STD 10





                              രസതന്ത്രം
സംക്രമണമൂലകങ്ങളുടെ നിറങ്ങൾ

colors of Fe(II) Hydroxide-white with greenish tinge
               Fe(III)Hydroxide-brown/reddish brown
               Fe(III)sulphateFe2(SO4)3-yellow
The second tube from the
left has almost pure
 whitish iron(II) hydroxide.
                CuCl2- green
               CuCl- white
               

Name
Formula
Color
Picture
Copper(II) sulfate
CuSO4
White

Copper(II) sulfate pentahydrate
CuSO4 · 5H2O
Blue
Large crystals of copper sulfate
Cobalt(II) chloride
CoCl2
Deep blue
Cobalt(II) chloride
Cobalt(II) chloride hexahydrate
CoCl2 · 6H2O
Deep magenta
Cobalt(II) chloride hexahydrate
Manganese(II) chloride tetrahydrate
MnCl2 · 4H2O
Pink
Manganese(II) chloride tetrahydrate
Copper(II) chloride dihydrate
CuCl2 · 2H2O
Blue-green
copper(II) chloride dihydrate
Nickel(II) chloride hexahydrate
NiCl2 · 6H2O
Green
Nickel(II) chloride hexahydrate
Lead(II) iodide
PbI2
Yellow
Lead(II) iodide

Ions in aqueous solution
Name
Formula
Color
Alkali metals
M+
None
Alkaline earth metals
M2+
None
Scandium(III)
Sc3+
None
Titanium(III)
Ti3+
Violet
Titanyl
TiO2+
None
Vanadium(II)
V2+
Lavender
Vanadium(III)
V3+
Dark grey/green
Vanadyl
VO2+
Blue
Pervanadyl
VO2+
Yellow
Metavanadate
VO3-
None
Orthovanadate
VO43-
None
Chromium(III)
Cr3+
Blue-green
Chromate
CrO4 2-
Colorless or Yellow(sometimes)
Dichromate
Cr2O72-
Orange
Manganese(II)
Mn2+
Colourless
Manganate(VII) (Permanganate)
MnO4-
Deep violet
Manganate(VI)
MnO42-
Dark green
Manganate(V)
MnO43-
Deep blue
Iron(II)
Fe2+
Light blue
Iron(III)
Fe3+
Yellow/brown
Cobalt(II)
Co2+
Pink
Cobalt-ammonium complex
Co(NH3)63+
Yellow/orange
Nickel(II)
Ni2+
Light green
Nickel-ammonium complex
Ni(NH3)62+
Lavender/blue
Copper(II)
Cu 2+
Blue
Copper-ammonium complex
Cu(NH3)42+
Royal Blue
Tetrachloro-copper complex
CuCl42-
Yellow/green
Zinc(II)
Zn2+
Bluish-white
Silver
Ag+
None
1.     Sc - scandium salts, such as the chloride, ScCl3, are colourless and are not typical of transition metals
2.     Ti - titanium(III) chloride, TiCl3, is purple
3.     V - vanadium(III) chloride, VCl3, is green
4.     Cr - chromium(III) sulphate, Cr2(SO4)3, is dark green (chromate(VI) salts are yellow, dichromate(VI) salts are orange)
5.     Mn - manganese compound -  potassium manganate(VII), KMnO4, is purple (manganese(II) salts eg MnCl2 are pale pink)
6.     Fe - iron(III) chloride, FeCl3, is yellow-orange-brown.
o    Iron(II) compounds are usually light green and iron(III) compounds orange/brown.
7.     Co - cobalt sulphate, CoSO4, is pinkish
8.     Ni - nickel chloride, NiCl2, is green
9.     Cu - copper(II) sulphate, CuSO4, is blue.
o    Most common copper compounds are blue in their crystals or solution and sometimes green.
o    The blue aqueous copper ion, Cu2+(aq), actually has a more complicated structure:
§  *[Cu(H2O)6]2+(aq) and when excess ammonia solution is added,
§  after the initial gelatinous blue copper(II) hydroxide precipitate is formed, Cu(OH)2,
§  it dissolves to form the deep royal blue ion: *[Cu(H2O)2(NH3)4]2+(aq).
§  *are called complex ions and when coloured are typical of transition metal chemistry.
o    Copper(II) oxide, CuO, black insoluble solid, readily dissolving in acids to give soluble blue salts e.g.
§  copper(II) sulphate, CuSO4, from dilute sulphuric acid,
§  copper(II) nitrate, Cu(NO3)2, from dilute nitric acid
§  and greeny-blue copper(II) chloride, CuCl2, from dilute hydrochloric acid.
o    Copper(II) hydroxide, Cu(OH)2, blue gelatinous precipitate formed when alkali added to copper salt solutions.
o    Copper(II) carbonate, CuCO3, is turquoise-green insoluble solid, readily dissolving in acids, evolving carbon dioxide, to give soluble blue salts (see above)
o    Copper's valency or combining power is usually two e.g. compounds containing the Cu2+ ion.
§  However there are copper(I) compounds where the valency is one.
§  This variable valency, hence compounds of the same elements, but with different formulae, is typical of transition metal compounds e.g.
§  copper(I) oxide, Cu2O, an insoluble red-brown solid (CuO is black),
§  or copper(I) sulphate, Cu2SO4, a white solid.
10. Zn - zinc salts such as zinc sulphate, ZnSO4, are usually colourless and are not typical of transition metals.


 Salts of Cu+ are reasonably common, often water insoluble and
mostly white in color.  However, Cu + is readily oxidized to Cu2+ in most aqueous solution
conditions.  So, Cu2+ salts are much more common than the Cu+ salts.  Many of these salts are
water soluble and highly colored













1)ചാള്‍സ് നിയമം


charles the great scientist



2)ബോയില്‍ നിയമം


Robert Boyle Father of Modern Science



SSLC 2011 FEB PHYSICS  MODEL QUESTION  14-ANSWER :A DISCUSSION WITH PHOTOS&VIDEO

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