Electrolysis of fused will give 1) Na 2) NaOH 3) NaClO 4) NaClO3 12. An element having electronic configuration1,2 , ,3 ,3 ,4s2 2 … D. the alkalI MetalS D1 The alkali metals are lithium, sodium, potassium, rubidium, cesium, and francium. 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. They occur in Group 1 of the periodic table and so have an ionic charge of +1 in their compounds. potassium and sodium . Structures of the monomeric group 2 metal dihalides, MX 2 Fluorides are sparingly soluble. 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. 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 But for the alkaline earth metals, the nucleus also contains an additional positive charge. An alkali metal can easily lose its valence electron to form the univalent cation. The alkali metals can react with water to form alkaline compounds. Alkali metals have only one oxidation state which is +1. Doping with alkali metal elements such as lithium (Li), sodium (Na), and cesium (Cs), is another path toward high-conductive metal oxide. All the alkali metals are very reactive. Types of metals :- 1-noble metals - generally unreactive , e.g. The … The metals in this series are relatively light— lithium, sodium, and potassium are less dense than water (less than 1 g cm-3). metals and ns1 for alkali metals. The monovalent ions On moving down the group, there is an increase in the number of shells and, therefore, atomic and ionic radii increase. This is why they are called alkali metals. Alkali metals react with water to form hydroxides and hydrogen gas is released in the process. The reaction is so vigorous in nature that the hydrogen gas produced during the reaction catches fire. 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. Also, the elements of Group 2 (alkaline earths) have much higher melting points and boiling points compared to those of Group 1 (alkali metals). To keep them from reacting with oxygen in the air, pure alkali metals are often stored in oil. None occur as the free metal in nature. 3-alkaline earth metals – less reactive, higher melting points and harder than alkali metals, e.g. This gives them the largest atomic radii of the elements in their respective periods. They must be stored under an inert substance, such as kero­ Atomic and ionic radii Being the first element of each period, alkali metals have the largest atomic and ionic radii in their respective periods. Lithium is the only alkali metal that reacts slowly with water. 2-alkali metals - very reactive with low melting points and soft , e.g. The alkali metals are very reactive and are rarely found in nature as pure elements. 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 … Alkali metals have one electron in their outer shell, which is loosely bound. calcium, magnesium and barium . Their low ionization energies result in their metallic properties and high reactivities. 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