Explanation:
The element with the electron configuration 1s22s22p6 is Neon (Ne).
This element belongs to group 18 (Noble Gases) in the periodic table. The reasoning is:
- The electron configuration shows a full outer energy level (octet) with 8 electrons, which is characteristic of the Noble Gases.
- The element has a stable electronic configuration, indicating it is a member of the Noble Gas family.
During the formation of a bond, Neon is likely to receive 0 electrons from another element. This is because:
- Neon has a full outer energy level, making it stable and unreactive.
- It does not tend to gain or lose electrons to form bonds, as its octet is already complete.
Therefore, Neon typically does not form bonds with other elements by receiving electrons. Instead, it often exists as a monatomic gas or participates in weak intermolecular forces.