Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 83

What type of solid will each of the following substances form? a. \(\mathrm{CO}_{2}\) b. \(\mathrm{SiO}_{2}\) c. \(\mathrm{Si}\) d. \(\mathrm{CH}_{4}\) e. \(\mathrm{Ru}\) f. \(\mathrm{I}_{2}\) g. \(\mathrm{KBr}\) h. \(\mathrm{H}_{2} \mathrm{O}\) i. \(\mathrm{NaOH}\) j. \(\mathrm{U}\) k. \(\mathrm{CaCO}_{3}\) I. \(\mathrm{PH}_{3}\)

Short Answer

Expert verified
a. Molecular solid b. Covalent solid c. Covalent solid d. Molecular solid e. Metallic solid f. Molecular solid g. Ionic solid h. Molecular solid i. Ionic solid j. Metallic solid k. Ionic solid l. Molecular solid

Step by step solution

01

a. CO2

\(\mathrm{CO}_{2}\) is a covalent compound, consisting of a central carbon atom double bonded to two oxygen atoms. This forms a linear molecule. Since \(\mathrm{CO}_{2}\) consists of discrete molecules held together by weak London dispersion forces, it forms a molecular solid.
02

b. SiO2

\(\mathrm{SiO}_{2}\) is a covalent compound made up of a silicon atom bonded to two oxygen atoms. In a solid state, each of these atoms continues to bond covalently with other atoms, forming an extended three-dimensional network of covalent bonds. Thus, \(\mathrm{SiO}_{2}\) forms a covalent (or network) solid.
03

c. Si

Silicon is a pure element with covalent bonding between its atoms. It forms a crystal structure similar to diamond, consisting of a network of covalently bonded silicon atoms. Thus, silicon forms a covalent solid.
04

d. CH4

Methane, \(\mathrm{CH}_{4}\), is a molecular compound composed of carbon covalently bonded to four hydrogen atoms. In methane's solid form, it consists of discrete molecules held together by weak London dispersion forces, forming a molecular solid.
05

e. Ru

Ruthenium (Ru) is a metal and forms metallic bonds, which involves the sharing of free electrons among a lattice of metal atoms. Therefore, ruthenium forms a metallic solid.
06

f. I2

Iodine (I2) is a diatomic molecule held together by a covalent bond. In its solid form, discrete iodine molecules are held together by weak London dispersion forces. Therefore, iodine forms a molecular solid.
07

g. KBr

\(\mathrm{KBr}\) is an ionic compound, formed by the transfer of an electron from potassium to bromine. In the solid state, potassium and bromine ions are held together by strong electrostatic forces (ionic bonds) in a crystal lattice, making it an ionic solid.
08

h. H2O

When water (\(\mathrm{H}_{2} \mathrm{O}\)) is in the solid state (ice), it forms a molecular solid. In ice, the water molecules are held together by hydrogen bonds, which are stronger than London dispersion forces but weaker compared to covalent or ionic bonds.
09

i. NaOH

Sodium hydroxide (\(\mathrm{NaOH}\)) is an ionic compound that consists of sodium ions and hydroxide ions. These ions are held together by strong electrostatic forces (ionic bonds) in a crystal lattice, making sodium hydroxide an ionic solid.
10

j. U

Uranium (U) is a metal and forms metallic bonds, in which free electrons are shared among a lattice of metal ions. Therefore, uranium forms a metallic solid.
11

k. CaCO3

Calcium carbonate (\(\mathrm{CaCO}_{3}\)) is an ionic compound, consisting of calcium, carbon, and oxygen ions. In the solid state, these ions are held together by strong electrostatic forces (ionic bonds) in a crystal lattice, making calcium carbonate an ionic solid.
12

l. PH3

Phosphine (\(\mathrm{PH}_{3}\)) is a molecular compound composed of phosphorus covalently bonded to three hydrogen atoms. In phosphine's solid form, it consists of discrete molecules held together by weak London dispersion forces, forming a molecular solid.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Explain how a p–n junction makes an excellent rectifier

Selenium is a semiconductor used in photocopying machines. What type of semiconductor would be formed if a small amount of indium impurity is added to pure selenium?

The CsCl structure is a simple cubic array of chloride ions with a cesium ion at the center of each cubic array (see Exercise 71 ). Given that the density of cesium chloride is 3.97 \(\mathrm{g} /\) \(\mathrm{cm}^{3},\) and assuming that the chloride and cesium ions touch along the body diagonal of the cubic unit cell, calculate the distance between the centers of adjacent \(\mathrm{Cs}^{+}\) and \(\mathrm{Cl}^{-}\) ions in the solid. Compare this value with the expected distance based on the sizes of the ions. The ionic radius of \(\mathrm{Cs}^{+}\) is \(169 \mathrm{pm},\) and the ionic radius of \(\mathrm{Cl}^{-}\) is 181 \(\mathrm{pm} .\)

A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their properties, since one is a molecular solid and the other is an ionic solid. How do the properties differ and why?

Like most substances, bromine exists in one of the three typical phases. Br_ has a normal melting point of \(-7.2^{\circ} \mathrm{C}\) and a normal boiling point of \(59^{\circ} \mathrm{C}\) . The triple point for \(\mathrm{Br}_{2}\) is \(-7.3^{\circ} \mathrm{C}\) and 40 torr, and the critical point is $320^{\circ} \mathrm{C}$ and 100 atm. Using this information, sketch a phase diagram for bromine indicating the points described above. Based on your phase diagram, order the three phases from least dense to most dense. What is the stable phase of \(\mathrm{Br}_{2}\) at room temperature and 1 atm? Under what temperature conditions can liquid bromine never exist? What phase changes occur as the temperature of a sample of bromine at 0.10 atm is increased from \(-50^{\circ} \mathrm{C}\) to \(200^{\circ} \mathrm{C} ?\)
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free