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Chapter 9: Problem 48

Which of the following ions are likely to be found in chemical compounds: \(\mathrm{Na}^{2+}, \mathrm{Li}^{+}, \mathrm{Al}^{4+}, \mathrm{F}^{2-},\) or \(\mathrm{Te}^{2-} ?\) Explain briefly.

Short Answer

Expert verified
\(\mathrm{Li}^{+}\) and \(\mathrm{Te}^{2-}\) are the ions likely to be found in chemical compounds.

Step by step solution

01

Analyze the Sodium Ion

Sodium (\(\mathrm{Na}\)) normally has an oxidation number of +1 since it has one electron in its outer shell that it easily gives away to reach a stable, full shell. Therefore, \(\mathrm{Na}^{2+}\) is not a common ion.
02

Analyze the Lithium Ion

Similar to sodium, Lithium (\(\mathrm{Li}\)) has one electron in its outer shell. Therefore, \(\mathrm{Li}^{+}\) is a common ion.
03

Analyze the Aluminium Ion

Aluminium (\(\mathrm{Al}\)) has three electrons in its outer shell. Therefore, \(\mathrm{Al}^{3+}\) is a common ion, not \(\mathrm{Al}^{4+}\).
04

Analyze the Fluorine Ion

Fluorine (\(\mathrm{F}\)) has seven electrons in its outer shell and typically gains one electron to reach a stable, full shell. Therefore, \(\mathrm{F}^{1-}\) is a common ion, not \(\mathrm{F}^{2-}\).
05

Analyze the Tellurium Ion

Tellurium (\(\mathrm{Te}\)) is in the same group as oxygen and sulfur and typically forms a 2- charge by gaining two electrons. Therefore, \(\mathrm{Te}^{2-}\) is a common ion.

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Most popular questions from this chapter

For the following groups of elements, select the one that has the property noted: (a) the largest atom: \(\mathrm{Mg}, \mathrm{Mn}, \mathrm{Mo}, \mathrm{Ba}, \mathrm{Bi}, \mathrm{Br}.\) (b) the lowest first ionization energy: \(\mathrm{B}, \mathrm{Sr}, \mathrm{Al}, \mathrm{Br}\) \(\mathrm{Mg}_{\ell} \mathrm{Pb}.\) (c) the most negative electron affinity: \(\mathrm{As}, \mathrm{B}, \mathrm{Cl}\) \(\mathrm{K}, \mathrm{Mg}, \mathrm{S}.\) (d) the largest number of unpaired electrons: \(\mathrm{F}, \mathrm{N}, \mathrm{S}^{2-}, \mathrm{Mg}^{2+}, \mathrm{Sc}^{3+}, \mathrm{Ti}^{3+}.\)

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.

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.

Two elements, \(A\) and \(B\), have the electron configurations shown. $$ \mathrm{A}=[\mathrm{Kr}] 4 s^{2} \quad \mathrm{B}=[\mathrm{Ar}] 3 d^{10} 4 s^{2} 4 p^{5} $$ (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?

Must all atoms with an odd atomic number be paramagnetic? Must all atoms with an even atomic number be diamagnetic? Explain.
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