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Solvay process is used to prepare sodium carbonate. Reactions occurs in solvay process are -  
When the alkaline earth metals are heated the electrons are excited to higher energy levels and when they drop back to the ground state, energy is emitted in the form of visible light. Hence the colour is observed. The electrons in beryllium and magnesium are too strongly bound to get excited by flame. Hence, these elements do not impart any colour.  
 The alkali metals dissolve in liquid ammonia giving deep blue solutions which are conducting in nature.  The blue colour of the solution is due to the ammoniated electron which absorbs energy in the visible region of light and thus imparts blue colour to the solution. The solutions are paramagnetic. In concentrated solution, the blue colour changes to bronze colour and becomes diamagnetic
It is because of the low ionisation energy of K and . They lose electron easily. On the other hand, Lithium is smaller in size as compared to caesium and lithium, it requires high energy to lose an electron. Therefore, lithium is not used in a photoelectric cell.  
Alkali and alkaline earth metals not be obtained by chemical reduction methods because to reduce their oxides we need to use a strong reducing agent, but there is no other reducing agent which is stronger than them.
Chemical similarities between lithium and magnesium-  and  slowly react with water and their hydroxide and oxides are also less soluble in water. On heating, their hydroxide decomposes. Both the element form nitride  and  by direct reaction with nitrogen.   and  do not give superoxide on reacting with an excess of oxygen. Lithium and Magnesium carbonates easily decompose into their oxides and...
(i) Ionisation enthalpy- Alkali metals have low first IE as compare to alkaline earth metals because of having a large atomic size also after losing one electron they attain noble gas configuration. In alkaline earth metals, their first IE is higher then alkali metals because they have high effective nuclear charge and small in size as compare to group 1st element. However, they have low second...
As we know that in alkali metals, as we go down the group the atomic size increases and also the effective nuclear charge decreases. So, therefore, the outermost electron of potassium is easily removed. Electronic configuration of  and electronic configuration of sodium  (Na= ). Hence the reactivity of sodium is less than of potassium.  
Let suppose the oxidation state of Na is to be x. In the case of peroixide, the oxygen has  -1 oxidation state. So, now   
Electronic Configuration All the alkali metals have one valence electron,   outside the noble gas core. The loosely held s electron in the outermost valence shell of these elements makes them the most electropositive metals. They readily lose an electron to give monovalent M+ ions. Hence they are never found in the free or native state in nature.  
The general characteristics and gradation in properties of alkaline earth metals- General electronic configuration is [noble gas]. Have two electrons to lose and attain their nearest noble gas configuration. have smaller atomic and ionic radii than corresponding alkali metals in the same periods. First IE is higher than those elements of group 1 electropositive nature increase down the group...
Physical and chemical features of alkali metals- Physical features- All the alkali metals are silvery white, soft and light metals. Because of the large size, these elements have a low density which increases down the group from Li to Cs. However, potassium is lighter than sodium. The melting and boiling points of the alkali metals are low indicating weak metallic bonding due to the presence...