The Chemistry of the Metallic Elements by David J. Steele and J. E. Spice (Auth.)

By David J. Steele and J. E. Spice (Auth.)

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The Wurtz reaction). (ii) A strong reducing agent ( e . g . TiCl 4 + Na - Ti). (iii) A coolant in nuclear reactors ( e . g . at Dounray). g. Na202. (i) (i) Small amounts used in bearing metal. (ii) A scavenger to remove traces of oxygen or nitrogen from other metals, e . g . copper. (iii) The production of LiAlH4 . U s e s of metal THE PROPERTIES OF THE ALKALI METALS: THEIR OCCURRENCE, EXTRACTION AND USES . Lithium TABLE 4. 3a. Group la: The Alkali Metals 33 Potassium (rubidium and c a e s ium are similar to potassium) Sodium Lithium Potassium halide (Occurs most readily) *X2 = any halogen.

M + i H 2 - MH Colour and structure Colourless ionic crystals containing the ions M + and H~ and having the sodium chloride structure Melting points, ° C. LiH = 6 8 0 ° . NaH = 7 0 0 - 8 0 0 ° . KH decomposes below melting point. Heat of formation A Hf kcal mole" 1 . LiH = - 2 1 . 0 KH= - 1 0 . 0 Water MH + H 3 0 - MOH + i H 2 t . Acid MH + H 3 0 + - M + + H s O + i H a t salt. Halogen (moist) MH + X3 - M + +X" + QX salt. hydrogen and is used in the filling of balloons at meterological stations: the ratio of volume of hydrogen liberated to weight of hydride is a maximum for lithium: L i H + H 2 0 -+LiOH+H 2 8g 22-4141.

A slow reaction. K2 0 2 , a n o r a n g e peroxide ion. (o-o)= Pale yellow crystals. Ions present: Na+ and Colourless crystals with the ' fluorite structure. Ions present: Na+ + 0 = . i s s i m i l a r t o Na 2 0 . ^ " - ° Colour and structure THE ALKAU METALS: THE CHEMISTRY OF THEIR OXIDES. Colourless crystals, with the ' fluorite' structure. Ions ♦<*>■•• present are Li+ + 0 = . 2Li + j 0 2 - Li 2 0 or Li 2 C0 3 Li 2 0, Lithium monoxide. 5. A very strong oxidising agent. A strong oxidising agent; reacts violently with cotton wool, sawdust, charcoal, aluminium powder and many organic substances.

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