7th Edition

ISBN: 9781119497325

Author: JESPERSEN

Publisher: WILEY

Concept explainers

Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be ne…

Polarity Of Water

In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in t…

Valence Bond Theory Vbt

Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the forma…

Videos

Textbook Question

Chapter 8, Problem 55RQ

Sketch the structures for (a) methane, (b) ethane, and (c) propane.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Chapter 8, Problem 54RQ

Chapter 8, Problem 56RQ

Students have asked these similar questions

For the four classes of hydrocarbons (Alkane, Alkene, Alkyne, Arene): Give a structural formula example of each, or identify the characteristic bond that is present.

Draw the shapes of the following molecules and ions in 3-dimension. Show clearly any lone pairs of electrons on the central atom, state the number of bond pairs and lone pairs of electrons on the central atom and name the shape of the molecule or ion. (a) SiCI4, silicon tetrachloride (b) PBr3, phosphorus tribromide (c) CI2O, dichlorine oxide Provide everything stated in the instructions for each compound.

The partial Lewis structure that follows is for a hydrocarbonmolecule. In the full Lewis structure, each carbon atomsatisfies the octet rule, and there are no unshared electronpairs in the molecule. The carbon—carbon bondsare labeled 1, 2, and 3. (a) How many hydrogen atomsare in the molecule? (b) Rank the carbon–carbonbonds in order of increasing bond length. (c) Whichcarbon—carbon bond is the strongest one? [Sections 8.3and 8.8]

Chapter 8 Solutions

CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS

Ch. 8 - Practice Exercise 8.1 Choose the ionic compound...Ch. 8 - Construct an energy diagram similar to the one in...Ch. 8 - What is wrong with the following electron...Ch. 8 - How do the electron configurations change when a...Ch. 8 - Practice Exercise 8.5 How are the electron...Ch. 8 - Practice Exercise 8.6 Draw the Lewis structures...Ch. 8 - Practice Exercise 8.7 Use Lewis symbols to diagram...Ch. 8 - Prob. 8PE Ch. 8 - Prob. 9PE Ch. 8 - For each atom that does not have an octet, how...

