because Mg and O have more electropositivity and electronegativity rspt. than Na and Cl atoms.
MgCl2
KI
Lattice energy increases with greater charge and smaller size. Since the charges are the same for both compounds, you have to look at the sizes of the atoms, K and Na, and since both have Cl, you don't have to compare that with anything. K is larger than Na, so since NaCl has a smaller size and the same charge, it has higher lattice energy.
Yes. Because hydration energy of Na+ is greater than K+. More the hydration energy greater is solubility. A compound is soluble if hydration energy is greater than lattice energy.
The lattice energy of potassium bromide is more exothermic than the lattice energy of rubidium iodide because lattice energy is inversely proportional to atomic radius.
No. The ions of a salt as simple as NaCl are smaller than the wavelength of any visible liqht; X-rays are needed to determine lattice spacing.
Cao or CaS have a higher lattice energy
Lattice energy increases with greater charge and smaller size. Since the charges are the same for both compounds, you have to look at the sizes of the atoms, K and Na, and since both have Cl, you don't have to compare that with anything. K is larger than Na, so since NaCl has a smaller size and the same charge, it has higher lattice energy.
Its Lattice energy is greater than the solvation energy of water.
Yes. Because hydration energy of Na+ is greater than K+. More the hydration energy greater is solubility. A compound is soluble if hydration energy is greater than lattice energy.
The lattice energy of potassium bromide is more exothermic than the lattice energy of rubidium iodide because lattice energy is inversely proportional to atomic radius.
The bonds in compound A are stronger than the bonds in compound B.
This can be rationalised by looking at the lattice energy. Using Madelungs method the smaller Na+ ion causes a stronger coulombic attraction making it harder to beak up the lattice and increasing the mp.
No. The ions of a salt as simple as NaCl are smaller than the wavelength of any visible liqht; X-rays are needed to determine lattice spacing.
Cao or CaS have a higher lattice energy
For dissolving any solute the solvation energy of the solvent has to be more than the lattige energy of the solute. In this case the lattice energy of Nacl[salt] is more than that of sugar. Hence it takes more time to dissolve in water. ---- Akashraj Ghosh.
The
since ca2+ has a larger atomic radii compared to Mg2+ (and the same for F and CL2), the electrons are dispersed over a wider surface area and so have a lesser strength than that of magnesium. Hence, with a smaller atomic radii, Magnesium has stronger attractive forces with require more energy to be broken and therefore making it more exothermic than calcium.
It is a matter of lattice energy vs. heat of solution. The lattice energy is the energy change associated with the ions in the gas phase forming a solid (crystalline) lattice. It is typically an exothermic process, liberating energy. The heat of solution is the energy change associated with the ions being dissolved by solvent, and can be exothermic or endothermic. If the heat of solution is more exothermic than the lattice energy, than it is energetically favorable for the ionic compound to be solvated. If the lattice energy is more exothermic, than solvation will not occur.