Okay for each of these molecules will draw the Louis structure and then determine the expected high hybrid orbital's that will be used for bonding around the central Adam and then predict whether or not these molecules are polar. For the 1st 1 will draw the Louis structure and recognize that it is a symmetrical molecule with the tetra he'd RL geometry. Therefore, it will not be polar. The bond angles will be about 109.5 degrees on the central atom will be SP three hybridized, and we'll go to nitrogen tri fluoride nitrogen Tri Fluoride has the Tetra Hydro electron group geometry, but the molecular geometry with one of them being a lone pair, is going to be tribunal parameter. The bond angles will be something just under 100 9.5 degrees, and the molecule will be polar because all of the nitrogen flooring bond polarities do not cancel because it's not. All of the electron groups are the nitrogen flooring bonds, so they're polarities. Don't it's not symmetrical in their polarities. Don't cancel. Then we look at oxygen die fluoride and we see therefore electron groups around oxygen. Two of them are bonding So this is bent it something just under 100 9.5 degrees. And because it's bent, the bond polarities of oxygen and flooring do not cancel. So it's polar and we'll move on to boron. Try fluoride and with boron, try fluoride. We see that there are only three electron groups around boron. It only has six valence electrons, but boron is one of the exceptions, or six valence. Electrons for some molecules is acceptable, so this is triggered plainer at 120 degrees SB two hybridized. And because of the cemetery, all of the boron flooring bond polarity is cancel so the molecule is non polar. Then we go to brilliant with two hydrogen beryllium only has four valence electrons surrounding it to electron groups. Brilliant is another one of the exceptions where some molecules of beryllium are fine, with just four valence electrons surrounding it. This would be one of them, so the molecule, then with only two electron groups, is linear at 180 degrees, and it has SP hybridization around beryllium, and because of the cemetery, the molecule is non polar. Then we look at trillium, 10 tra fluoride and we end up placing another lone pair around Trillium because we have the an extra set of electrons. That extra set of electrons typically is placed around the central Adam. So now we have five electron groups around the central Adam, with by electron groups around the central Adam, one of them being a lone pair. This has a seaside geometry. There's actually two bond angles. One is 120 degrees, the other is 90 degrees. If you go back and review the seesaw geometry with five electron groups around the central Adam, this is DSP three hybridized molecules, not symmetrical, although all the bonds are the trillium flooring bonds because it's not symmetrical, molecule is polar. Okay, then, for the next one, we've got our snick pent of fluoride. If we take all the valence electrons that are available to us, we'll see that, um, arsenic is just going to have five bonding group surrounding it. Five funding groups correspond to a tribunal by parameter all geometry with bond angles of 120 90 degrees, a dsp three hybridization, and because of the cemetery of the molecule, this molecule is also non polar. Okay for the next one. Then we've got Krypton. Die fluoride. Dr. Lewis, Structure will end up with, um, three lone pairs around Krypton after bonding to two different floor Eames. The electron group geometry then is trickle by parameter, but with three of them being lone pairs, the molecules actually linear with bond angle, a bond angle of 180 degrees. The five electron groups that give it the tribunal by parameter electron group geometry results in a DSP three hybridization. But because this molecule is linear, the cemetery allows the polarities to cancel on. This is a non polar molecule. Well, then go to create krypton. Tetra fluoride crypt on tetra fluoride ends up having two lone pairs around Krypton after bonding to four floor rains. So we do have six electron group surrounding crypt krypton, resulting in a de two sp three hybridization because two of them are lone pairs. The geometry is square, plainer, with bond angles of 90 degrees, and with a perfectly square plainer molecule than the bond. Polarities will cancel because of this perfect square plane geometry, so the molecule would be non polar. Then we'll go to a selenium hexafluoride and selenium hexafluoride We just have six Loreen surrounding selenium, all of them being bonded to its. We have six bonding groups. This is an optical federal geometry at 90 degrees for all bond angles. DSP three hybridized. And because we have a perfect octave Futural structure where all the bonds are exactly the same. Sliney and flooring bonds this is a non polar molecule on. We have iodine Penta fluoride, so we've got five I Florian's bonded to iodine. After we finished the Louis structure, there's no there's one extra pair of electrons that we will add to the iodine central Adam giving us six electron group surrounding the iodine. One of them is a lone pair, so the molecular geometry ends up being square parameter. All all bond angles are 90 degrees, approximately 90 degrees and the hybridization with six electron groups five bombed in one lone pair would be de two sp three and we lost that perfect doctor huge RL geometry because we introduced one of lone pairs. So the bond polarity is Do not cancel in. This is a polar molecule. The last one is I dying. Try fluoride after we complete the octet for all the floor Eanes. There's two more pairs of electrons that we place on iodine. We now have five electron group surrounding iodine, three bonding, two lone pairs, so the geometry then ends up being T shaped. All bond angles there, approximately 90 degrees with five electron groups. Hybridization is DSP three, and because of the T shape, the geometry results in a polar molecule.