Which essentially implies breaking a few bonds. Thus, higher the stronger the bond between the atoms, higher will be the melting point.

1. As the atomic number of elements increases, the melting point increases because there are more electrons around the nucleus, which creates a stronger negatively-charged force. With stronger forces, the melting point rises. Non-metals usually have low melting points.

Atomic radius does not influence boiling point, but both are influenced by the number of electrons associated with the heavier halogens.

The atoms also get smaller and have more protons as you go from sodium to magnesium to aluminum. The attractions and therefore the melting and boiling points increase because: The nuclei of the atoms are more positively charged.

As you move right along the table, however, polarizability and van der Waals interactions predominate, and as larger atoms are more polarizable, they tend to exhibit stronger intermolecular forces and therefore higher melting and boiling points.

But what determines a substance’s melting point? So, the melting point depends on the energy it takes to overcome the forces between the molecules, or the intermolecular forces, holding them in the lattice. The stronger the intermolecular forces are, the more energy is required, so the higher the melting point is.

Melting range broadening (the range simply increases. Often the low end drops a lot, the high end less so or sometimes not much at all.) A melting range of 5º or more indicates that a compound is impure.

The stronger the forces of attraction between the particles, the more energy is needed to overcome them. The more energy is needed, the higher the melting point. The melting temperature of a crystalline solid is thus an indicator for the stability of its lattice.

Knowing the melting point of a chemical is very important for its storage & transport. In addition to that, melting point is often used to predict the partition behavior of a chemical between solid and gas phases. A higher melting point indicates greater intermolecular forces and therefore less vapour pressure.

Impurities in a solid cause a melting point depression because the impurity disrupts the crystal lattice energies. The more concentrated the solute, the greater the interference and the lower the freezing point of the solution. This concept can be applied to melting point (or freezing point) of a pure compound.

The most obvious is temperature. If the air temperature is above 32°F snow and ice will start to melt, at or below 32° and it will remain frozen. If the surface temperatures warm above 32°, the snow and ice touching the surface will warm and begin to melt.