Interpretation:
The correct ground-state electron configurations of Al, B, and F are to be determined and the reason behind the given incorrect electronic configurations is to be explained.
Concept introduction:
An atom has a positivelycharged nucleus, which is surrounded by negativelycharged electrons. The electrons revolve around the nucleus in their orbitals (or shells). Each orbital has subshells.
The arrangement of electrons in the orbitals of an atom is called electron configuration. It is written with the help of quantum numbers.
Every electron occupies orbitals in the increasing order of their energies.
Pauli Exclusion Principle states that no two electrons in the same atom can have the same quantum numbers.
Hund’s Rule states that when electrons occupy degenerate orbitals (i.e., orbitals having the same energies), they should occupy all the empty orbitals of the subshell before occupying the orbital with one electron.
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- One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?arrow_forwardUsing orbital box diagrams, depict an electron configuration for each of the following ions: (a) Mg2+, (b) K+, (c) Cl, and (d) O2.arrow_forward
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