ASAP: in group 13, the only metalloid, boron, is at the very top of the group. Explain why the rest of the group has metallic behavior but boron does not.

The rest of the group will form bonds with intermediate nature between covalent and ions bods in their respective compounds, with thallium (Tl) behaving most close to a metal.

Moreover boron have a very high melting points (around 2200 °C) while in the boron cristal the chemical bonds are directed in space, similar with carbon suggesting his nature as a non-metal.

Other elements form the group Al, Ga, In, Tl have lower melting points 660, 30, 157 and 304 °C, respectively. Also in the elemental state, they have metallic characteristics: metalic luster, ductility, high electrical and thermal conductivity.

rosewarrior0 rosewarrior0 · Answer 2 · 2021-02-01T09:10:26+01:00

Answer: All elements in group 13 have 3 valence electrons. Boron has a few electron shells that it is just as easy for it to lose electrons, as it is to gain electrons, so it behaves like a metalloid. Since losing an electron is during a chemical reactions causes metallic behavior in elements. It is easier to lose 3 electrons than it is to gain 5, most of group 13 elements behave as metals.

Explanation:

All elements in group 13 have 3 valence electrons.

Losing electrons during chemical reactions causes metallic behavior in elements.

It is easier to lose 3 electrons than it is to gain 5, so most group 13 elements behave as metals.

Having fewer electron shells makes it easier to gain electrons.

Boron has so few electron shells that it is just as easy for it to lose electrons as it is to gain electrons, so it behaves like a metalloid.