Does MgO have the highest lattice energy?
Does MgO have the highest lattice energy?
Magnesium oxide will have the largest lattice energy because it has the largest attraction between the two ions. The size of the magnesium ion is smaller than the sodium ion; the size of the oxide ion (though having a larger charge) is smaller than chloride because they are in different ‘n’ shells.
Why is SiO2 melting lower than MgO?
Na2O, Al2O3 and MgO are ionic oxides and hence have a high melting point. MgO and Al2O3 have a higher melting point than Na2O since the charges are higher, resulting in a stonger attraction between the ions. SiO2 has a giant covalent structure and hence a high melting point. The melting points are thus much lower.
What is the lattice energy of MgO?
−3795 kJ/mol
Representative lattice energies
| Compound | Experimental Lattice Energy | Structure type |
|---|---|---|
| MgO | −3795 kJ/mol | NaCl |
| CaO | −3414 kJ/mol | NaCl |
| SrO | −3217 kJ/mol | NaCl |
| MgF2 | −2922 kJ/mol | rutile |
Which aluminum compound will have the highest lattice energy?
Why does aluminum chloride have a higher lattice energy than aluminum fluoride? From the table below (source: McMurry’s Chemistry [1, p. 212]), it is evident that AlCl3 has a higher lattice energy than AlF3, even though F is smaller than Cl.
Why is SiO2 more stable than Al2O3 and MgO?
SiO2 is much more stable then that of Al2O3 and MgO…. The reason is being that silicon dioxide is a covelent compound whereas , Magnesium oxide and Aluminium trioxide are both ionic compounds … The crystal lattice of silicon dioxide is much more stable and efficient …
Why is the lattice enthalpy of Alf₃ greater than MgO?
This factor makes lattice enthalpy increase; ion charge: the greater the charge on ions, the greater the attractive forces between them and, therefore, the larger the lattice enthalpy. As it turns out, the lattice enthalpy of AlF₃ (5215 kJ/mol) is indeed greater than that of MgO (3791 kJ/mol).
What is the lattice energy of the salt MgF2?
So, greater the charges of cation & anion, higher will be the lattice energy of the corresponding salt. Again, smaller the ionic radii of cation and anion, higher will be the lattice energy. Now, in comparison between MgF2 & LiF, we deal with Mg+2, Li+ and F– (in both case) ions.
How do you find the lattice enthalpy of two salts?
Lattice enthalpy of two salts can be compared by using Born–Lande equation (one of method) as, So, greater the charges of cation & anion, higher will be the lattice energy of the corresponding salt. Again, smaller the ionic radii of cation and anion, higher will be the lattice energy.