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How To Use this Booklet:
This booklet has been created by addressing all the points on the OCR B
salters specification for the section, what's in medicine. I advise reading
through the Book, highlighting or underlining words written in ALL
CAPITALS. I also suggest making a spider diagram or mind map to
summarise key points and help the information here stick in your mind. You
could also draw your own images by points on this book that may help you
to remember that point.…read more

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Write out the two half equations and reverse the one with the most negative
standard electrode potential (I.e. swap the reactants on the left with the
products on the right and vice versa)
2) Make the number of electrons in each equation equal via a suitable
multiplication (or division).
3) Add the two equations together (the electrons should cancel out!)
C) Given the necessary information, describe and explain procedures for
acid-base and redox titrations and carry out non-structured calculations
based on the results.…read more

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D) Use and explain the term COORDINATION NUMBER. Draw and name the
shapes of complexes with coordination numbers 4 (tetrahedral and square
planar) and 6 (octahedral).
The coordination number of a complex is the number of bonds that a central
metal atom or ion can form with ligands. I.e. a coordination number of 6 means
the central ion can form 6 bonds meaning it can have a maximum of 6 ligands
attached to it.…read more

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REDOX TITRATIONS (Manganate (VII) titrations): Fill a burette with a
potassium manganate (VII) solution of known concentration. Add a known
volume (measured by volumetric pipette) of substance X to a conical flask. Add
an approximately equal volume of 1 mol dm-3 sulfuric acid to the flask. Titrate
the solution of substance X with manganate (VII) while swirling the flask, until
are within 0.1 cm3 of each other, then take an average.…read more

Page 6

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I) Use standard electrode potentials to:
(i) calculate Ecell
Take away the most negative standard electrode potential from the most
positive. This will ensure that the Ecell value will be positive (as it always must
(ii) Predict the feasibility of redox reactions and understand that the rate of
reaction may be an important factor in deciding whether the reaction
actually takes place under standard conditions.…read more

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K) Describe and Explain approaches to corrosion prevention:
(i) Sacrificial protection by galvanising and use of zinc blocks.
Galvanising means to plate the iron with zinc or another metal which has a
more negative standard electrode potential than iron. This means the zinc will
corrode instead of the iron.
Another way to protect the iron is to weld zinc blocks to it. A cell is set up in
which the zinc corrodes.…read more

Page 8

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M) Give the necessary information, explain the chemical processes occurring
during the extraction and purification of metals from their ores.
N) Recall that the periodic table lists elements in order of atomic number
and groups elements together according to their common properties; recall
the classification of elements into S-, P- and D-blocks.
i) Recall and explain the relationship between the position of an element in
the periodic table and the charge on its ion(s).
Groups 1+2 form ions with a +1 or +2 charge respectively.…read more

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NO3-= Nitrate ion NH4+ = Ammonium ion
SO42- = Sulfate ion HCO3-= Bicarbonate ion (?)
CO32- = Carbonate ion
OH- = Hydroxide ion
O) Recall that transition metals are d-block elements forming one or more
stable ions which have incompletely filled d-orbitals; recall the common
oxidation states of iron and copper and the colours of their aqueous
The only oxidation states I need to know off by heart are those of IRON (2+ and
3+) and COPPER (1+ and 2+).…read more



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