the Chlorines than on the hydrogen atom, creating a non-zero net dipole moment, hence it is polar.

This is similar to if we had S=C=O (Carbonyl sulfide). Unlike O=C=O, Carbonyl sulfide is not symmetrical and does have a net dipole moment, hence again being polar.

Answer 3

SiCl4 or silicon tetrachloride is a non-polar molecule. It is used in a variety of ways, but mainly in the production of very pure silicon.

Answer 4

sicl4 is non polar the reason is that all the vector of dipole movement are cancel out and polarity is zero.

Answer 5

SiCl4 is nonpolar