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Chapter 12: Problem 12

Silicon is the fundamental component of integrated circuits. Si has the same structure as diamond. (a) Is Si a molecular, metallic, ionic, or covalent- network solid? (b) Silicon readily reacts to form silicon dioxide, \(\mathrm{SiO}_{2,}\) which is quite hard and is insoluble in water. Is \(\mathrm{SiO}_{2}\) most likely a molecular, metallic, ionic, or covalent- network solid?

Short Answer

Expert verified
(a) Si is a covalent-network solid. (b) SiO2 is a covalent-network solid.

Step by step solution

01

Determine the elements in Silicon (Si)

Silicon is a single element with the chemical symbol Si. It is in Group 14 of the periodic table, which means it has 4 valence electrons. The diamond-like structure of Silicon implies that it has a strong covalent bonding.
02

Identify the type of bonding in Silicon (Si)

Silicon forms covalent bonds with other Silicon atoms due to its 4 valence electrons. These bonds result in a covalent-network structure, similar to that of diamond.
03

Classify Silicon (Si) as a type of solid

Since Silicon has a covalent-network structure formed by covalent bonds, it is considered a covalent-network solid. So, answer (a) is that Si is a covalent-network solid. #Determine the classification of Silicon dioxide (SiO2) solid#
04

Determine the elements in Silicon Dioxide (SiO2)

Silicon Dioxide consists of Silicon (Si) and Oxygen (O) elements. It has the chemical formula SiO2, which indicates that there is one Silicon atom and two Oxygen atoms in each molecule.
05

Identify the type of bonding in Silicon Dioxide (SiO2)

Silicon and Oxygen both form covalent bonds to create a stable structure for SiO2. Each Silicon atom bonds with two Oxygen atoms in a tetrahedral arrangement, which results in a tightly bonded covalent-network structure.
06

Classify Silicon Dioxide (SiO2) as a type of solid

Since Silicon Dioxide has a covalent-network structure formed by covalent bonds, it is considered a covalent-network solid. So, answer (b) is that SiO2 is a covalent-network solid.

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Most popular questions from this chapter

At room temperature and pressure RbCl crystallizes with the NaCl-type structure. (a) Use ionic radii to predict the length of the cubic unit cell edge. (b) Use this value to estimate the density. (c) At high temperature and pressure, the structure transforms to one with a CsCl-type structure. Use ionic radii to predict the length of the cubic unit cell edge for the high- pressure form of RbCl. (d) Use this value to estimate the density. How does this density compare with the density you calculated in part (b)?

Determine if each statement is true or false: (a) Substitutional alloys are solid solutions, but interstitial alloys are heterogenous alloys. (b) Substitutional alloys have "solute" atoms that replace "solvent" atoms in a lattice, but interstitial alloys have "solute" atoms that are in between the "solvent" atoms in a lattice. (c) The atomic radii of the atoms in a substitutional alloy are similar to each other, but in an interstitial alloy, the interstitial atoms are a lot smaller than the host lattice atoms.

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