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Empirical numbers have to contain whole numbers since you can't have a fraction of an atom. Therefore, if you get nonwhole numbers in your conversation to the empirical formula, multiple the ratios by whole numbers until your product is close to the nearest whole number!
When calculating empirical formulas, you will have to have them as whole numbers. Thus, when calculating empirical formulas, you would have to multiply every single element in a way that gets rid of any fraction.
All empirical formulas need to be in whole numbers. However, keep in mind that they should also be reduced to the lowest possible whole numbers as well, meaning that the numbers don't all share a common factor.
I agree with what was said, if you end up with a fraction in your empirical formula, multiply it by whatever number gets the fraction to a whole number. Then don't forget to multiply all of your other numbers in the empirical formula by that same value to make sure everything is equal.
Empirical formulas do need to be whole numbers as you cannot have a fraction of an atom. That is why we multiply to get a whole number ratio (ex. 1.5x2=3) but it is key to make sure that it is in its lowest whole number ratio, otherwise it will be considered a molecular formula.
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