CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
7th Edition
ISBN: 9781119497325
Author: JESPERSEN
Publisher: WILEY
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Textbook Question
Chapter 8, Problem 77RQ
How much energy, in joules, is required to break the bond in one chlorine molecule? The bond energy of
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A scientist studies the bond energies of different compounds containing nitrogen (N). The scientist observes that the N–N bonds in one group of compounds have a bond energy of 209 kJ/mol, while the N–N bonds in another group of compounds have a bond energy of 418 kJ/mol. In one or two sentences, postulate a reason for this difference.
An experiment was conducted to determine the Cl - Cl bond energy in chlorine. It was determined the minimum energy required to break a Cl - Cl bond was 3.90 x 10-19 J. According to these experimental results, what is the Cl - Cl bond energy (in kJ/mol)?
A certain element X forms two compounds with hydrogen, XH3 and X2H4 (H2X–XH2). The total bond enthalpies of XH3(g) and X2H4(g) are 846 kJ/mol and 1341 kJ/mol, respectively. What is the average bond enthalpy of the X–X bond?
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. 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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