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Chapter 7: Problem 70

Which of the following do you expect to be nonmolecular solids? (a) Sodium hydroxide, \(\mathrm{NaOH}\) (b) Solid ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) (c) Iron, Fe (d) Solid silane, \(\mathrm{SiH}_{4}\)

Short Answer

Expert verified
Sodium hydroxide (NaOH) and iron (Fe) are nonmolecular solids. Sodium hydroxide forms an ionic solid due to the strong electrostatic forces between its ions, while iron is a metallic solid with closely packed metal atoms held by metallic bonds.

Step by step solution

01

Sodium hydroxide (NaOH)

Sodium hydroxide consists of the positively charged sodium ion (Na+) and negatively charged hydroxide ion (OH-). These ions are held together by strong electrostatic forces, known as ionic bonds. Thus, sodium hydroxide forms an ionic solid.
02

Solid ethanol (CH3CH2OH)

Solid ethanol is made up of ethanol molecules with a hydroxyl group (OH). These molecules are held together by hydrogen bonding, a type of van der Waals interaction. As a result, solid ethanol is considered a molecular solid.
03

Iron (Fe)

Iron is a metal. Its solid consists of metal atoms closely packed together and held by metallic bonds, where the valence electrons are delocalized and shared among all atoms. Therefore, iron is a metallic solid.
04

Solid silane (SiH4)

Solid silane consists of SiH4 molecules, which are held together by weak van der Waals forces. As a result, solid silane is considered a molecular solid. Finally, to answer the question, we can see that out of the given substances, sodium hydroxide (NaOH) and iron (Fe) are nonmolecular solids - as sodium hydroxide is an ionic solid and iron is a metallic solid.

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Most popular questions from this chapter

Predict which compound in each pair will have the higher melting point, and explain why for each pair. (a) HI or KI (b) \(\mathrm{Na}_{2} \mathrm{O}\) or \(\mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{CaF}_{2}\) or \(\mathrm{HF}\) (d) \(\mathrm{SiO}_{2}\) or \(\mathrm{CO}_{2}\)

Chloromethane \(\left(\mathrm{CH}_{3} \mathrm{Cl}\right)\) has a much higher boiling point than methane \(\left(\mathrm{CH}_{4}\right)\). Give two reasons for this.

At \(25^{\circ} \mathrm{C}\), fluorine, \(\mathrm{F}_{2}\), and chlorine, \(\mathrm{Cl}_{2}\), are gases but bromine, \(\mathrm{Br}_{2}\), is a liquid. What does this say about the intermolecular forces in bromine relative to those in fluorine and chlorine?

Most covalent molecular substances have much lower melting points than ionic substances. What does this say about the strength of a covalent bond relative to the strength of an ionic bond? Explain your answer.

All of the following are solids at room temperature. Classify them as molecular, ionic, network, or metallic. (a) Potassium \((\mathrm{K}), \mathrm{mp}=64{ }^{\circ} \mathrm{C}\) (b) Potassium chloride \((\mathrm{KCl}), \mathrm{mp}=770{ }^{\circ} \mathrm{C}\) (c) Red phosphorus \((\mathrm{P}), \mathrm{mp}=590{ }^{\circ} \mathrm{C}\) (d) Boron triiodide \(\left(\mathrm{BI}_{3}\right), \mathrm{mp}=50{ }^{\circ} \mathrm{C}\)
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