Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
Question
Chapter 9, Problem 46QAP

(a)

Interpretation Introduction

Interpretation: The formula of a solid polar molecule containing oxygen should be determined.

Concept Introduction : The solid substances are classified as molecular and non-molecular in nature. The molecular solids can be polar and non-polar in nature. In a polar molecule, one side of molecule is negatively charged, whereas the other one is positively charged. When these opposite charged molecules come in contact, they exert a dipole-dipole interaction and hydrogen bonding to form a polar bond. Similarly, non-polar molecules do not have a separation between negative and positively charged sides. The solids containing these types of bonds are identified as polar and non-polar solids respectively.

Ionic bonds are formed between the atoms of two species having opposite charges. In such bonds, the excess electrons from one atom are donated to the adjoining atom in order to stabilize the molecule/compound. They are mostly formed between a metal and non-metal.

Network covalent or covalent bonds are formed when atoms of various species share the electrons in their outer orbital. It has very low polarity and the bonds are formed between species with almost similar electro-negativity.

(a)

Expert Solution
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Answer to Problem 46QAP

An example of polar molecular solid is nitrogen monoxide, NO .

Explanation of Solution

Nitrogen monoxide ( NO )

  1. The number of valence electrons of both species.
  2. Nitrogen (N) has 5 valence electrons and Oxygen (O) has six valence electrons.

  3. The formation of double bond between N and O takes place by sharing of four electrons between them. And rest of the valence electrons are present as lone pair electrons
  4. Using the Lewis dot structure of NO will be:
  5.   Chemistry: Principles and Reactions, Chapter 9, Problem 46QAP , additional homework tip  1

Since, O is most electronegative than N so, it has tendency to attract the shared pair of electron towards them and possess the negative charge, whereas the N will possess positive charge.

This proves that the charges are unevenly distributed and hence, this molecule is polar in nature.

(b)

Interpretation Introduction

Interpretation: The formula of a solid ionic compound containing oxygen should be determined.

Concept Introduction : The solid substances are classified as molecular and non-molecular in nature. The molecular solids can be polar and non-polar in nature. In a polar molecule, one side of molecule is negatively charged, whereas the other one is positively charged. When these opposite charged molecules come in contact, they exert a dipole-dipole interaction and hydrogen bonding to form a polar bond. Similarly, non-polar molecules do not have a separation between negative and positively charged sides. The solids containing these types of bonds are identified as polar and non-polar solids respectively.

Ionic bonds are formed between the atoms of two species having opposite charges. In such bonds, the excess electrons from one atom are donated to the adjoining atom in order to stabilize the molecule/compound. They are mostly formed between a metal and non-metal.

Network covalent or covalent bonds are formed when atoms of various species share the electrons in their outer orbital. It has very low polarity and the bonds are formed between species with almost similar electro-negativity.

(b)

Expert Solution
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Answer to Problem 46QAP

An example of ionic solid is calcium oxide, CaO .

Explanation of Solution

Calcium Oxide ( CaO )

  1. The first rule of an ionic bond is that it occurs between metal (Ca) and non-metal (O) by transfer of valence electrons.
  2. Using the Lewis dot structure, calcium (Ca) has 2 valence electrons and oxygen (O) has 6 valence electrons. Using a single bond, Ca donates its 2 valence electrons to O and thus Ca gains (+2, positive ion) charge, whereas O get (-2, negative ion) charge. As they combine through opposite charges (complete transfer of electrons), an ionic bond is formed.
  3.   Chemistry: Principles and Reactions, Chapter 9, Problem 46QAP , additional homework tip  2

(c)

Interpretation Introduction

Interpretation: The formula of a solid network covalent molecule containing oxygen should be determined.

Concept Introduction : The solid substances are classified as molecular and non-molecular in nature. The molecular solids can be polar and non-polar in nature. In a polar molecule, one side of molecule is negatively charged, whereas the other one is positively charged. When these opposite charged molecules come in contact, they exert a dipole-dipole interaction and hydrogen bonding to form a polar bond. Similarly, non-polar molecules do not have a separation between negative and positively charged sides. The solids containing these types of bonds are identified as polar and non-polar solids respectively.

Ionic bonds are formed between the atoms of two species having opposite charges. In such bonds, the excess electrons from one atom are donated to the adjoining atom in order to stabilize the molecule/compound. They are mostly formed between a metal and non-metal.

Network covalent or covalent bonds are formed when atoms of various species share the electrons in their outer orbital. It has very low polarity and the bonds are formed between species with almost similar electro-negativity.

(c)

Expert Solution
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Answer to Problem 46QAP

An example of network covalent solid is quartz, SiO2 .

Explanation of Solution

Quartz ( SiO2 )

  1. Silicon has four valence electrons and two atoms of oxygen gives a total of 12 valence electrons. The total number of valence electrons is thus (12+4= 16). So, either Silicon can take four electrons from Oxygen or Oxygen gains all the four electrons of Silicon thereby leaving it without any electrons.
  2. From the Lewis structure, it is evident that the four electrons that Si requires are shared by the outer orbital of adjoining oxygen atoms. Thus covalent bonds are formed. Apart from the given form, SiO2 can also exist like a grid containing repetitive units of Si and O such that its bond sharing continues through the substance.
  3.   Chemistry: Principles and Reactions, Chapter 9, Problem 46QAP , additional homework tip  3

(d)

Interpretation Introduction

Interpretation: The formula of a non-polar molecule containing oxygen should be determined.

