91Ó°ÊÓ

Explain why there are 14 members of each \(f\) block series.

Indicate which of the following electron configurations are ruled out by the Pauli exclusion principle: (a) \(1 s^{2} 2 s^{2} 2 p^{7}\) (b) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{3}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{12}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\)

Explain why the following ground state elecron configurations are not possible: (a) \(1 s^{2} 2 s^{3} 2 p^{3}\) (b) \(1 s^{2} 2 s^{2} 2 p^{\prime \prime} 3 s^{6}\) (c) \(1 s^{2} 2 s^{2} 2 p^{7} 3 s^{2} 3 p^{\mathrm{s}}\) (d) \(1 s^{22} 2 s^{22} p^{6} 3 s^{4} 3 p^{1} 4 s^{2} 3 d^{14}\)

Using the noble-gas shorthand notation, write the ground state electron configurations for the following elements: (a) Ti (b) \(\mathrm{K}\) (c) Fe (d) As (e) \(\mathrm{F}\)

Using the noble-gas shorthand notation, write. the ground state electron configurations for the following elements: (a) Si (b) Ni (c) Se (d) \(\mathrm{Cd}\) (e) \(\mathrm{Mg}\)

Using the noble-gas shorthand notation, write the ground state electron configurations for the following neutral atoms: (a) \(\mathrm{Ba}\) (b) \(\mathrm{Ag}\) (c) Gd (d) \(\mathrm{Pd}\) (e) Sn

Write out the complete pictorial representation of the electron configurations beyond the noble-gas core, using up and down arrows to represent each of the electron spins for the atoms \(\mathrm{Si}\) and Fe.

Write out the complete pictorial representation of the electron configurations beyond the noble-gas core, using up and down arrows to represent each of the electron spins for the atoms \(\mathrm{S}\) and \(\mathrm{Cr}\).

Using only the periodic table, write the ground state electron configuration of the following elements using the noble-gas shorthand notation: (a) \(\mathrm{Ca}\) (b) \(\mathrm{Br}\) (c) \(\mathrm{B}\) (d) \(\mathrm{Zn}\) (e) \(\underline{W}\)

Using only the periodic table, write the ground state electron configuration of the following elements using the noble-gas shorthand notation: (a) \(\mathrm{Y}\) (b) Po (c) Co (d) Es (e) \(\mathrm{Pb}\)