[Tony30]

A compound of chlorine and fluorine, CIFx, reacts at about 75 degrees C with uranium to produce uranium hexafluoride and chlrine fluoride, CIF. A certain amount of uranium produced 5.63 g of uranium hexafluroide and 457 mL of chlorine fluoride at 75 degrees C and 3.00 atm. What is X? Describe the geometry, polarity, and bond angles, of the compound and the hybridization of chlorine. How many sigma and pi bonds are there.

[Arkcon]

Alright.  There are a few things we can do to start working on this problem.  For starters, there are at least 3 different questions, that aren't really related (well, two are kinda related.)  Can you split this question up into blocks of those 3 questions, so it looks less daunting?  And can you start solving the first one?

*[EDIT]*

In a previous, similar question of yours, it's been mentioned that you need a balanced reaction.  That's a little hard, in this case, because the formula contains an X.  But can you try, and then see what you need to do to solve for X?

[Tony30]

CIFx + U = UF6 + ClF.

[Arkcon]

Good.  You've written a chemical formula.  This formula, what are it's units?  And yes, there are units there, sort of hidden, but it may have been mentioned before.   What units are you given for reactants?  And can you convert?

[Tony30]

Well units probably is in STP. Also i figure if i use the amount of Uranium 5.63 g to work backwords. I just need help for the hybridization and how to find what X is

[Arkcon]

Well units probably is in STP.

That wasn't where I was going with the term units.  It's a subtle bit, that chem profs only seem to hint at  -- the balanced chemical reaction is an equation.  That is, it contains, almost, arithmetic operators, this plus this yields this plus this -- correct?  The "units" of a chemical equation are moles.

Also i figure if i use the amount of Uranium 5.63 g to work backwords.

Good work, you realize, you've been given mass, and have to convert to moles, and you know how.  You also know how to use the gas laws, to determine moles.

I just need help for the hybridization and how to find what X is

Well, yeah, until we know what X is, we don't know how many atoms are where, and we won't know the geometry, and we won't know the hybridization.

[Tony30]

So how would i find X that is probably the first step in solving this problem.

[Arkcon]

You will need to balance the equation, same numbers of atoms (moles of reactants) on either side of the arrow.  You've been told how much product in grams of solid and volume of gas at a temperature and pressue, can you convert?

[Donaldson Tan]

To solve this problem, we need de-construct the data provided into solvable simultaneous equations.

A compuond of chlorine and fluorine, CIFx, reacts at about 75 degrees C with uranium to produce uranium hexafluoride and chlrine fluoride, CIF.

This is an unbalanced equation: ClF_x + U -> UF₆ + ClF

We have to balance it first: ClF_x + y.U -> y.UF₆ + ClF
=> x = 6y + 1
=> we need 1 more independent equation to solve this problem.

A certain amount of uranium produced 5.63 g of uranium hexafluroide and 457 mL of chlorine fluoride at 75 degrees C and 3.00 atm.

This data here would provide us the means to calculate the various mole ratio of reactant to reactant and reactant to product. This mole ratio would be the source of our 2nd independent equation.

molar mass of UF₆ = 238.03 + 6*19.00 = 352.03 g/mol
number of moles of UF₆ formed = mass / (molar mass) = 5.63 / 352.03 = 0.01599 = 0.016 moles

assuming perfect gas,
number of moles of ClF formed = (P*V)/ (R*T) = (3.03975*10⁵ Pa * 0.000457 m³) / (8.314 J.mol^-1.K^-1 * 348 K) = 0.048 moles

Given that the molar ratio of UF₆ to ClF is y:1, then
y = (number of moles of UF₆ formed) / (number of moles of ClF formed) = 0.016/0.048 = 1/3
x = 6y + 1 = 3

Describe the geometry, polarity, and bond angles, of the compound and the hybridization of chlorine. How many sigma and pi bonds are there.

Don't forget to consider the lone pairs and the bonding pair of electrons on Chlorine's valence shell to evaluate the state of Chlorine's hybridisation.