Question

write the electron configuration of an atom of the element highlighted in this outline of the periodic table: hint: you do not need to know the name or symbol of the highlighted element!

Explanation:

Step1: Determine the noble gas core

The element is in period 4. The noble gas before period 4 is Ar (argon). The electron configuration of Ar is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}\).

Step2: Fill the remaining orbitals

After Ar, we have the 4s, 3d, and 4p orbitals. The 4s orbital fills first (\(4s^{2}\)), then the 3d orbitals (there are 10 electrons in 3d: \(3d^{10}\)), and then we count the position in the p - block. Since it is in the 4th period and p - block (the 14th column of the p - block part in the given table). After filling 4s and 3d, for the p - block, the number of electrons in the 4p orbital: we know that in the p - block, the first element of the p - block in period 4 has \(4p^{1}\). Our element is the 4th element in the p - block of period 4, so \(4p^{4}\)

Combining with the noble gas core (Ar), the electron configuration is \([Ar]4s^{2}3d^{10}4p^{4}\)

Answer:

\([Ar]4s^{2}3d^{10}4p^{4}\)