Lattice energy is a measure of energy released in ionic crystals when the ions are brought together from infinity. It measures the attraction between ions so that they are held in a position. Ionic compound stability is mostly due to lattice energy.

Lattice energy is directly proportional to the charge on the ions and inversely proportional to the size of the ions.  Smaller the size, greater is the lattice energy.

The melting point of a material with low binding energy is low. When, the binding energy is low, the attraction between the valence electron and the nucleus is low. This also means that the intermolecular attraction is low. Hence, the melting point is low.

Lattice Energy is directly proportional to the charge on the ions and inversely proportional the size of the ions. As size decreases, lattice energy increases. So $MgO$ have higher lattice energy than $KCl$.

Lattice energy is the energy required to break apart an ionic solid and convert its component atoms into gaseous ions. The value of the lattice energy to always be positive.

The lattice energy of a salt  gives a rough indication of the solubility of the salt in water because it reflects the energy needed to separate the positive and negative ions in a salt. Sodium and potassium salts are soluble in water because they have relatively small lattice energies. Magnesium and aluminum salts are often much less soluble because it takes more energy to separate the positive and negative ions in these salts.

When sodium and chlorine react, an ionic bond is formed, and formation of ionic bond is fast and exothermic.

Lattice energy of ionic compound is directly proportional to charge on the ion and inversely propotional to size of ion.

Lattice Energy is directly proportional to the charge on the ions and inversely proportional to the size of the ions. The two species have the same charge but the size of $Se$ is greater than $O$. Hence lattoce energy of $Al _2O _3$ is greater than $Al _3Se _3$.

Lattice Energy is directly proportional to the charge on the ions and inversely proportional to the size of the ions. There are two factors at work here. The main factor is the charge on the ions. In $ZnO$, both positive and negative ions carry two charges. In $NaCl$, they only carry one. The lattice energy is much greater in $ZnO$ than in $NaCl$.

The breaking up of a compound into simpler constituents that are usually capable of recombining under other conditions. In electrolytic, or ionic, dissociation, the addition of a solvent or of energy in the form of heat causes molecules or crystals of the substance to break up into ions (electrically charged particles).

$NaF$  shows the highest lattice energy.Smaller the size of cation, more is attraction among ions. The bond between ions of opposite charge is strongest when the ions are small.The lattice energies for the alkali metal halides is therefore, largest.

Comparison of melting points of ionic compounds is generally done by considering the following two factors:

1. Charge of the cation/anion  : More the charge of cation or anion, stronger will be the forces of attraction between the ions and higher will be the melting point.
2. Ionic radii: More the distance between ions, lesser will be the strength of the bond giving rise to lesser melting point.                                              

Among the halides of lithium, $LiF$ has highest lattice energy due to similar sizes of cation and anion which results in efficient packing in the crystal structure.

The lattice energy decreases in the order $LiCl\, >\, LiBr\, >\, LiI$. 

Lattice energy is defined as the heat of formation for ions of opposite charge in the gas phase to combine into an ionic solid. It is directly proportional to the charge on the ions and inversely proportional to the size of the ions. 

Among the cations, $Al^{3+},\ Ca^{2+},\ Li^{+}$ and $Mg^{2+}$, $Al^{3+}$ has the highest charge. Hence, $AlBr _3$ has the highest lattice energy. The lattice energy is directly proportional to the charge on the ion and inversely proportional to the size of the ion. 

Lattice energy is directly proportional to the charge of the ions and inversely proportional to the size of the ions. Thus lattice energy increases as the size of anion decreases. 

Bond strength mostly depends on the charges present on each ion and the distance between them.Small, highly charged ions will form stronger bonds while large,minimally charged ions will form weaker bonds.

$NaCl$ will have the highest boiling point as it is the strongest ionic compound present in the given options. $NaCl$ have strong interionic forces as $Na^+$ and $Cl^-$ attracts each other very strongly which results in an increase in the compactness of the molecule, further its lattice enthalpy.

$LiCl$. $Li^+$ due to its small size and has high polarizing power and attracts the electron cloud of $Cl^-$ towards itself which results in high lattice energy of the molecule.

Lattice enthalpy is a measure of the strength of the forces between the ions in an ionic solid. The greater the lattice enthalpy, the stronger the forces. 

Charge matter in lattice energy so here $Al^{+3}, Ca^{+2}, Mg^{+2}, Na^+$ and $O^{-2}$ & $Br^{-1}$
So $cao>MgBr _2 \Rightarrow$ overall order $Al _2O _3>Cao>MgBr _2>NaCl.$

lattice energy is high