1s2 2s2 2p3 (the numbers at the end of each little thingymabober are smalll like exponents!)
The electron configuration for a nitrogen anion with a charge of -2 (N²⁻) involves adding two additional electrons to the neutral nitrogen atom. The neutral nitrogen atom has an electron configuration of 1s² 2s² 2p³. Therefore, the electron configuration for the N²⁻ ion is 1s² 2s² 2p⁵.
The general electron configuration for lanthanides is [Xe] 4f^n 5d^1 6s^2, where n ranges from 1 to 14 depending on the specific lanthanide element.
The chemical symbol for an element with an electron configuration that ends with np² is represented by the group 14 elements in the periodic table. For example, if n = 2, the element is silicon (Si); if n = 3, it is germanium (Ge); and if n = 4, it is tin (Sn). Each of these elements has an outer electron configuration that concludes with np².
Hydrogen electron configuration will be 1s1.
The n value for the 6g sublevel is 6. The principal quantum number (n) represents the energy level or shell in the electron configuration. In this case, the electron is in the 6th energy level.
Nitrogen's symbol is N. Its electron configuration is 2s, 3p.
The electron configuration of oxygen is 1s22s22p4.
The electron configuration for a nitrogen anion with a charge of -2 (N²⁻) involves adding two additional electrons to the neutral nitrogen atom. The neutral nitrogen atom has an electron configuration of 1s² 2s² 2p³. Therefore, the electron configuration for the N²⁻ ion is 1s² 2s² 2p⁵.
Cobalt electron configuration is [Ar]3d7.4s2.Nitrogen electron configuration is [He]2s2.2p3.
The shorthand electron configuration allows all of the electrons in a noble gas preceding an element to be omitting and written by [nobel gas name]. For nitrogen, the noble gas preceding it is He. Thus, its configuration is [He]2s2 2p3.
The general electron configuration for lanthanides is [Xe] 4f^n 5d^1 6s^2, where n ranges from 1 to 14 depending on the specific lanthanide element.
L-1 electron configuration
The chemical symbol for an element with an electron configuration that ends with np² is represented by the group 14 elements in the periodic table. For example, if n = 2, the element is silicon (Si); if n = 3, it is germanium (Ge); and if n = 4, it is tin (Sn). Each of these elements has an outer electron configuration that concludes with np².
The valance electron configuration is the same in each at ns1 where n = the period number.
To determine the number of valence electrons in an atom using its electron configuration, look at the highest energy level (n) in the electron configuration. The number of electrons in this energy level is the number of valence electrons.
1s22s22p3
The outer electron configuration for all group 1 elements is ns1, where n represents the energy level of the outermost electron. This means that group 1 elements have one electron in their outermost shell.