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Chapter 9: Problem 17

Among the following ions, several pairs are isoelectronic. Identify these pairs. \(\mathrm{Fe}^{2+}, \mathrm{Sc}^{3+}, \mathrm{Ca}^{2+}, \mathrm{F}^{-}\) \(\mathrm{Co}^{2+}, \mathrm{Co}^{3+}, \mathrm{Sr}^{2+}, \mathrm{Cu}^{+}, \mathrm{Zn}^{2+}, \mathrm{Al}^{3+}.\)

Short Answer

Expert verified
The isoelectronic pairs are (\(\mathrm{Fe}^{2+}\), \(\mathrm{Co}^{3+}\)), (\(\mathrm{Sc}^{3+}\), \(\mathrm{Ca}^{2+}\)), (\(\mathrm{F}^{-}\), \(\mathrm{Al}^{3+}\)) and (\(\mathrm{Cu}^{+}\), \(\mathrm{Zn}^{2+}\)).

Step by step solution

01

Determine the Number of Electrons in Each Ion

By summing the atomic number and the charge of the ions, the total number of electrons in each ion can be determined. Use the periodic table to find the atomic number of each element. For example, the atomic number of Fe is 26. Since the ion is \(\mathrm{Fe}^{2+}\), it has lost 2 electrons, so it has 24 electrons in total.
02

Repeat for All Ions

Apply the same process to all of the ions: \(\mathrm{Sc}^{3+}\) has 18 electrons, \(\mathrm{Ca}^{2+}\) has 18 electrons, \(\mathrm{F}^{-}\) has 10 electrons, \(\mathrm{Co}^{2+}\) has 25 electrons, \(\mathrm{Co}^{3+}\) has 24 electrons, \(\mathrm{Sr}^{2+}\) has 36 electrons, \(\mathrm{Cu}^{+}\) has 28 electrons, \(\mathrm{Zn}^{2+}\) has 28 electrons and \(\mathrm{Al}^{3+}\) has 10 electrons.
03

Identify Isoelectronic Pairs

Two ions are isoelectronic if they have the same number of electrons. From the calculations carried out, the isoelectronic pairs can therefore be identified as (\(\mathrm{Fe}^{2+}\), \(\mathrm{Co}^{3+}\)), (\(\mathrm{Sc}^{3+}\), \(\mathrm{Ca}^{2+}\)), (\(\mathrm{F}^{-}\), \(\mathrm{Al}^{3+}\)) and (\(\mathrm{Cu}^{+}\), \(\mathrm{Zn}^{2+}\)).

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Most popular questions from this chapter

Plot a graph of the square roots of the ionization energies versus the nuclear charge for the two series \(\mathrm{Li}, \mathrm{Be}^{+}, \mathrm{B}^{2+}, \mathrm{C}^{3+},\) and \(\mathrm{Na}, \mathrm{Mg}^{+}, \mathrm{Al}^{2+}, \mathrm{Si}^{3+} .\) Explain the observed relationship with the aid of Bohr's expression for the binding energy of an electron in a one electron atom.

Use principles established in this chapter to arrange the following atoms in order of increasing value of the first ionization energy: $\mathrm{Sr}, \mathrm{Cs}, \mathrm{S}, \mathrm{F}, \mathrm{As}.$

Two elements, \(A\) and \(B\), have the electron configurations shown. $$ \mathrm{A}=\left[\begin{array}{ll} \mathrm{Ar} & 4 s^{1} \end{array} \quad \mathrm{B}=\left[\begin{array}{l} \mathrm{Ar} \end{array}\right] 3 d^{10} 4 \mathrm{s}^{2} 4 p^{3}\right. $$ (a) Which element is a metal? (b) Which element has the greater ionization energy? (c) Which element has the larger atomic radius? (d) Which element has the greater electron affinity?

Briefly describe each of the following ideas or phenomena: (a) the periodic law; (b) ionization energy; (c) electron affinity; (d) paramagnetism.

For the atom \(^{119} \mathrm{Sn}\), indicate the number of (a) protons in the nucleus; (b) neutrons in the nucleus; (c) \(4 d\) electrons; (d) 3s electrons; (e) 5 \(p\) electrons; (f) electrons in the valence shell.
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