[He]2s^22p^6
A neutral oxygen atom has the electron configuration of: 1s2 2s2 2p4
Oxygen has six valence (outer-shell) electrons and therefore gains two more electrons to form the O-2 ion. Its electron configuration is: 1s2 2s2 2p6 or simply [Ne].
1s^2 2s^2 2p^6 If it was a standard oxygen atom it's configuration would be: 1s^2 2s^2 2p^4. However, since it is an ion, it gains two electrons.
[He]2s^22p^6
figure it out yourself.
1s22s22p6
[Ar]3d9
1s2 2s2
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.
Strontium (Sr) Sr2+ ion and krypton have he same electronic configuration
With it being a dipositive ion, the original element has lost 2 electrons. Making the configuration 1s2 2s2 2p6 3s2 2p4. That Configuration is Sulfur.
The ions of elements nitrogen (N3-), oxygen (O2-), and fluorine (F-) will have the same electron configuration as a sodium ion (Na+), which is the same as the electron configuration of the noble gas neon.
The electron configuration is [Ar]3d2.4s2.
The electron configuration of selenium for a 2- ion is [Kr]4s2.3d10.4p6.
1s2 2s2 2p4
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.
It has 2 electrons in the first shell, and 8 in the second as it gains an electron to form an ion so the configuration is 2,8.
Se2- 1s22s22p63s23p64s23d104p6
Electron configuration of radium:Ra: [Rn]7s2Ra(2+): 1s2.2s2.2p6.3s2.3p6.3d10.4s2.4p6.4d1o.4f14.5s2.5p6.5d10.6s2.6p6.
Iron 2 is Fe 2+ and has electron configuration [Ar] s1d5 Iron 3 is Fe 3+ and has electron configuration [Ar] d5
The core notation for the electron configuration of a cobalt 2 ion is [Ar] 3d7. The [Ar] represents the electron configuration of the argon noble gas, which has the electron configuration 1s2 2s2 2p6 3s2 3p6. The 3d7 indicates that there are seven electrons in the 3d subshell of the cobalt ion.
Strontium (Sr) Sr2+ ion and krypton have he same electronic configuration
With it being a dipositive ion, the original element has lost 2 electrons. Making the configuration 1s2 2s2 2p6 3s2 2p4. That Configuration is Sulfur.
The ions of elements nitrogen (N3-), oxygen (O2-), and fluorine (F-) will have the same electron configuration as a sodium ion (Na+), which is the same as the electron configuration of the noble gas neon.
The electron configuration is [Ar]3d2.4s2.