The atomic number of an element is 14. Examine if this element will have metallic properties or not. Give reason to justify your answer.
Answer
Since Atomic number is 14
Electronic configuration: 2, 8, 4
This element belongs to the
- 14th group , as it has 4 valence electrons and Group Number = 10 + Number of electrons in outermost shell(valence electrons) = 10 + 4 = 14
- 3rd period , since there are three shells.
Therefore, the element is silicon .
Since it has 4 electrons in its outermost shell , it can neither gain electrons nor lose electrons as it will become unstable.
So,it forms covalent bonds (by sharing of electrons).
Silicon shows properties of both metals and non-metals. So, it is a metalloid.
