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1s2 2s2 2p4
Electron configuration for oxygen (O) is 1s2 2s2 2p4. The valency is 2-.
1s2 2s2 2p4
6 valence electrons 1s2 2s2 2p4 These 6 valence electrons are in the outer shell.
Atoms of the element sodium (atomic number 11) have the electron configuration 1s22s22p63s1 with the noble gas form [Ne]3s1
1s^2 2s^2 2p^2 3s^2
Gallium does. Atomic # 31
Electron Configuration: 1s2 2s2 2p4 Abbr: [He] 2s2 2p4
1s2 2s2 2p4
S- = 1s2 2s2 2p4
1s2 2s2 2p4
1s2 2s2 2p4
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.
Ground state: 1s2 2s2 2p5Excited state: 1s2 2s2 2p4 3s1In the excited state, one of the 2p electrons jumped into a 3s orbital. This is unstable, and the electron will jump back down, releasing energy in the same amount of energy that was required to excite the electron initially.
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.
4 is the number of electrons in that sublevel.
Electron configuration for oxygen (O) is 1s2 2s2 2p4. The valency is 2-.