Ch. 8 - The chlorine end of the chlorine monoxide molecule...Ch. 8 - Although isolated Na+ and Cl- ions are unstable,...Ch. 8 - Bromine and chlorine form a molecular substance...Ch. 8 - Practice Exercise 8.14 For each of the following...Ch. 8 - Prob. 15PE Ch. 8 - Draw Lewis structures for...Ch. 8 - Practice Exercise 8.17 Using the structures drawn...Ch. 8 - Practice Exercise 8.18 A student drew the...Ch. 8 - Assign formal charges to the atoms in the...Ch. 8 - Practice Exercise 8.20 Draw the preferred Lewis...Ch. 8 - Prob. 21PE Ch. 8 - Practice Exercise 8.22 Use Lewis structures to...Ch. 8 - Prob. 23PE Ch. 8 - Practice Exercise 8.24 Draw the resonance...Ch. 8 - Determine the preferred Lewis structure for the...Ch. 8 - Prob. 26PE Ch. 8 - Practice Exercise 8.27 The following questions...Ch. 8 - What must be true about the change in the total...Ch. 8 - 8.2 Under what conditions could a compound form...Ch. 8 - 8.3 What is an ionic bond? Ch. 8 - Define the term lattice energy. In what ways does...Ch. 8 - How is the tendency to form ionic bonds related to...Ch. 8 - What influence do ion size and charge have on...Ch. 8 - 8.7 What is the octet rule? What is responsible...Ch. 8 - 8.8 Why doesn’t hydrogen obey the octet rule? Ch. 8 - 8.9 Magnesium forms compounds containing the ion ...Ch. 8 - Prob. 10RQ Ch. 8 - Why do many of the transition elements in Period 4...Ch. 8 - Prob. 12RQ Ch. 8 - Prob. 13RQ Ch. 8 - Which of these Lewis symbols is incorrect?Ch. 8 - Define bond length and bond energy.Ch. 8 - 8.16 Define bond order. How are bond energy and...Ch. 8 - 8.17 The energy required to break the H—Cl bond to...Ch. 8 - In terms of the potential energy change, why...Ch. 8 - Prob. 19RQ Ch. 8 - Describe what happens to the electron density...Ch. 8 - Is the formation of a covalent bond endothermic or...Ch. 8 - What factors control the bond length in a covalent...Ch. 8 - How many covalent bonds are normally formed by (a)...Ch. 8 - What is a polar covalent bond?Ch. 8 - Define dipole moment in the form of an equation....Ch. 8 - 8.26 Define electronegativity. On what basis did...Ch. 8 - Which element has the highest electronegativity?...Ch. 8 - Prob. 28RQ Ch. 8 - If an element has a low electronegativity, is it...Ch. 8 - In what groups in the periodic table are the most...Ch. 8 - How is the electronegativity of a metal related to...Ch. 8 - 8.32 When we say that aluminum is more reactive...Ch. 8 - Arrange the following metals in their approximate...Ch. 8 - 8.34 Complete and balance the following equations....Ch. 8 - Prob. 35RQ Ch. 8 - Without looking at the text, describe the steps...Ch. 8 - 8.37 Why do we usually place the least...Ch. 8 - Why do Period 2 elements never form more than four...Ch. 8 - Define (a) single bond, (b) double bond, and (c)...Ch. 8 - Prob. 40RQ Ch. 8 - How many electrons are in the valence shells of...Ch. 8 - What is the minimum number of electrons that would...Ch. 8 - 8.43 Nitrogen and arsenic are in the same group in...Ch. 8 - 8.44 What is the definition of formal charge? How...Ch. 8 - How are formal charges for atoms in a molecule...Ch. 8 - 8.46 How are formal charges used to select the...Ch. 8 - 8.47 What are the formal charges on the atoms in...Ch. 8 - What is a coordinate covalent bond?Ch. 8 - Once formed, how (if at all) does a coordinate...Ch. 8 - BC13 has an incomplete valence shell. Use Lewis...Ch. 8 - Prob. 51RQ Ch. 8 - 8.52 What is a resonance hybrid? How does it...Ch. 8 - Prob. 53RQ Ch. 8 - Polystyrene plastic is a hydrocarbon that consists...Ch. 8 - Sketch the structures for (a) methane, (b) ethane,...Ch. 8 - Draw the structure for a hydrocarbon that has a...Ch. 8 - How many different molecules have the formula...Ch. 8 - What is a carbonyl group? In which classes of...Ch. 8 - Prob. 59RQ Ch. 8 - 8.60 Write a chemical equation for the ionization...Ch. 8 - Match the compounds on the left with the family...Ch. 8 - Prob. 62RQ Ch. 8 - In each of the following pairs of compounds, which...Ch. 8 - In each of the following pairs of compounds, which...Ch. 8 - Prob. 65RQ Ch. 8 - *8.66 Use an enthalpy diagram to calculate the...Ch. 8 - Explain what happens to the electron...Ch. 8 - Describe what happens to the electron...Ch. 8 - 8.69 What are the electron configurations of the ...Ch. 8 - 8.70 What are the electron configurations of the ...Ch. 8 - Write the abbreviated electron configuration of...Ch. 8 - Write the abbreviated electron configuration of...Ch. 8 - Prob. 73RQ Ch. 8 - Prob. 74RQ Ch. 8 - Prob. 75RQ Ch. 8 - Prob. 