[Ne] because adding the 3 electrons to Nitrogen which originally contains 7 e-, will give it 10e-, the same number as Neon, if you're using masteringchemistry, this is what you want to enter.
Argon has the same electron configuration as N3. Both have 10 electrons with the electron configuration 1s2 2s2 2p6.
Hydrogen electron configuration will be 1s1.
The electron configuration for germanium is [Ar]3d10.4s2.4p2.
The electron configuration of zirconium is: [Kr]5s24d2
Al3+
Argon has the same electron configuration as N3. Both have 10 electrons with the electron configuration 1s2 2s2 2p6.
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 of a nitride ion (N3-) is 1s2 2s2 2p6. This is because nitrogen has 7 electrons, and when it gains 3 electrons to become a nitride ion, it achieves a full outer shell with 8 electrons.
The ionic radius of N3- is larger than that of O2- because the extra electron in the N3- ion is located in a higher energy level, leading to larger electron-electron repulsions and an increase in the ionic radius. Additionally, the effective nuclear charge experienced by the electrons in the N3- ion is lower than that in the O2- ion, further contributing to the larger ionic radius of N3-.
The electron configuration for oxygen is [He]2s2.2p4.The electron configuration for sulfur is [Ne]3s2.3p4.
A cation has a depleted electron configuration.
The electron configuration for beryllium, Be, is 1s22s2.
The electronic configuration of einsteinium is: [Rn]5f11.7s2.
The electron configuration of francium is [Rn]7s1.
Nitrogen typically forms negative ions, such as nitride (N3-) ions, by gaining three electrons to achieve a stable electron configuration.
Hydrogen electron configuration will be 1s1.
The groundstate for Sodium (11-Na) is: 1S2 , 2S2, 2P6, 3S1 If you count the ^powers you notice it'll sum to 11, when Sodium is excited the outermost electron (3S1) will be excited from the 3S shell to the next shell up which is the 3P shell. The "core" electron configuration doesn't change so the first excited state is simply: 1S2 , 2S2, 2P6, 3P1 For the next excited state the electron that is now in the 3P shell will transition to the 4S shell before the 3D shell