The metals in this series are relatively light— lithium, sodium, and potassium are less dense than water (less than 1 g cm-3). The reaction is so vigorous in nature that the hydrogen gas produced during the reaction catches fire. MgF 2 K sp = 7.42x10-11 CaF 2 K sp = 1.46x10-10 SrF 2 K sp = 4.33x10-9 BaF 2 K sp = 1.87x10-7 Slightly more solubility for larger cations The alkali metals are very reactive and are rarely found in nature as pure elements. calcium, magnesium and barium . metals and ns1 for alkali metals. Types of metals :- 1-noble metals - generally unreactive , e.g. Alkali metals are soft enough to be cut with a knife. Alkali nitrides Li 3N Na 3N Reactivity of alkali metals with halogens, hydrogen, nitrogen H (MX,s) H (M,s) IE 1 (M,g) H (X,g) (X,g) Ho (MX,s) EA lattice o a a o f metal-dependant term halide-dependant term Standard enthalpies of formation ( fH ) and lattice energies ( latticeH ) of alkali metal halides, MX. The alkali metals (lithium, sodium potassium., cesium, and francium) are the most reactive metals in the Periodic Table (Table 3.7) insofar as they react vigorously or even explosively with cold water, resulting in the displacmet of hydrogen, itself a flammable gas that can … Their low ionization energies result in their metallic properties and high reactivities. But for the alkaline earth metals, the nucleus also contains an additional positive charge. potassium and sodium . Alkali metals react with water to form hydroxides and hydrogen gas is released in the process. Lithium is the only alkali metal that reacts slowly with water. It is difficult to develop a simple explanation for this trend because density depends on two factors, both of which change down the group. The … An element having electronic configuration1,2 , ,3 ,3 ,4s2 2 … On moving down the group, there is an increase in the number of shells and, therefore, atomic and ionic radii increase. The alkali metals can react with water to form alkaline compounds. They must be stored under an inert substance, such as kero­ An alkali metal can easily lose its valence electron to form the univalent cation. Traditionally, they are used as p-type dopants in ZnO (Park et al., 2002; Zeng et al., 2005; Wang et al., 2009).As shown in Fig. silver, platinum , gold and palladium . None occur as the free metal in nature. Alkali metals have only one oxidation state which is +1. The monovalent ions Also, the elements of Group 2 (alkaline earths) have much higher melting points and boiling points compared to those of Group 1 (alkali metals). This gives them the largest atomic radii of the elements in their respective periods. 3-alkaline earth metals – less reactive, higher melting points and harder than alkali metals, e.g. Electrolysis of fused will give 1) Na 2) NaOH 3) NaClO 4) NaClO3 12. Structures of the monomeric group 2 metal dihalides, MX 2 Fluorides are sparingly soluble. 2-alkali metals - very reactive with low melting points and soft , e.g. All the alkali metals are very reactive. D. the alkalI MetalS D1 The alkali metals are lithium, sodium, potassium, rubidium, cesium, and francium. Alkali metals have one electron in their outer shell, which is loosely bound. This is why they are called alkali metals. Alkali metals are powerful reducing agents because 1) These are metals 2) these are monovalent 3) Their ionic radii are large 4) their ionization potentials are low 11. They occur in Group 1 of the periodic table and so have an ionic charge of +1 in their compounds. Doping with alkali metal elements such as lithium (Li), sodium (Na), and cesium (Cs), is another path toward high-conductive metal oxide. To keep them from reacting with oxygen in the air, pure alkali metals are often stored in oil. 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