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Chemistry Unit 2
| Question | Answer |
|---|---|
| percent composition steps | 1) multiply the quantity of each type of atom by the average atomic mass 2) add each of those totals together to get the formula weight 3) divide the number you got for a type of atom by the formula weight 4) multiply answer by 100 |
| Avogadro's number | 6.022 x 10^23 (mole) |
| average atomic mass number (amu) molar mass number (grams) | bottom number in square of element on periodic table |
| formula for converting moles to grams | # of moles given average atomic mass -------------------- = ---------------------------- 1 1 mol of element |
| formula for converting numbers of moles to number of atoms | # of moles x (6.022 x 10^23) = # of atoms |
| What do you do when you see a percentage? | Turn it into grams (i.e. 54.3% --> 54.3 grams) |
| formula for converting grams to moles for an element | # of grams given 1 mol of element -------------------- = ---------------------------- 1 average atomic mass |
| empirical formula steps | 1) solve formula for converting grams to moles or vice versa (do this for each element in the molecular formula) 2) take the answer from and divide by the smallest molar mass you got out of all the elements. 3) multiply the answers to make whole #s. |
Created by:
zbw
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