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Chapter 11: Problem 97

The best electrical conductor of the following materials is (a) \(\mathrm{Li}(\mathrm{s}) ;\) (b) \(\mathrm{Br}_{2}(\mathrm{l}) ;\) (c) \(\mathrm{Ge}(\mathrm{s}) ;\) (d) \(\mathrm{Si}(\mathrm{s})\).

Short Answer

Expert verified
The best electrical conductor among the given elements is Lithium (Li).

Step by step solution

01

Analyze the Element Types

The elements given in the question are Lithium(Li), Bromine(Br), Germanium(Ge), and Silicon(Si). Lithium is a metal, Bromine is a halogen, and Germanium and Silicon are metalloids. In general, metals are good conductors of electricity, halogens are poor conductors, and metalloids have intermediate conductivity.
02

Compare the Conductivity

Among all these elements, Lithium, being a metal, is the best electrical conductor. Metals have free electrons that can move easily, which makes them good conductors of electricity. On the other hand, bromine being a halogen is a poor conductor. Germanium and Silicon being metalloids have intermediate conductivity.
03

Conclusion

With the given information, it can be concluded that among the given elements Lithium (Li) is the best conductor of electricity.

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Most popular questions from this chapter

Consider the molecules \(\mathrm{CO}^{+}\) and \(\mathrm{CN}^{-}\) and use molecular orbital theory to answer the following: (a) Write the molecular orbital configuration of each ion (ignore the 1 s electrons). (b) Predict the bond order of each ion. (c) Which of these ions is paramagnetic? Which is diamagnetic? (d) Which of these ions do you think has the greater bond length? Explain.

Use the valence molecular orbital configuration to determine which of the following species is expected to have the lowest ionization energy: (a) \(\mathrm{C}_{2}^{+} ;\) (b) \(\mathrm{C}_{2}\) (c) \(\mathrm{C}_{2}^{-}\)

The ion \(\mathrm{F}_{2} \mathrm{Cl}^{-}\) is linear, but the ion \(\mathrm{F}_{2} \mathrm{Cl}^{+}\) is bent. Describe hybridization schemes for the central \(\mathrm{Cl}\) atom consistent with this difference in structure.

Match each of the following species with one of these hybridization schemes: \(s p, s p^{2}, s p^{3}, s p^{3} d, s p^{3} d^{2} .\) (a) \(\mathrm{PF}_{6}^{-}\) (b) \(\operatorname{COS} ;\) (c) \(\operatorname{SiCl}_{4} ;\) (d) \(\mathrm{NO}_{3}^{-}\);(e) AsF \(_{5}\)

\(\mathrm{He}_{2}\) does not exist as a stable molecule, but there is evidence that such a molecule can be formed between electronically excited He atoms. Write a molecular orbital diagram to account for this.
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