s- Block Reactions | A Problemistic Approach | Part-3 | Explained by IITian | Jee Mains | Advanced

Hello Guys, In this video we are going to discuss some of the awesome questions for jee mains, advanve, NEET, AIIMS and BITSAT. Since, s-block is one of the most important topic for Jee Mains, Advance, NEET and BITSAT.
Firstly, I would like to revise the previous learned reactions.
2NaOH + 2C → 2Na +2CO + H2
FeCl3 + 3NaOH →Fe(OH)3 + 3NaCl
NH4Cl + NaOH → NaCl + NH3 (pungent smell) + H2O
HgCl2 + 2NaOH → HgO (yellow powder) + 2NaCl + H2O
Zn(OH)2 ↑ + 2NaOH → Na2ZnO2 + 2H2Oh
Al2O3 ↑ + 2NaOH → 2NaAlO2 + H2O
SiO2 + 2NaOH → Na2SiO3 + H2O
3P + 3 NaOH +3H2O → PH3 + 3NaH2PO2
2Al + 2 NaOH + 2H2O → 3H2 + 2NaAlO2
2Na2O2 = 2 Na2O + O2 (400-675°C, vacuum).
Na2O2 + 8H2O(moisture) = Na2O2 - 8H2O (0° С).
Na2O2 + 2H2O(cold) = H2O2 + 2NaOH
2Na2O2 + 2H2O(hot) = O2↑ + 4NaOH.
Na2O2 + 2HCl(diluted, cold) = 2NaCl + H2O2.
2Na2O2 + 2H2SO4 (diluted, hot) = 2Na2SO4 + 2H2O + O2↑.
Na2O2 + O2 = 2NaO2 (450-500°C, pressure).
2Na2O2 + S = Na2SO3 + Na2O (100° C)
2Na2O2 + С(graphite) = Na2CO3 + Na2O (100°C)
3Na2O2 + 2Al (powder) = 2NaAlO2 + 2Na2O (70-120°C).
2Na2O2 + 2 CO2 = 2Na2CO3 + O2
Na2O2 + CO = Na2CO3 (normal temp.).
Na2O2 + MnO2 = Na2MnO4 (400-500°C).
Na2O2 + 2Na = 2Na2O (130-200°C, in the atmosphere of Ar).
5Na2O2 + 8H2SO4(diluted) + 2KMnO4 = 5O2↑ + 2MnSO4 + 8H2O + 5Na2SO4 + K2SO4.
Na2O2 + 2H2SO4(diluted) + 2NaI = I2↓ + 2Na2SO4 + 2H2O.
3Na2O2 + 2Na3[Cr(OH)6] (hot) = 2 Na2CrO4 + 8NaOH + 2H2O.
Na2O2 + 2H2SO4 (diluted) + 2FeSO4 = Fe2(SO4)3 + Na2SO4 + 2H2O
Na2O2 + 2Fe(ОН)2(suspension) = 2FeO(OH)↓ + 2NaOH.
group 2 metals are called alkali earth metals because their hydroxides are strong alkali (just like those of alkali metals) plus these all are found in earth crust.
Like alkali metals, alkaline earth metals are also highly reactive and hence do not occur in the free state but are likely distributed in nature in the combined state as silicates, carbonates, sulphates and phosphates.
Reaction With Hydrogen - (Formation of Hydrides)
All the alkaline earth metals except be combine with hydrogen directly on heating to form metal hydrides of formula MH2.
M + H2 → MH2
The hydride of beryllium can also be obtained by the reduction of BeCl2 with LiAlH4
2BeCl2 + LiAlH4 → 2BeH2 + LiCl + AlCl3
Both BeH2 and MgH2 are covalent compounds having polymeric structures in which H - atoms between beryllium atoms are held together by three
centre - two electron (3C - 2e) bonds.
The hydrides of other elements of this group i.e. CaH2, SrH2 and BaH2 are ionic and contain the H- ions.
All the hydrides of alkaline earth metals reacts with water liberating H2 gas and thus act as reducing agents.
MH2 + 2H2O → M (OH)2 + 2H2
CaH2 is called Hydrolith and is used for production of H2 by action of water on it.
Reaction With Carbon - (Formation of Carbides)
When BeO is heated with carbon at 2175 - 2275 K a brick red coloured carbide of the formula Be2C is formed
2BeO + 2C = Be2C + 2CO.
It is a covalent compound and react water forming methane.
Be2C + 4H2O → 2Be (OH)2 + CH4
The rest of the alkaline earth metals (Mg, Ca, Sr & Ba) form carbides of the general formula, MC2 either when the metal is heated with carbon in an electric furnace or when their oxides are heated with carbon.
Ca + 2C = CaC2
CaO + 3C = CaC2 + CO
All these carbides react with water producing acetylene gas.
CaC2 + 2H2O → HC ≡ CH + Ca (OH)2
Reaction with Halogens
The alkaline earth metals react with halogens at elevated temperature to form the halides of the types MX2.
Action of Acids
The alkaline earth metals readily react with acids liberating hydrogen.
M + 2HCl → MCl2 + H2 ( M = Be, Mg, Ca, Sr, Ba)
Reaction with Ammonia
Like alkali metal, the alkaline earth metals dissolve in liquid ammonia to give deep blue black solution from which ammoniates [ M (NH3)6 ]2+ can be recovered.
Reaction With Air (Nitrogen and Oxygen)
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