Exam 4
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Atomic mass unit amu | Small unit used to describe the mass of an atom.
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| Average atomic mass | It means that any sample of C can be treated as it were made up of identical carbon atoms.
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| Mole | Unit use to measure the amount of a chemical substance.
It helps to convert from particles to mass of a substance.
The number of atoms present in 12.01 g of C
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| Avogandro's number | One mole of something is 6.022 x 10^23 units of that substance.(Symbol N)
Ex. A mole of water is 6.022 x 10^23 H2O molecules.
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| Molar mass/ Molecular weigh | T: Sum of the atomic masses of each element in a formula
B: The mass of 1 mol of the substance (g)
(MM)... Remember diatomic elements and count 2 times.
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| Formula weight | Sometimes used to name the molar mass for ionic compounds like NaCl.
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| Percent composition | Gives the mass % of each element in a substance.
Formula: Divide the total mass of an element by the total mass of the molecule and then multiply by 100.
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| Empirical Formula (Simplest formula) | The smallest whole-number ratio of elements in a formula. Can be the same for various compounds.
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| Molecular Formula | T: multiple of the empirical formula.
B: Gives the composition of the molecules that are present in a compound(Without simplifying).
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