\nIron(III) sulphate crystal<\/td>\n | Brown<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n The aqueous solutions<\/strong> of these compounds are also coloured<\/strong> because of the existence of ions of transition elements.<\/p>\nTable shows the colours<\/strong> of some ions<\/strong> ions of transition elements<\/strong> in aqueous solutions.<\/p>\n\n\n\nIons of transition\u00a0element<\/strong><\/td>\nFormula of the ion\u00a0<\/strong><\/td>\nColour of ion in aqueous solution<\/strong><\/td>\n<\/tr>\n\nCopper(II) ion<\/td>\n | Cu2+<\/sup>(aq)<\/td>\nBlue<\/td>\n<\/tr>\n | \nIron(II) ion<\/td>\n | Fe2+<\/sup>(aq)<\/td>\nPale green<\/td>\n<\/tr>\n | \nIron(III) ion<\/td>\n | Fe3+<\/sup>(aq)<\/td>\nYellow \/ yellowish- brown \/ brown<\/td>\n<\/tr>\n | \nCobalt(II) ion<\/td>\n | Co2+<\/sup>(aq)<\/td>\nPink<\/td>\n<\/tr>\n | \nNickel(II) ion<\/td>\n | Ni2+<\/sup>(aq)<\/td>\nGreen<\/td>\n<\/tr>\n | \nChromium(III) ion<\/td>\n | Cr3+<\/sup>(aq)<\/td>\nGreen<\/td>\n<\/tr>\n | \nManganese(II) ion<\/td>\n | Mn2+<\/sup>(aq)<\/td>\nLight pink<\/td>\n<\/tr>\n | \nManganate(VII) ion<\/td>\n | MnO4<\/sub>–<\/sup>(aq)<\/td>\nPurple<\/td>\n<\/tr>\n | \nChromate(VI) ion<\/td>\n | CrO4<\/sub>2-<\/sup>(aq)<\/td>\nYellow<\/td>\n<\/tr>\n | \nDichromate(VI) ion<\/td>\n | Cr2<\/sub>O7<\/sub>2-<\/sup>(aq)<\/td>\nOrange<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n Reactions of aqueous solutions of transition element compounds with sodium hydroxide solution and ammonia solution<\/strong><\/p>\n\n- Aqueous solutions of transition element compounds are coloured.<\/li>\n
- These aqueous solutions can react with sodium hydroxide solution and ammonia solution to form coloured precipitates of metal hydroxides.<\/strong> These precipitates may be soluble\/insoluble<\/strong> in excess sodium hydroxide solution and ammonia solution.<\/li>\n
- The precipitates of the metal hydroxides formed are coloured because these are compounds of transition elements.<\/strong><\/li>\n<\/ul>\n
Table shows some examples of these reactions. \n<\/p>\n Uses of coloured transition element compounds<\/strong><\/p>\nIn our daily life, compounds of transition elements are added to paints and glass to make them coloured. \nFor example:<\/p>\n \n- Green glass is made by adding a mixture of chromium(III) oxide and copper(II) oxide to the glass.<\/li>\n
- Yellow paint is made by adding barium chromate(VI) to the paint.<\/li>\n<\/ul>\n
Existence of naturally occurring substances containing transition element compounds<\/strong><\/p>\n\n- Precious stones (gemstones) are naturally occurring substances that exist in different colours.<\/li>\n
- Precious stones are coloured naturally because of the existence of the compounds of transition elements in them.<\/li>\n
- Precious stones are usually used as ornaments<\/strong> and decorative pieces<\/strong>.<\/li>\n
- Table shows the colours and the types of compounds of transition elements that exist in a few precious stones
\n\n\n\n\n Precious\u00a0<\/strong>stone<\/strong><\/p>\n<\/td>\nColour<\/strong><\/td>\nTransition elements that exist in the form of compounds<\/strong><\/td>\n<\/tr>\n\nEmerald<\/td>\n | Green<\/td>\n | Nickel, iron<\/td>\n<\/tr>\n | \nRuby<\/td>\n | Red<\/td>\n | Chromium<\/td>\n<\/tr>\n | \nSapphire<\/td>\n | Blue<\/td>\n | Iron, titanium<\/td>\n<\/tr>\n | \nAmethyst<\/td>\n | Purple<\/td>\n | Iron<\/td>\n<\/tr>\n | \nAgate<\/td>\n | Brownish-red<\/td>\n | Manganese, iron<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/li>\n<\/ul>\n 2. Exhibit different oxidation numbers in compounds<\/strong><\/span><\/p>\n\n- Transition elements exhibit different oxidation numbers in their compounds.<\/li>\n
- Oxidation number<\/strong> measures the charge carried by an element in its compounds. It has a positive or negative sign.<\/li>\n
- Table shows the oxidation numbers of some transition elements in their compounds.
\n\n\n\nTransition element<\/strong><\/td>\nOxidation number in compounds<\/strong><\/td>\n<\/tr>\n\nIron<\/td>\n | +2, +3<\/td>\n<\/tr>\n | \nNickel<\/td>\n | +2, +3<\/td>\n<\/tr>\n | \nCopper<\/td>\n | +1, +2<\/td>\n<\/tr>\n | \nManganese<\/td>\n | +2, +3, +4, +6, +7<\/td>\n<\/tr>\n | \nChromium<\/td>\n | +2, +3, +6<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/li>\n<\/ul>\n Naming of compounds<\/strong><\/p>\n\n- In the naming of compounds of transition elements with more than one oxidation number, Roman numerals<\/strong> that represent the oxidation numbers of that transition element must be inserted in the names of those compounds according to the IUPAC system.<\/strong><\/li>\n
- For example:
\nFeCl2<\/sub> is named as iron(II) chloride because the oxidation number of iron is +2. FeCl3<\/sub> is named as iron(III) chloride because the oxidation number of iron is +3.<\/li>\n<\/ul>\n3. Form complex ions<\/strong><\/span><\/p>\n\n- Transition elements can form complex ions.<\/li>\n
- A complex ion<\/strong> is a bigger-sized polyatomic ion formed when a fixed number of small molecules or ions <\/strong>(known as ligands<\/strong>) are bonded to a central transition metal ion.<\/li>\n
- An example of a complex ion formed by a transition element is tetraamminecopper(II) ion,<\/strong>\u00a0[Cu(NH3<\/sub>)4<\/sub>]2+<\/sup>. This complex ion consists of four ammonia molecules, NH3<\/sub> (ligands) bonded to the central copper(II) ion, Cu2+<\/sup>.
\nCu2+<\/sup> + 4NH3<\/sub>\u00a0\u2192 [Cu(NH3<\/sub>)4<\/sub>]2+<\/sup><\/li>\n- Other examples of complex ions are:\n
\n- Hexacyanoferrate(II) ion, [Fe(CN)6<\/sub>]2-<\/sup><\/li>\n
- Hexacyanoferrate(III) ion, [Fe(CN)6<\/sub>]3-<\/sup><\/li>\n
- Hexaaquocobalt(II) ion, [Co(H,0)6<\/sub>]2+<\/sup><\/li>\n
- Hexaamminechromium(III) ion, [Cr(NH3<\/sub>)6<\/sub>]3+<\/sup><\/li>\n<\/ul>\n<\/li>\n<\/ul>\n
4. Act as catalysts<\/strong><\/span><\/p>\nHow do transition elements act as catalysts?<\/h2>\nTransition elements or their compounds can act as | | | | | | | | | | | | | | | | | | | | | |