for an oxygen atom,wich requeres more energy,the addition of two electrons or the removal of one electron?explain why

It much prefers to add two electrons over removing one electron. The removal of an electron must expend energy to remove a negatively charged electron from the positively charged nucleus. Adding two electrons actually gives up energy because the outside shell is being filled.

For an oxygen atom, it requires more energy to remove one electron than to add two electrons. This is because oxygen belongs to Group 16 (or Group VI) of the periodic table, which means it has six valence electrons. The electron configuration of an oxygen atom is 1s² 2s² 2p⁴.

When adding two electrons to an oxygen atom, these electrons will occupy the 2p orbital, which can hold a total of six electrons. Therefore, adding two electrons completes the 2p orbital, resulting in a stable configuration with a full outer shell. This is energetically favorable as it allows the oxygen atom to achieve a stable electron configuration similar to that of the noble gas neon.

On the other hand, removing one electron from an oxygen atom involves breaking the stability of the electron configuration. It would result in a partially filled 2p orbital, which is less stable. The remaining five valence electrons in the atom would experience increased repulsion, which requires more energy to overcome. Due to this repulsion, removing an electron from the oxygen atom is considered energetically unfavorable.

Therefore, adding two electrons to an oxygen atom requires less energy than removing one electron.

To determine whether the addition of two electrons or the removal of one electron requires more energy for an oxygen atom, we need to consider the atom's electron configuration and its tendency to gain or lose electrons.

The electron configuration of an oxygen atom is 1s² 2s² 2p⁴, which means it has six valence electrons. These electrons occupy the outermost energy level, also known as the valence shell.

Oxygen has a tendency to gain two electrons to achieve a stable electron configuration similar to that of the noble gas neon, which has a full valence shell. By adding two electrons, the electron configuration becomes 1s² 2s² 2p⁶, identical to that of neon.

On the other hand, removing one electron from an oxygen atom would disrupt the stability of its electron configuration. It would result in an electron configuration of 1s² 2s² 2p³, which is less stable compared to its original configuration. Removing an electron creates an oxygen ion with a positive charge (O+), and this scenario requires more energy due to the increased electrostatic forces of attraction between the remaining electrons and the positively charged nucleus.

Therefore, in the case of an oxygen atom, it requires more energy to remove one electron (ionization energy) than it does to add two electrons (electron affinity) because oxygen has a stronger tendency to gain electrons and achieve a stable electron configuration.

I don't know, sorry. I use to be so good at Chemistry.