The electron configuration of oxygen is [He]2s22p4.
The electrons configuration for O2- is [He]2s22p6.
Yes, O2 has shared electrons. In the O2 molecule, each oxygen atom shares two electrons with the other oxygen atom, forming a covalent bond. This sharing of electrons allows the atoms to achieve a stable electron configuration.
Na, Rb, Al3+, and S2- do not have a noble gas configuration as they do not have the complete outer shell of electrons like a noble gas. O2, Br, Ca, and O2- have noble gas configurations as they either have a complete outer shell of electrons or have gained/lost electrons to achieve a stable noble gas configuration.
The electron configuration of oxygen in the oxide ion (O2-) is 1s2 2s2 2p6 (equivalent to the configuration of a neon atom), as the oxide ion has gained two extra electrons compared to a neutral oxygen atom.
Oxygen tends to gain two electrons to complete its "octet", making it O2- with the electron configuration 1s22s22p6
The noble gas configuration of O2 is similar to that of neon (Ne). Oxygen (O) typically forms a stable configuration by gaining 2 electrons to achieve a full valence shell, similar to the configuration of a noble gas.
The electrons configuration for O2- is [He]2s22p6.
Yes, O2 has shared electrons. In the O2 molecule, each oxygen atom shares two electrons with the other oxygen atom, forming a covalent bond. This sharing of electrons allows the atoms to achieve a stable electron configuration.
Na, Rb, Al3+, and S2- do not have a noble gas configuration as they do not have the complete outer shell of electrons like a noble gas. O2, Br, Ca, and O2- have noble gas configurations as they either have a complete outer shell of electrons or have gained/lost electrons to achieve a stable noble gas configuration.
The electron configuration of oxygen in the oxide ion (O2-) is 1s2 2s2 2p6 (equivalent to the configuration of a neon atom), as the oxide ion has gained two extra electrons compared to a neutral oxygen atom.
Oxygen tends to gain two electrons to complete its "octet", making it O2- with the electron configuration 1s22s22p6
Neon, if you are talking about an oxygen ion.
The element, oxygen, is in group 16, period 2 of the periodic table. Thus its electron configuration is 1s2 2s2 2p4. Oxide's ionic state is O2-, so to get its electron configuration we just need to add two electrons to the old one. That yields 1s2 2s2 2p6.
[He]2s^22p^6
O: 1s22s22p4
MgO exists as Mg2+ and O2- ions due to the difference in electronegativity between magnesium and oxygen. Magnesium readily loses two electrons to achieve a stable electron configuration, forming Mg2+ ions. Oxygen readily gains two electrons to achieve a stable electron configuration, forming O2- ions. This transfer of electrons results in an ionic bond between the magnesium and oxygen ions, rather than a covalent bond where electrons are shared.
O2 shares two electron pairs, giving both oxygen atoms 8 electrons on the outer shell (noble gas configuration).