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21 Cards in this Set
- Front
- Back
Element |
Substance made up of only one kind of atom and cant be broken down further into a simpler substance by chemical means |
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Atom |
Smallest particle of an element that can take part in a chemical reaction |
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Mixture |
Substances made up of two or more elements not chemically combined |
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Compound |
Substance made up of two or more elements that are chemically combined |
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Isotope |
Atom of the same element with the same number of protons and electrons but different number of neutrons |
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Relative Atomic Mass |
The weighted average mass of all natural known isotopes of an element compared with C12 where one atom C12 has a mass up exactly 12 units |
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Relative Isotopic Mass |
The mass of a particular isotope of an element compared with C12 where one atom of C12 has a mass of exactly 12 units |
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Rlative Molecular Mass |
Weighted average mass of 1 molecule of a compound compared with C12 where one atom of C12 has a mass of exactly 12 units |
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Relative Formula Mass |
The weighted average mass of the formula of a compound compared with C12 where 1 atom of C12 has a mass of exactly 12 units |
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The Mole |
Amount of substance in grams which has the same number of particles as there are in 12 grams of Carbon |
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Avagadro's Constant |
Number of atoms, ions, molecules or electrons in a mole = 6.023x10^23 (atoms) |
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Mass and Moles Formula |
Moles = Mass of substance (g) / Molecular mass (Mr) |
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Dm^3 to cm^3 |
1 dm^3 = 1000 cm^3 |
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Gas and Moles |
Moles = Volume of gas (dm^3) / Molar mass (24) |
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Concentration (g/dm^3) |
Concentration = Mass (g) / Volume (dm^3) |
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Concentration (mol/dm^3) |
Concentration = moles / Volume (dm^3) |
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Percentage Yield (%) |
Percentage yeild = [ Amount you make (measured) / Maximum amount (calculated) ] x100 |
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Ar From a Mass Spectra Diagram |
Ar = mass x relative abundance / 100 |
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Empirical Formula |
Simplest whole number ratio of the elements present in 1 molecule of a compound |
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Molecular Formula Def. |
Total number of atoms present in each element in a molecule |
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Molecular Formula |
Molecular formula = n(Empirical Formula) n = molecular mass (given) / molecular mass of Empirical formula |