i)XeOF4

In order to be able to determine the molecular geometry of xenon oxytetrafluoride,

XeOF4, you need to start by drawing its Lewis structure.

To find the number of valence electron you get in one molecule of xenon oxytetrafluoride, add the number of valence electrons of each individual atom that makes up the molecule.

So, xenon oxytetrafluoride will have a total of

42 valence electrons 8 valence electrons are coming from the xenon atom 6 valence electrons are coming from the oxygen atom 7 valence electrons from each of the four fluorine atoms.

Now, xenon will be the central atom. It will bond with the oxygen atom via a double bond. This will ensure that oxygen has a complete octet.

The xenon atom will bond with the four fluorine atoms via four single bonds, which will ensure that each of the four fluorine atoms gets a complete octet. Afterwards the xenon atom will make double bond with oxygen atom to fulfill its octet. The remaining two electrons will remain as a lone pair.

Typically, N–N bonds are similar in length to that inhydrazine(145 pm). Dinitrogen trioxide, however, has an unusually long N–N bond at 186 pm. Some other nitrogen oxides do also possess long N–N bonds, including dinitrogen tetroxide (175 pm). The N2O3molecule is planar and exhibits Cs symmetry. The dimensions displayed below come from microwave spectroscopy of low-temperature, gaseous N2O3

Based on VSEPR Theory (Valence Shell Electron Pair Repulsion Theory) the electron clouds on atoms and lone pairs of electrons around the O will repel each other. As a result they will be pushed apart giving theOF2molecule a bentgeometryorshape.