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Stack #4615675
| Term | Definition |
|---|---|
| empirical formula | the lowest whole number ratio for atoms in a compound |
| grams per mole | the unit for molar mass |
| hydrate | an ionic compound that has water molecules associated with its crystal lattice |
| moles | "all roads lead through __" |
| molar mass | the mass of one mole of a substance |
| atom | the smallest unit of an element |
| molecular formula | a whole-number multiple of an empirical- the true formula of a covalent compound |
| carbon-12 | the isotope that molar mass and the atomic mass unit are based on |
| conversion factor | a ratio that can be inverted- used to make conversions |
| percent composition | the numerical description of the chemical makeup of a compound based on mass |
| desiccant | a chemical that absorbs water vapor from its surroundings- often used in packaging of moisture-sensitive items |
| atomic mass unit | the unit used to mass atoms |
| avogadro's number | another name for the mole |
| molecule | the smallest unit of a covalent compound |
| formula unit | the lowest whole number ratio of ions in an ionic compound |
| mole | 6.022 x 10^23 particle represent a __ of particles |
| grams | to convert % composition data to an empirical formula, we can assume that 100% = 100 __ |
| anhydrous | an adjective that describes hydrates that have had all waters if hydration driven away |
| % -> grams then x by 1 mol/mass then divide by smallest | empirical formula from % |
| x each element by their mass then add together for total, then divide that by given molar mass. approx. answer should then be x by the empirical formula | molecular formula from empirical formula and molar mass |
| given atoms x mol/ Avogadro then x by mass of compound/ 1 mol | mass from atoms |
| x each element by their mass (make sure to x any subscripts) then add them for total. then divide each element's mass by the total mass and x by 100 | percent composition of compound |
| subtract for mass H2O then x that number by 1 mol/ mass of compound or element. then divide the two answers. then finish by naming using greek prefix | hydrate from data |
| % of each element x 1 mol/atomic mass. then divide by smallest. after that add all of the answers you got from x-ing and divide by the given molar mass | molecular formula from % |
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