the correct order of the lattice energies of teh following ionic compounds is
a) Nacl>MgBr2>CaO>Al2O3
b)Al2O3>MgBr2>CaO>NaCl
c)MgBr2>Al2O3>CaO>NaCl
d)Al2O3>CaO>MgBr2>NaCl
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As we go across a period, the ionic charges increase. Due to this the lattice enthalpy or charges also increase. Hence lattice energy of Al > Mg > Na.
Also as we go down a group ionic size only increases but charge remains same. Hence as we go down a group, lattice energy decreases.
=> Li > Na > K
No we can first arrange the cations in the question.
Given Cations are : Na, Mg, Ca, Al
We know that, Al > Mg > Na
Also Mg > Ca
=> Correct order of decreasing lattice enthalpies are :
Al > Mg > Ca > Na
=> Option ( b ) has the same criteria.
Hence Option ( B ) is correct option.
Al₂O₃ > MgBr₂ > CaO > NaCl.
rajk123654987:
Ca > Na because Ca has charge + 2 while Na has charge + 1. Since charge is essential for higher lattice energy, Ca has greater lattice energy than Na.
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