00:01
Hello everyone, let's start the question.
00:03
In this question, in the first part, we are asked to draw the correct lewis structure for the two molecules given.
00:12
One is sf4 and the other one is sf6.
00:16
So if we first draw the lewis structure for the first compounds, that is sf4, it can be drawn in this manner by taking sulfur as a central atom to which four fluorine that is the side atoms are attached and they are arranged in an asymmetric pattern across the central atoms.
00:42
And each fluorine has three lone pairs available which are arranged in this manner.
00:53
So this is the structure for sf4.
00:59
This fluorine is slightly tilted making the arrangement asymmetric.
01:05
Asymmetric and now if we come to sf6 in this case also sulper has one lone pair and if we talk of sf6 here also sulfur is in center that is the central atom and six fluorine are arranged in this manner symmetrically basically around the central atom which is sulfur and each fluorine atom has three loan pairs available which are arranged like this as depicted in the lowest structure for the aesthetic compound so now we're also asked to write the shape of each of the compounds if we talk about the shape of the first compound that is sf4 it is trigonal bipyramidal trigonial by pyramidal and for sf6, the shape is octahedral.
02:21
The geometry is.
02:22
Now let's consider the second part of the question in which we are being asked that out of the two sf4 or sf6, which one is polar is polar and which one is non -polar...