how are the alkali metals different from a alkaline earth metals give their reactions with water . oxygen. nitrogen and halogens
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Answer:
Alkali metals differ from Alkaline earth metals in their electronic configuration
The electronic configuration is ns¹ whereas the electronic configuration of alkaline earth metals is ns²
Alkali Metals reactions
Reaction with water - Alkali metals form hydroxide and dihydrogen by reacting with water
2M+2H₂o → 2M +2OH + H₂
(M is an alkali metal)
Reaction with oxygen - Alkali metals form oxides , peroxide and superoxide after reacting with oxygen
Lithium forms oxide, and some peroxide on reacting with oxygen
Li + O₂ =====> Li₂O
Sodium forms peroxide, and some superoxide on reacting with oxygen
Na + O₂ → Na₂O₂
Potassium, Rubidium and Caesium form superoxide on reacting with oxygen
K + O₂ → KO₂
Rb + O₂ → RbO₂
Cs + O₂ → CsO₂
Reaction with nitrogen - Only lithium reacts with nitrogen from alkali metals
6Li + N₂ → 2Li₃N
Reaction with halogens - Alkali metals react vigorously with halogens to form ionic halides
2Li + X₂ → 2LiX (where X is chlorine, bromine or iodine)
Alkaline Earth Metals reactions
Reaction with water - Beryllium and Magnesium are kinetically inert to water because of the formation of an oxide film on their surface. Calcium, Strontium and Barium react with water with increasing vigor even in cold to form hydroxides
M + 2H₂O → M(OH)₂ + H₂ (where M is an alkaline earth metal)
Reaction with oxygen - Alkaline earth metals also react with oxygen, though not as rapidly as Group 1 metals; these reactions also require heating. Similarly to Group 1 oxides, most group 2 oxides and hydroxides are only slightly soluble in water and form basic, or alkaline solutions.
All Group 2 metals all react similarly, burning to form oxides (compounds containing the O²⁻ ion) as shown:
2M +O₂ →2MO
Once initiated, the reactions with oxygen are vigorous. The only peroxides (compounds containing the O₂²⁻ ion) that can be formed from alkaline metals are strontium peroxide and barium peroxide. Both reactions require heat and excess oxygen. The general reaction is given below:
M+O₂→MO₂
where M represents Sr or Ba.
Reaction with nitrogen - Nitrates are formed by dissolution of carbonates in dilute nitric acid . Magnesium nitrate crystallises with 6 molecules of water whereas Barium nitrate crystallises as the anhydrous salt . All of them decompose on heating to give the oxide like lithium nitrate
2M(NO₃)₂ → 2MO + 4NO₂ +O₂ (M=Be, Mg, Ca, Sr, Ba)