The metallic character of group 14 elements increases from top to bottom because removal of electron becomes easier on moving down the group. Metallic character increases as you move down an element group in the periodic table. This is because electrons become easier to lose as the atomic radius increases, where there is less attraction between the nucleus and the valence electrons because of the increased distance between them.

Explanation:
Group 14 elements are also called Carbon family. The group includes four elements- Carbon (C), Silicon (Si), Germanium (Ge) and Tin (Sn). The metallic character of these elements can be explained as follows:

Increasing atomic size: As we move down the group, the atomic size of the elements increases. This is because of the addition of a new energy level in each successive element. Due to the increase in atomic size, the metallic character of these elements increases from top to bottom.

Decreasing ionization energy: The ionization energy of an element is the energy required to remove an electron from its outermost shell. As we move down the group, the ionization energy decreases due to the increase in atomic size. The outermost electron is held more loosely by the nucleus and is easier to remove. This decrease in ionization energy makes it easier for the elements to lose electrons and form positive ions, thus increasing their metallic character.

Decreasing electronegativity: Electronegativity is the tendency of an atom to attract electrons towards itself when it is bonded to another atom. As we move down the group, the electronegativity decreases due to the increase in atomic size. The valence electrons are farther away from the nucleus and experience less attraction from it. This decrease in electronegativity makes it easier for the elements to lose electrons and form positive ions, thus increasing their metallic character.

Metallic character trend: Based on the above factors, the metallic character of group 14 elements increases from top to bottom. Carbon and silicon are non-metals, germanium is a metalloid and tin is a metal. Tin has the highest metallic character among the group 14 elements due to its large atomic size, low ionization energy and low electronegativity.

Therefore, the correct answer is option 'B' - the metallic character of group 14 elements increases from top to bottom in the group due to the increasing atomic size, decreasing ionization energy and decreasing electronegativity.

Down the group atomic size increase no.of orbits increases electropositive nature increses therefore metallic character increase