Honors Chemistry A - Unit 6 (Extra Notes/Resources!)

geez louise there’s a lot of stuff this unit, let’s speed through it all

percent composition is just the percentage of a certain element in a compound
it’s like saying “oh yah that compound is 20% iron” or “bella’s diet is 95% smarties”
steps:
1. find mass of the element ur finding the percent of (and don’t forget to multiply by number of atoms there are, or if its a BrINClHOF element)
2. find total mass of compound
3. plug into the formula! divide the mass of the element by the total mass of the compound, then multiply by 100 to get a percentage!
vid: https://www.youtube.com/watch?v=JqKEaPmNFLg&list=PLytGGifnD9dUom302biLWWGuTxg7lgI7P&index=11

dimensional analysis is using fractions to turn one unit of measurement to another
you take your starting unit, then multiply it by another fraction with the new unit of measurement on top, and the one you want to cancel out on the bottom

example problem: A compound is 71.65% chlorine, 24.27% carbon, and 4.07% hydrogen. What is the empirical formula of the compound?

Convert %’s into grams (if the question already gives the info in grams, skip this step)
71.65% Cl → 71.65 g Cl
24.27% C → 24.27 g C
4.07% H → 4.07 g H
Convert grams to moles
now divide alll the numbers by the the smallest number of moles
if the numbers aren’t whole, multiply them so they’re whole, we don’t do decimals here
and voila, the numbers u got are now the subscripts for the elements!

we’re gonna go off the last question from above^, cuz that’s how it’ll be formatted on the test

so: If the molar mass of the previous compound (CH2Cl) is 148.41 g, what is the molecular formula?

find total mass of empirical formula
divide molar mass by empirical mass
148.41 / 49.48 = 3
take that number ^, and multiply all the subscripts of the empirical formula by it, and bada bam boom, you have molecular formula
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