Problem 82
The ground-state electron configurations listed here are incorrect. Explain what mistakes have been made in each and write the correct electron configurations. Al: \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{2} 3 p^{3}\) B: \(1 s^{2} 2 s^{2} 2 p^{5}\) \(\mathrm{F}: 1 s^{2} 2 s^{2} 2 p^{6}\)
Problem 83
Indicate the number of unpaired electrons present in each of the following atoms: \(\mathrm{B}, \mathrm{Ne}, \mathrm{P}, \mathrm{Sc}, \mathrm{Mn}, \mathrm{Se}, \mathrm{Kr}\) \(\mathrm{Fe}, \mathrm{Cd}, \mathrm{I}, \mathrm{Pb}\).
Problem 84
The electron configuration of a neutral atom is \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}\). Write a complete set of quantum numbers for each of the electrons. Name the element.
Problem 85
Which of the following species has the greatest number of unpaired electrons: \(\mathrm{S}^{+}, \mathrm{S},\) or \(\mathrm{S}^{-} ?\)
Problem 87
Describe the characteristics of transition metals.
Problem 88
What is the noble gas core? How does it simplify the writing of electron configurations?
Problem 89
What are the group and period of the element osmium?
Problem 90
Define the following terms and give an example of each: lanthanides actinides
Problem 91
Explain why the ground-state electron configurations of \(\mathrm{Cr}\) and \(\mathrm{Cu}\) are different from what we might expect.
Problem 93
Comment on the correctness of the following statement: The probability of finding two electrons with the same four quantum numbers in an atom is zero.