76RQ Ch. 8 - How much energy, in joules, is required to break...Ch. 8 - How much energy is released in the formation of...Ch. 8 - The reason there is danger in exposure to...Ch. 8 - A mixture of H2andCl2 is stable, but a bright...Ch. 8 - Prob. 81RQ Ch. 8 - Use Lewis structures to diagram the formation of...Ch. 8 - Chlorine tends to form only one covalent bond...Ch. 8 - Use the octet rule to predict the formula of the...Ch. 8 - Prob. 85RQ Ch. 8 - What would be the formula for the simplest...Ch. 8 - 8.87 Use the data in Table 8.3 to calculate the...Ch. 8 - The molecule bromine monofluoride has a dipole...Ch. 8 - Prob. 89RQ Ch. 8 - 8.90 The dipole moment of HF is 1.83 D and the...Ch. 8 - Prob. 91RQ Ch. 8 - Prob. 92RQ Ch. 8 - Which of the bonds in Problem 8.91 is the most...Ch. 8 - 8.94 Which of the bonds in the Problem 8.92 is the...Ch. 8 - Draw Lewis structures for...Ch. 8 - Draw Lewis structures for...Ch. 8 - Prob. 97RQ Ch. 8 - 8.98 Draw Lewis structures for Ch. 8 - 8.99 Draw Lewis structures for (a) carbon...Ch. 8 - Draw Lewis structures for (a) selenium trioxide,...Ch. 8 - Prob. 101RQ Ch. 8 - 8.102 Draw Lewis structures for . Ch. 8 - Draw the Lewis structure for (a) CH2O (the central...Ch. 8 - Draw Lewis structures for (a) the peroxide ion,...Ch. 8 - Assign formal charges to each atom in the...Ch. 8 - 8.106 Assign formal charges to each atom in the...Ch. 8 - Draw the Lewis structure for HCIO4. Assign formal...Ch. 8 - Draw the Lewis structure for SOCl2 (sulfur bonded...Ch. 8 - Prob. 109RQ Ch. 8 - 8.110 The following are two Lewis structures that...Ch. 8 - 8.111 Use Lewis structures to show that the...Ch. 8 - Use Lewis structures to show that the reaction...Ch. 8 - Draw all of the resonance structures for the N2O4...Ch. 8 - Prob. 114RQ Ch. 8 - How should the NO bond lengths compare in the NO3...Ch. 8 - Arrange the following in order of increasing CO...Ch. 8 - 8.117 The Lewis structure of was given as but...Ch. 8 - *8.118 Use formal charges to establish the...Ch. 8 - 8.119 Give the formula and name of four different...Ch. 8 - Use data from the tables of ionization energies...Ch. 8 - 8.121 Changing to gaseous atoms requires a total...Ch. 8 - In many ways, tin(IV) chloride behaves more like a...Ch. 8 - In each pair, choose the one with the more polar...Ch. 8 - How many electrons are in the outer shell of the...Ch. 8 - Prob. 125RQ Ch. 8 - 8.126 Are the following Lewis structures...Ch. 8 - Assign formal charges to all the atoms in the...Ch. 8 - 8.128 Assign formal charges to all the atoms in...Ch. 8 - The inflation of an air bag when a car experiences...Ch. 8 - 8.130 How should the sulfur-oxygen bond lengths...Ch. 8 - What is the most reasonable Lewis structure for...Ch. 8 - Prob. 132RQ Ch. 8 - Prob. 133RQ Ch. 8 - 8.134 Below is a ball-and-stick model of a type of...Ch. 8 - 8.135 Explain why ions of the representative...Ch. 8 - Use Lewis structures to show the ionization of the...Ch. 8 - The compound below, an amine, is a weak base and...Ch. 8 - 8.138 Use Lewis structures to diagram the reaction...Ch. 8 - How many grams of water could have its temperature...Ch. 8 - Prob. 140RQ Ch. 8 - A 38.40 mg sample of an organic acid composed of...Ch. 8 - What is the average bond energy of a CC covalent...Ch. 8 - One way of estimating the electronegativity of an...Ch. 8 - 8.144 The attractions between molecules of a...Ch. 8 - The positive end of the dipole in a water molecule...Ch. 8 - In describing the structures of molecules, we use...

Additional Science Textbook Solutions

Find more solutions based on key concepts

Compare and contrast the carbon, sulfur, and nitrogen cycles in terms of the physiologies of the organisms that...

Brock Biology of Microorganisms (15th Edition)

5. When the phenotype of heterozygotes is intermediate between the phenotypes of the two homozygotes, this patt...

Biology: Life on Earth (11th Edition)

Match the following examples of mutagens. Column A Column B ___a. A mutagen that is incorporated into DNA in pl...

Microbiology: An Introduction

Practice Problem 2.21 Write bond-line formulas for four carboxylic acids with the formula.

Organic Chemistry

40. Use the Henderson–Hasselbalch equation to calculate the pH of each solution. a. a solution that is 0.145 M ...

Chemistry: A Molecular Approach (4th Edition)

The following results were obtained from a broth dilution test for microbial susceptibility. Antibiotic Concent...

Microbiology: An Introduction

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.