What is the formula for the simplest stable compound formed between fluorine and nitrogen?

Answer 1

NF3 is a relatively stable compound that is available commercially in a liquid form. It is not flammable but it is a strong oxidizing agent and very reactive.

Because the Fluorine atoms are small, there is not the stress buildup in the NF3 solid crystals like there is in Nitrogen Triiode, which is very unstable and spontaneously decomposes into Nitrogen gas and Iodine vapor.

Answer 2

The molecular formula is N2F2. to unravel this difficulty, we ought to constantly first assume which you have one hundred g of substance. 40 two% of that's nitrogen, and something is fluorine. having suggested that, we've 40 two g N and fifty 8 g F (bear in mind: one hundred g - 40 two g = fifty 8 g F) recent interior the pattern. we desire this information in determining the empirical formula. After determining the empirical formula, we are able to be certain the molecular formula from it. What we do now's to transform 40 two g N and fifty 8 g F to moles by applying dividing each and each by applying their molar hundreds. bear in mind right here that N and F exist in atomic form, no longer diatomic (molecular) form. 40 two g N * a million mol N / 14 g N = 3.00 mol N fifty 8 g F * a million mol F / 19 g F = 3.05 mol F Then, divide each and each volume by applying the smaller form of moles. 3.00 mol N / 3 = a million 3.05 mol F / 3 = a million.01 = a million The empirical formula is subsequently NF (use those values above via fact the subscripts of the respective aspects). We now be certain the molar mass of the compound, as you're able to be certain the molar mass of alternative compounds. The molar mass of the compound is 33 g/mol. Then, we be certain the subscripts of the molecular formula by applying dividing the molar mass of the genuinely compound by applying the empirical formula mass (the only we computed until now). molecular formula = molar mass / empirical formula mass = sixty six g/mol / 33 g/mol = 2 We multiply this huge form by applying the subscripts of the empirical formula to get the molecular formula. 2(NF) = N2F2 :)

Answer 3

NF3