Trends In Periodic Table

Indium (In) is a group 13 element and has 3 valence electrons, while silicon (Si) has 4.
When indium is doped into silicon, it creates holes (absence of electrons) because one valence bond remains unsatisfied.
These holes act as positive charge carriers, making the semiconductor a p-type.

The given electronic configuration is . For , the electronic configuration becomes: This indicates that the element has 2 electrons in the -orbital and 2 electrons in the -orbital. The number of electrons in the -orbital (2 electrons) and -orbital (2 electrons) determines the group number. - The -block elements (transition metals) follow the and filling rule. The sum of the electrons in the -orbital and -orbital gives the group number. - The number of electrons in the and orbitals is 4, and the element will belong to Group 4. Thus, the group number of the element is 4.