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  • Created by: Jordan
  • Created on: 19-03-11 01:06

1. Atoms and Electron Structure


Isotopes                                    atoms of an element with different numbers of neutrons and different masses


Relative atomic mass                  average mass of an atom relative to 1/12 of the mass of a carbon-12 atom


Relative isotopic mass                mass of a particular isotope relative to 1/12 of the mass of a carbon-12 atom


Orbital                                      a region that can hold up to 2 electrons with opposite spins


1st ionisation energy                   energy change when one mole of electrons is removed from one mole of gaseous atoms


Successive ionisation energy       energy change when one mole of electrons is removed from one mole of gaseous positively charged ions

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2. Equations and acids


Acid                                          proton donor (H+ donor)


Base                                         proton acceptor (H+ acceptor)


Salt                                           produced when the H+ of an acid is replaced by another positive ion


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3. Redox


Oxidation                                   loss of electrons or increase in oxidation number


Reduction                                  gain of electrons or decrease in oxidation number


Disproportionation                      a reaction in which an element is simultaneously oxidised and reduced

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4. Moles and Equations


Amount of substance                  the number of moles of substance that you have


Mole                                         unit for amount of substance


Avogadro constant, NA                number of particles present in a mole (6.02 x 1023 mol-1)


Empirical formula                       simplest whole number ratio of the atoms of each element in a compound


Molecular formula                      actual number of atoms of each element in a molecule


Concentrated                             containing a large amount of solute per dm3

(say 10 mol dm-3 or more)


Dilute                                        containing a small amount of solute per dm3

(say 2 mol dm-3 or less)

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5. Bonding and Structure


Ionic bond                                 electrostatic attraction between oppositely charged ions


Covalent bond                            a shared pair of electrons


Metallic bond                             attraction between positive ions and delocalised electrons


Electronegativity                        ability of an atom to attract the electrons in a covalent bond


Hydrogen bond                          attraction between a lone pair and a hydrogen atom attached to O, N or F


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6. The Periodic Table



Periodicity                                 patterns repeated across different periods (rows of the Periodic Table)



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gabriella PAOLONI

simple and effective


these are way too simplified...


You should use the glossary in the back of the textbook, it has the actual definitions as they appear on the mark scheme


Does any1 have the mark scheme for f321 jan 2011?

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