Atomic masses
- Created by: Andrei stephen
- Created on: 07-10-13 16:34
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- Atomic masses
- relative atomic/ isotomic mass
- the mass of an atom of an element /isotope compeared to the mass of 1/12 of carbon 12
- relative abundance
- (reltive abundance x isotope) + (reltive abundance x isotope)/100
- e.g (75 x 35)+(25 x 37)/100 = 35Cl
- (reltive abundance x isotope) + (reltive abundance x isotope)/100
- relative molecular mass the Mr is the weight mass of an molecule compared to 1/12 of the mass of carbon
- relative formulae mass = the Mr of all the molecules added together
- formulae
- mass/no of mols = relative atomic mass
- mass/relative atomic mass = no of mols
- no of mols x Mr = mass
- concentration x volume/ 1000 = no of mols in dm3 or without the 1000 if volume already in Dm3
- volume = no of moles / volume
- concentration = no of moles/ concentration
- empirical formulae= first do M/Mr then apply this ratio you get to the elements you have to get the empirical formulae
- empirical formulae the lowest no ratio of elements in a substance
- acids and bases
- acid= is a spices that is a proton doner = H+
- ate(with oxygen) ide (without oxygen)
- cation = +ive anion= -ive
- relative atomic/ isotomic mass
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