F321
- Created by: FreyaBee
- Created on: 05-12-12 09:42
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- F321
- Atomic Masses
- Relative isotopic mass = mass of an istope compared with 1/12 mass of carbon-12
- Relative atomic mass (Ar) = The weighted mean mass of an atom of an element compared with 1/12 the mass of carbon-12
- Relative formulamass = weighted mean mass of a formula unit compared with 1/12 Carbon-12
- Relative Molecular Mass (Mr) = Weighted mean mass of a molecule compared with the mass of 1/12 cabon-12
- Moles (n)
- Avagadro's Constant
- The number of atoms per mole of the carbon-12 istotope
- 6.02 x 10^23 mol^-2
- Working out moles
- Gas
- |STP| n=V(in cm3)/22,400
- |RTP| n=V(in cm3)/24,000
- Equal volumes of gases at the same temp and pressure = equal number of molecules
- Solid
- moles = mass/molecular mass
- n=m/M
- Gas
- Amount of any substance containing as many particles as there are carbon atoms in 12g of carbon-12.
- Molar mass (M) = Mass per mole of a substance
- Found by adding together relative atomic masses
- Molar mass (M) = Mass per mole of a substance
- Avagadro's Constant
- Formulas
- Empirical formula
- Smallest whole number ratio of atoms of each element present in a compound
- Always used for compounds with giant structures
- Found by dividing by smallest value
- Molecular Formula
- Actual number of atoms of each element in a molecule
- Molecules
- small group of atoms held together by covalent bonds
- Empirical formula
- Atomic Masses
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