Xenon forms xenon hexafluoride, XeF6
Yes. it has a pseudo octahedral geometry in XeF6
Use the Ideal Gas Law: PV=nRT (pressure times volume equals moles times the ideal gas constant of 0.082 times the Kelvin temperature.) First, convert 25 Celsius to Kelvin: 25+273=298. Next, find out how many moles is in 25.0g of XeF6: 1(Xe)+6(F)=1(131.3)+6(19)=245g/mol; 25g XeF6=0.102mol. Then, plug it all in and solve for the pressure, which is your unknown: P(5L)=0.102mol(0.082)(298kelvins) Simplify: 5P=2.4925, P=0.4985, or approximately 0.5 atm of pressure.
Noble gases are generally chemically as they have completely filled orbitals. So any compound by xenon as in XeF2, XeF4, XeF6, XeOF4 etc are unusual.
The bonding in Mo(CN)84- anion as been described in terms of sp3d4 hybridisation. The geometry of the hybrid bonds is "dodecahedral". The use of hybridisation to describe the bonding in transition metal complexes is very old school and other metods are generally used nowadays. There are some horrible pictures of this geometry on the web, try googling books for pictures.
The chemical formula XeF6 is for xenon hexafluoride.
XeF6.
sp3d2
sp3d3
xeonon hexafluoride
i pretty sure there's only 1 pair of electrons on XeF6
It is not practically confirmed but theoritically XeF6 has either Pentagonal bipyramidal structure or Distorted octahedral structure.
XeF6
ionic
Xenon Hexafluorid
Six.
The answer depends on the quantity of XeF6