melting point and boiling point trends in the periodic t

The melting and boiling point of alkaline Earth metals are characteristically low and do not show regular trends down the group. However these points are higher than the corresponding alkali metals in the same period as atoms of alkaline ..

Melting Points and Boiling Points - The melting and boiling points of group 14 elements are much higher as compared to those of group 13 elements. Explanation: It is because the atoms of group 14 can form four covalent bonds with..

The melting and boiling points of group 14 elements are much higher as compared to those of group 13 element..

Metals have high melting and boiling point - Tungsten has the highest melting point where as Hg has low boiling point. Na and K have low melting points..

Melting points (except for antimony and bismuth) and boiling points increase on going down the group from N to B..

The compounds containing hydrogen bonds have high melting and boiling points. Due to hydrogen bonding, the intermolecular force of attraction in the compound becomes large. Consequently, larger energy is required in separating these molecules before they can melt..

The melting and boiling points of covalent compounds are generally low. This is because of the fact that the forces between the molecules are weak and thus are easily overcome at low temperature..

Ionic compounds have high melting and boiling points. A large amount of energy is required to break the crystal lattice, because the ions are held together by strong electrostatic forces of attraction. The variation in melting point depends upon th..

All alkali metals are soft and have low melting and boiling points. As alkali metals have only one valence electron per metal atom, the energy binding the atoms in the crystal lattice of the metal is low. Consequently, the metallic bonds in these metals are not very s..

Ammonia (240 K) has a higher boiling point than phosphine (190 K) and then the boiling point increases down the group because of increase in size. In PH 3 and other hydrides, the intermolecular forces are Van der Waals' forces. These van der Waals' forc..