In the electron configuration of an atom, the 4s orbital is generally filled before the 3d orbital due to the lower energy level of the 4s orbital. This follows the Aufbau principle, where electrons fill orbitals in order of increasing energy. Thus, in the electron configuration of an atom, the 4s orbital is filled before the 3d orbital, leading to the configuration 4s2 instead of 3d2.
The noble gas configuration for Titanium (Ti) is [Ar] 3d2 4s2.
The element is titanium and is in 4th period, group 4.
[Ar] 3d2 4s2
The electron configuration of titanium (Ti) is Ar 4s² 3d². When titanium loses two electrons to form Ti²⁺, the electrons are removed first from the 4s subshell before the 3d subshell. Therefore, the electron configuration of Ti²⁺ is Ar 3d².
[Ar] 4s2 3d10 4p5
[Ar]4s23d2
The noble gas configuration for Titanium (Ti) is [Ar] 3d2 4s2.
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The element is titanium and is in 4th period, group 4.
[Ar] 3d2 4s2
Titanium --------------------------> Ti4+ + 4e-[1s2, 2s22p6, 3s23p6] 3d2, 4s2 --->[1s2, 2s22p6, 3s23p6] + 4 electrons (from 3d and 4s orbital)Ti4+ is iso-electronic to Argon [1s2, 2s22p6, 3s23p6 ], the foregoing noble gas.
[Ar]4s23d2
Period 4, Group 14 (= IV-A)Germanium, 32Ge, [Ar] 3d10 4s2 4p2 KLMN: (2, 8, 18, 4)Period 4, Group 4 (= IV) Titanium, 22Ti, [Ar] 3d2 4s2 KLMN: (2, 8, 10, 2)
1s2 2s2 2p6 3s2 3p6 4s2 3d3A+
Titanium has 10 core electrons, which are the electrons in the inner energy levels that are not involved in chemical bonding. The electron configuration of titanium is 1s2 2s2 2p6 3s2 3p6 4s2 3d2.
1s2 2s2 2p6 3s2 3p6 4s2 3d3
If you mean: 3d2+20d+12 then it is (3d+2)(d+6) when factored with the help of the quadratic equation formula