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  7. Unit AS 1 - Basic Concepts in Physical and Inorganic Chemistry

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Summary Atomic Structure Notes with Labelled Diagrams
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Detailed Atomic Structure Notes fully typed with labelled diagrams. Combination of revision guides, teachers notes, exam hints and past paper questions. Written with concise layout using the Cornell Method. Notes from an A* student. Whole chapter

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  • April 1, 2021
  • 19
  • 2020/2021
  • Summary

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Atomic
Structure
Chemistry AS1

Year 13

, Atomic Structure - Background Knowledge


John Dalton Theory,1804 – Now Incorrect

 Element is composed of atoms of identical size and mass
(isotopes prove wrong)
 Atoms are invisible and remain unchanged during chemical
reactions (the transfer of electrons proves this wrong)



Bohr-Rutherford Model, 1912 – Most modern

 Central positively-charged nucleus of very high density
 Surrounded by much larger-sized volumes in which electrons
move

Mass Charge Location
Proton 1 +1 Nucleus
Neutron 1 0 Nucleus
Electron 1 -1 Orbital Shells /
1840 Energy Levels


No. of Protons =
Atomic Number




Element
No. of Electrons =
Atomic Number Relative
Atomic Mass
No. of Neutrons = Atomic
RAM – Atomic number Number

No of shells = period number

No of electrons in outer shell = group number


1

, Mass Spectronomy
Determines the mass of atoms and molecules



A MASS SPECTRONOMER atomises and ionises a sample, producing
ions with a single positive charge – ALL ions in a mass spectrum have a
single positive charge

Accelerated by electric field

Magnetic field deflects positive ions

Extent of deflection depends on mass and charge of ion



Altering magnetic field strength brings ions to focus on detector



To work out RAM:

1. Add all the products of the RIM multiplied by its relative abundance
2. Divide by 100


Data obtained can be from:

An Element Spectrum will show masses and relative abundance
for all istopes of element
Data supplied in table or a mass spectrum

Relative Isotopic Mass Relative Abdunance
50 7
52 74
53 15
54 4




2

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