Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 8, Problem 27PE
The following questions apply to the compounds in Practice Exercise 8.26. (a) Which produces a basic solution in water? (b) Which produces an acidic aqueous solution? (c) For the acid, what is the Lewis structure of the anion formed when it is neutralized? (d) For the base, what is the Lewis structure of the cation formed when it reacts with
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Write an electron configuration for each element and the corresponding Lewis structure. Indicate which electrons in the electron configuration are included in the Lewis structure.(a) N(b) C(c) Cl(d) Ar
Write electron configurations and Lewis structures for each element. Indicate which of the electrons in the electron configuration are shown in the Lewis structure.(a) Ca(b) Ga(c) As(d) I
Show how each chemical change obeys the octet rule.
(a) Hydrogen forms H2 (hydride ion)
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...
Additional Science Textbook Solutions
Find more solutions based on key concepts
Which substance is a pure compound? a. Gold b. Water c. Milk d. Fruit cake
Introductory Chemistry (5th Edition) (Standalone Book)
Calculate the lattice energy of CaCl2 using a Born-Haber cycle and data from Appendices F and L and Table 7.5. ...
Chemistry & Chemical Reactivity
1. Why is the quantum-mechanical model of the atom important for understanding chemistry?
Chemistry: Structure and Properties (2nd Edition)
The formation of cations of Scandium from orbital notation needs to be explained. Concept introduction: The ele...
Chemistry: Matter and Change
a. Draw the resonance forms for SO2 (bonded OSO). b. Draw the resonance forms for ozone (bonded OOO). c. Sulfur...
Organic Chemistry (9th Edition)
Five liters of liquid n-hexane and 4 liters of liquid n-heptane are mixed and burned with 4000 gram moles of ai...
Elementary Principles of Chemical Processes, Binder Ready Version
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.Similar questions
- Which of the following statements are true regarding the formation of an ionic bond between a metal and a nonmetal? (a) The atomic radius of a metal atom is greater than its ionic radius. (b) The atomic radius of a nonmetal atom is less than its ionic radius. (c) Energy is released in the formation of an ionic bond.arrow_forwardWhich statements are true about electronegativity? (a) Electronegativity increases from left to right in a period of the Periodic Table. (b) Electronegativity increases from top to bottom in a column of the Periodic Table . (c) Hydrogen, the element with the lowest atomic number, has the smallest electronegativity. (d) The higher the atomic number of an element, the greater its electronegativity.arrow_forwardDraw Lewis diagrams for the following ions. In the formula the symbol of the central atom is given first. (Hint:The valence octet may be expanded for the central atom.)(a) BrO4 - (b) PCl6 - (c) XeF6+arrow_forward
- Answer the following questions that relate to the chemistry of nitrogen. (a) Two nitrogen atoms combine to form a nitrogen molecule, as represented by the following equation. 2 N(g) ® N2(g) Using the table of average bond energies below, determine the enthalpy change, AH, for the reaction. Average Bond Energy (k) mol-1) Bond N-N 160 N=N 420 N°N 950 (b) The reaction between nitrogen and hydrogen to form ammonia is represented below. N2(g) + 3 H2(g)® 2 NH3(g) AH° = -92.2 kJ Predict the sign of the standard entropy change, AS', for the reaction. Justify your answer. (C) The value of AG° for the reaction represented in part (b) is negative at low temperatures but positive at high temperatures. Explain.arrow_forward7. Consider the following compounds: BaBr 2, MgCl 2, and SrCl 2. Answer the following questions based on expected periodic trends: (a) Which is expected to have the shortest ionic bonds? (b) Which is expected to have the highest lattice energy? (c) Which is expected to have the lowest melting point?arrow_forwardA resident expert on electronegativity comes up to visit with you. He makes two claims (seen below) about electronegativity with relation to covalent bonding. Is the expert correct or can you refute him with your knowledge of electronegativity? (a) If a diatomic molecule is made up of atoms X and Y, which have different electronegativities, the molecule must be polar. (b) The farther two atoms are apart in a bond, the larger the dipole moment will be.arrow_forward
- In the vapor phase, BeCl2 exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule? (b) What other resonance structures are possible that satisfy the octet rule? (c) On the basis of the formal charges, which Lewis structure is expected to be dominant for BeCl2?arrow_forwardWrite the Lewis dot symbols of the reactants and products in the followingreactions. (First balance the equations.)(a) Sr + Se → SrSe(b) Ca + H2 → CaH2(c) Li + N2 → Li3N(d) Al + S → Al2S3arrow_forwardWhere in the periodic table are the most electronegative elements found, and where are the least electronegative elements found?arrow_forward
- 1. Hydrogen (H2) and oxygen (O2) react to produce water (H2O). (a) Write down the equation for the above reaction. (b) The enthalpy change of reaction is –286 kJ mol-!. Is the reaction endothermic or exothermic? (c) What kinds of bonds are broken during the reaction? (d) What kinds of bonds are formed during the reaction? (e) Construct a diagram showing the change in enthalpy for the reaction.arrow_forwardWhich pair of elements has the most similar Lewis structures?(a) N and S (b) F and Ar(c) Cl and Ar (d) O and Sarrow_forwardWhich of the following statements about electronegativity isfalse? (a) Electronegativity is the ability of an atom in a moleculeto attract electron density toward itself. (b) Electronegativity isthe same thing as electron affinity. (c) The numerical valuesfor electronegativity have no units. (d) Fluorine is the mostelectronegative element. (e) Cesium is the least electronegativeelement.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Types of bonds; Author: Edspira;https://www.youtube.com/watch?v=Jj0V01Arebk;License: Standard YouTube License, CC-BY