Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Textbook Question
Chapter 8, Problem 25RQ
Define dipole moment in the form of an equation. What is the value of the debye (with appropriate units)?
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Chapter 8 Solutions
Chemistry: The Molecular Nature of Matter
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. 8PECh. 8 - Prob. 9PECh. 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. 15PECh. 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. 21PECh. 8 - Practice Exercise 8.22
Use Lewis structures to...Ch. 8 - Prob. 23PECh. 8 - Practice Exercise 8.24
Draw the resonance...Ch. 8 - Determine the preferred Lewis structure for the...Ch. 8 - Prob. 26PECh. 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. 10RQCh. 8 - Why do many of the transition elements in Period 4...Ch. 8 - Prob. 12RQCh. 8 - Prob. 13RQCh. 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. 19RQCh. 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. 28RQCh. 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. 35RQCh. 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. 40RQCh. 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. 51RQCh. 8 - 8.52 What is a resonance hybrid? How does it...Ch. 8 - Prob. 53RQCh. 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. 59RQCh. 8 - 8.60 Write a chemical equation for the ionization...Ch. 8 - Match the compounds on the left with the family...Ch. 8 - Prob. 62RQCh. 8 - In each of the following pairs of compounds, which...Ch. 8 - In each of the following pairs of compounds, which...Ch. 8 - Prob. 65RQCh. 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. 73RQCh. 8 - Prob. 74RQCh. 8 - Prob. 75RQCh. 8 - Prob. 76RQCh. 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. 81RQCh. 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. 85RQCh. 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. 89RQCh. 8 - 8.90 The dipole moment of HF is 1.83 D and the...Ch. 8 - Prob. 91RQCh. 8 - Prob. 92RQCh. 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. 97RQCh. 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. 101RQCh. 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. 109RQCh. 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. 114RQCh. 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. 125RQCh. 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. 132RQCh. 8 - Prob. 133RQCh. 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. 140RQCh. 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...
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- In the gas phase, positive and negative ions form ion pairs that are like molecules. An example is KF, which is found to have a dipole moment of 28.7 1030 C m and a distance of separation between the two ions of 217.2 pm. Use this information and the definition of dipole moment to calculate the partial charge on each atom. Compare your result with the expected charge, which is the charge on an electron, 1.602 1019 C. Based on your result, is KF really completely ionic?arrow_forwardThe molecule XCl2 has a dipole moment. Is X beryllium or sulfur?arrow_forwardComplete the table on next page.arrow_forward
- The molecule XF3 has a dipole moment. Is X boron or phosphorus?arrow_forwardOn the basis of the electronegativity values given in Fig. 12.3. indicate which is the more polar bond in each of the following pairs. msp;a.OClorOBrc.PSorPOb.NOorNFd.HOorHNarrow_forwardA hypothetical covalent molecule, X–Y, has a dipole moment of 1.12D and a bond length of 101 pm. Calculate the partial charge on a pole of this molecule in terms of e, where e is the charge on an electron.arrow_forward
- Show how the bond dipole moments (and those of any nonbonding pairs of electrons) contribute to the molecular dipole moment.arrow_forwardHow many valence electrons does IOF5 have? A) 34 B) 46 C) 48 D) 50 A student chemist hears the following explanation: "an object with small specific heat can be heated or cooled quickly as its temperature changes by small amount of heat. It is interesting that heating or cooling an object with large specific heat takes longer". The understanding is that embraces the amount of heat required for raising temperature of an object per FIDE unit mass by A) boiling point, specific heat capacity B) melting point, unit temperature C) specific heat capacity, unit temperature D) freezing point, specific heat capacityarrow_forwardCarbon tetrafluoride (CF4) is a non-polar molecule. Which of the following is not a factor that accounts for its non-polarity?arrow_forward
- (a) How does a polar molecule differ from a nonpolar one? (b) Atoms X and Y have different electronegativities. Will the diatomic molecule X—Y necessarily be polar? Explain. (c) What factors affect the size of the dipole moment of a diatomic molecule?arrow_forwardWhy is the concept of hybridization important in understanding bond angle and polarity? Explain thoroughly.arrow_forwardA student makes the following statement, the shape of water is tetrahedral because the four electron pairs about oxygen are approximately 109.5 apart and point to the corners of a tetrahedron. What misconceptions does this statement convey.arrow_forward
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