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    Hey ppl

    Just thought that Id type out the notes I ve just remembered so it wud test me and also be useful to others???? Check em also plz?

    Structural Isomerism: When the molecular formula is the same but the structural arrangement isn't.

    Stereoisomerism: When the molecular formula is the same but the arrangement of atoms is space differs.

    Transition Metals: Very small and densely charged Attract Ligands ( molecules or ions which bind onto non metals....by forming dative covalent bonds) which the form complex ions ( these are when the central metal ion is surrounded by ligands.

    Ligands: Usually NH3, H20 AND CL

    when NH3 and H2O they form octahedral shaped ions which also have the coordinate number 6.....but Cl which is smaller than H20 then only 4 are used...this forms a tetrahedral structure...with the coordinate number 4.....

    When ligand exchange reactions take place they usually dont change number (coordinate) but when exchange reaction takes place between Cl then they shape and number changes.

    Transition Metals also change their Oxidation states by gaining/loosing electrons thats is why they are useful catalysts...e.g Nickel....

    For moving up Oxidation states then use H202 in alkali solution but if moving down use Zinc/HCL.

    Hope it Helps!
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    (Original post by Bond007)
    Hey ppl

    Transition Metals: Very small and densely charged Attract Ligands ( molecules or ions which bind onto non metals....by forming dative covalent bonds) which the form complex ions ( these are when the central metal ion is surrounded by ligands.

    Ligands: Usually NH3, H20 AND CL

    when NH3 and H2O they form octahedral shaped ions which also have the coordinate number 6.....but Cl which is smaller than H20 then only 4 are used...this forms a tetrahedral structure...with the coordinate number 4.....
    Cl is larger than H2O isnt it??
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    yes much larger, and that is why it only forms 4 dative bonds and not 6!
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    lol sorry typing error.......was typing too fast too notice.....
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    just correcting you like you asked us to, no need to be sorry
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    Although most transition metals are pretty dense, that isnt really a definition and there are more important common properties (i realise that you put it cos it was before the 'attracting ligands' bit, but I thought id add to it neway;

    Definition; form one or more stable ions which has an incomplete d sub-shell

    Common properties;form coloured ions and precipitates, usually have many (stable) oxidation states
 
 
 
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