how does ionic bonding affect the melting point?

Hint: compounds with ionic bonds are generally strong at room temperature, so I need different answers than this. (What’s more, this inquiry can likewise be concerning why compounds with ionic bonds are normally strong in room temperature).

Complete step by step answer:
Mixtures with ionic holding (\[NaCl\]) have higher liquefying focuses than those with covalent holding (\[CCl4\]). Intermolecular powers decide the liquefying purposes of mixtures. Ionic bond energies range from 250 to 4000 kJ/mol. It takes considerably more energy to isolate particles than it does to isolate atoms from one another. For instance, the atom carbon tetrachloride is a nonpolar covalent particle, (\[CCl4\]). Its dissolving point is - 23$^\circ $C. Conversely, the ionic strong \[NaCl\] has a dissolving purpose of 800$^\circ $C.
The electrostatic fascination (ionic connection) among cations and anions is solid. It takes a great deal of energy to defeat this fascination to permit the particles to move all the more unreservedly and structure a fluid.
Ionic mixtures have higher softening (and limits) than covalent mixtures. You can consider it like this: In an ionic compound, the entirety of the particles resemble little magnets. Thus, the entirety of the magnets adhere to one another firmly, making them difficult to pull separated (you need to really break ionic securities to liquefy the compound).

Note: Mixtures with ionic holding have higher dissolving focuses than those with covalent holding. Intermolecular powers decide the liquefying purposes of mixtures. An ionic compound is composed of charged particles, called particles. It has a goliath cross-section structure with solid electrostatic powers of fascination.