Question

lectron configuration of oxygen to explain why it tends to form a 2 - ion.
e items in the left column to the appropriate blanks in the sentences on the right.
the electron configuration of oxygen is
by
two electrons to form the

• ion. the electron configuration of the oxygen ion becomes the same as a noble gas

the noble gases are

Explanation:

Oxygen has an atomic number of 8. Its electron configuration is \(1s^{2}2s^{2}2p^{4}\) which can also be written as \([He]2s^{2}2p^{4}\). Noble gases have a full - filled valence shell and are stable. Oxygen needs to gain 2 electrons to achieve a full - filled valence shell (similar to neon, which has the electron configuration \(1s^{2}2s^{2}2p^{6}\) or \([Ne]\)). When oxygen gains 2 electrons to form \(O^{2 -}\), its electron configuration becomes \(1s^{2}2s^{2}2p^{6}\) (or \([Ne]\)). Noble gases are known for their stability due to their full valence shells.

Answer:

The electron configuration of oxygen is \([He]2s^{2}2p^{4}\). By gaining two electrons to form the \(2-\) ion, the electron configuration of the oxygen ion becomes the same as a noble gas neon. The noble gases are stable.