Why does metalic character increase down a group in the periodic table?
Metallic charcter increases down group because: Metals lose outer electrons. At the bottom of group 4 for example, in tin and lead, outer electrons are far from the nucleus, weakly held and so lost easily. These outer electrons are also more shielded than in smaller atoms. Tin and lead therefore easily lose electrons, form ions and are metals. Their outer electrons delocalise to give the pure element a metal structure. At the top of group 4, in carbon and silicon, outer electrons are close to the nucleus and strongly held so not easily lost. Carbon and silicon are therefore non-metals. Atomic radius increases down the group Small atoms at the top attract bonding pairs of electrons strongly so covalent bonds favoured. Ionisation energies high at top because electrons close to nucleus so no positive ions formed. Large atoms at bottom weakly attract bonding pairs of electrons so covalent bonds are formed with difficulty. Ionisation energies low at bottom because electrons distant from nuc