Concept Introduction : The solid substances are classified as molecular and non-molecular in nature. The molecular solids can be polar and non-polar in nature. In a polar molecule, one side of molecule is negatively charged, whereas the other one is positively charged. When these opposite charged molecules come in contact, they exert a dipole-dipole interaction and hydrogen bonding to form a polar bond. Similarly, non-polar molecules do not have a separation between negative and positively charged sides. The solids containing these types of bonds are identified as polar and non-polar solids respectively.

Ionic bonds are formed between the atoms of two species having opposite charges. In such bonds, the excess electrons from one atom are donated to the adjoining atom in order to stabilize the molecule/compound. They are mostly formed between a metal and non-metal.

Network covalent or covalent bonds are formed when atoms of various species share the electrons in their outer orbital. It has very low polarity and the bonds are formed between species with almost similar electro-negativity.

(d)

Expert Solution
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Answer to Problem 46QAP

An example of the non-polar case is solid oxygen molecule, O2 .

Explanation of Solution

Oxygen molecule ( O2 )

  1. The first rule on non-polar molecule is that it must have an even distribution of charge.
  2. The number of valence electrons of oxygen is six. Using a double bond (where one bond refers to two electrons) both atoms can satisfy the octet rule and the molecule is uniformly charged. Hence, it is a non-polar molecule.
  3. Although, oxygen is naturally in gaseous form, yet solid oxygen can form at a temperature below -219oC.

Lewis dot structure of O2 molecule:

  Chemistry: Principles and Reactions, Chapter 9, Problem 46QAP , additional homework tip  4

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Chapter 9 Solutions

Chemistry: Principles and Reactions

Ch. 9 - At a resort in Sante Fe, New Mexico, the...Ch. 9 - Prob. 12QAPCh. 9 - Prob. 13QAPCh. 9 - Consider the following data for the vapor pressure...Ch. 9 - Referring to Figure 9.7, state what phase(s)...Ch. 9 - Referring to Figure 9.7, state what phase(s) is...Ch. 9 - Prob. 17QAPCh. 9 - Consider the phase diagram of the compound in...Ch. 9 - Prob. 19QAPCh. 9 - Prob. 20QAPCh. 9 - Given the following data about xenon,...Ch. 9 - Given the following data about CO2: • triple...Ch. 9 - A pure substance X has the following properties:...Ch. 9 - Prob. 24QAPCh. 9 - Prob. 25QAPCh. 9 - Arrange the following compounds in order of...Ch. 9 - Which of the following would you expect to show...Ch. 9 - Which of the following compounds would you expect...Ch. 9 - Prob. 29QAPCh. 9 - Prob. 30QAPCh. 9 - Explain in terms of forces between structural...Ch. 9 - Prob. 32QAPCh. 9 - Prob. 33QAPCh. 9 - In which of the following processes is it...Ch. 9 - For each of the following pairs, choose the member...Ch. 9 - Follow the directions for Question 35 for the...Ch. 9 - What are the strongest attractive forces that must...Ch. 9 - What are the strongest attractive forces that must...Ch. 9 - Prob. 39QAPCh. 9 - Prob. 40QAPCh. 9 - Of the four general types of solids, which one(s)...Ch. 9 - Of the four general types of solids, which one(s)...Ch. 9 - Prob. 43QAPCh. 9 - Prob. 44QAPCh. 9 - Give the formula of a solid containing Si that is...Ch. 9 - Prob. 46QAPCh. 9 - Prob. 47QAPCh. 9 - Describe the structural units in (a) C (graphite)...Ch. 9 - Molybdenum has an atomic radius of 0.145 nm. The...Ch. 9 - Nickel has an atomic radius of 0.162 nm. The edge...Ch. 9 - Lead (atomicradius=0.181nm) crystallizes with a...Ch. 9 - Iridium crystallizes in a face-centered unit cell....Ch. 9 - In the LiCl structure shown in Figure 9.21, the...Ch. 9 - Potassium iodide has a unit cell similar to that...Ch. 9 - Prob. 55QAPCh. 9 - Consider the CsCl cell (Figure 9.21). The ionic...Ch. 9 - Consider the sodium chloride unit cell shown in...Ch. 9 - Consider the CsCl unit shown in Figure 9.21. How...Ch. 9 - A 1.25-L clean and dry flask is sealed. The air in...Ch. 9 - Aluminum metal crystallizes with a face-centered...Ch. 9 - Consider a sealed flask with a movable piston that...Ch. 9 - Prob. 62QAPCh. 9 - Prob. 63QAPCh. 9 - Prob. 64QAPCh. 9 - Chloroform, CHCl3, has a normal boiling point of...Ch. 9 - Prob. 66QAPCh. 9 - Prob. 67QAPCh. 9 - In the blanks provided, answer the questions...Ch. 9 - Answer the questions below, by filling in the...Ch. 9 - Prob. 70QAPCh. 9 - Prob. 71QAPCh. 9 - What is the difference between (a) a covalent bond...Ch. 9 - Four shiny solids are labeled A, B, C, and D....Ch. 9 - Prob. 74QAPCh. 9 - The following data are given for CC14:...Ch. 9 - Iron crystallizes in a body-centered unit cell....Ch. 9 - Prob. 77QAPCh. 9 - Trichloroethane, C2H3Cl3, is the active ingredient...Ch. 9 - Prob. 79QAPCh. 9 - Prob. 80QAPCh. 9 - Prob. 81QAP
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