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2211469
Chemistry - C2.3
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Atomic Structure, Analysis and Quantative Chemistry
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rachaelchandler1
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Resource summary
Chemistry - C2.3
In an Atom the number of protons = number of electrons so atoms have no overall charge
Mass Number = Number of Neutrons + Number of Protons
Number of Neutrons = Mass Number - Atomic Number
Atomic Number = Number of Protons
Isotopes = Atoms of the same element with the same number of protons but a diferent number of neutrons
An example of a isotope is carbon
Relative atomic mass compares the mass of atoms of a elements have different isotopes and is an average value
Is an average value because elements have different isotopes with different mass number
The relative atomic mass is found from a periodic table and is the big number from an element
Mole is the formula mass of a substance in grams
Number of Moles = Mass divided by Molar Mass
Total of each type of element in reactants = Total of each type of element in products
Big numbers placed infront of substances in equations only
Atoms are multiplied by the big number
% yield = (Actual Mass divided by Theoretical Mass) x 100
% yield = percentage of what is produced compared to what should have been produced in theory
Reactants can react in ways that are different to what is expected
Reactions may not go to completion because it is reversible
Some products may be lost when it is seperated
% mass = (Ar x number if elements x 100) divided by Mr
Percentage of an element in a compound is calculated using Ar and Mr
Mr = E (Ar x Number of Atoms)
Relative Formula Mass of compound is the sum of the relative atomic masses of the atoms in the formula
Empirical Formula = simplest whole number ratio of elements in a compound
Use the table to calculate
Write out the formula once you have worked it out
Balanced Symbol Equation used to find masses of any reactants of products
Mole quantaties are used to work out masses of substances in the reaction
Used to work out masses of any substances in the reaction
Use lumpy bicycle or reacting mass equation
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