When finding the identity of the element, you’ll have to identify the atomic number of that element. Recall that every single element in the periodic table has a corresponding atomic number.
The atomic number of an element is always equal to the number of protons of that element. And when the element is neutral (charge = 0), the number of protons is equal to the number of electrons.
Neutral element: Atomic number = # protons = # of electrons
Given electron configuration: [Ar]4s23d104p2 (in condensed electron configuration)
→ atomic number = 18
→ # of protons = # of electrons = 18
4s2→ 2 e-
3d2→ 2 e-
Give the chemical symbol for the element with the following ground state electron configuration.
Write the quantum numbers n and l select all possible values for ml for each subshell of the element.
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What scientific concept do you need to know in order to solve this problem?
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