Question

Clicker Question Rank this series of ionic compounds from smallest to largest magnitude (most exothermic) lattice energy: +3-2 Al,O 41- NaC MgO CaO NaCl< CaO< MgO < Al,0, A. B. CaO< NaCl < MgO < Al,0 Al,0,<CaO< NaCl < MgO C. CaO< NaCl< Al,O D. < MgO 5 7 8 10 Li Be E. Al,O,< NaCl< CaO < MgO Ne 6941 9.012 10 81 12 01 1401 16.00 19.00 20.18 11 12 13 14 15 16 17 18 Na Mg 22 99 Al Si P Cl 35 451 Ar 2431 26 9 28.09 30.97 32 07 39.95 19 20 K 31 32 33 35 36 Ca Ga Ge As Se Br Kr 39 10 40.08 072 72 61 7492 78.96 9.90 83.80 6C

Answer 1

a) NaCl < CaO < MgO < Al₂O₃

lattice energy is directly proportional to magnitude of charge because higher the charge higher is the electrostatic force of attraction and hence more energy will release. so, Al2O3 have highest lattice energy as Al has +3 charge .

MgO has high lattice energy than CaO because Mg2+ size is smaller than Ca2+ so charge density is high in Mg2+ as compare Ca2+ to .

NaCl have lowest lattice energy as here Na has +1 charge lowest magnitude of charge.