Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 3, Problem 3.17P
Explain the following:
a.
b.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
This thermodynamic cycle describes the formation of an ionic compound MX from a metal element M and nonmetal element X in their standard states. Based of the table (picture):
A. What is the lattice enthalpy of MX2? (in kJ/mol)
B. What is the enthalpy of formation of MX2? (in kJ/mol)
C. Suppose the electron affinity of X were bigger and the heat of sublimation of M were smaller. Would MX2 be more or less stable? Or would it be impossible to tell without more information?
This thermodynamic cycle describes the formation of an ionic compound MX from a metal element M and nonmetal element X in their standard states. Based of the table (picture):
A. What is the lattice enthalpy of MX? (in kJ/mol)
B. What is the enthalpy of formation of MX? (in kJ/mol)
C. Suppose both the electron affinity of X and the heat of sublimation of M were bigger. Would MX be more or less stable?
Explain the following trends in latttice energy:
a. NaCl >RbBr
b. BaO > KF
c. SrO > SrCl2
Chapter 3 Solutions
Inorganic Chemistry
Ch. 3.1 - Use electron-dot diagrams and formal charges to...Ch. 3.2 - Predict the structures of the following ions....Ch. 3.2 - Prob. 3.3ECh. 3.2 - Which molecule has the smallest bond angle in each...Ch. 3.2 - Briefly account for the following observations: a....Ch. 3.2 - Does this approach work for different steric...Ch. 3 - The dimethyldithiocarbamate ion, [S2CN( CH 3 )2]-...Ch. 3 - Several resonance structures are possible for each...Ch. 3 - Draw the resonance structures for the...Ch. 3 - Three isomers having the formula N2CO are known:...
Ch. 3 - Show the possible resonance structures for nitrous...Ch. 3 - Nitric acid, which exists as HNO3 molecules in the...Ch. 3 - L. C. Allen has suggested that a more meaningful...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Explain the trends in bond angles and bond lengths...Ch. 3 - Select from each set the molecule or ¡on having...Ch. 3 - a. Compare the structures of the azide ion, N3 ,...Ch. 3 - Consider the series OCl2,O( CH3)2 , and O( SiH3)2...Ch. 3 - Two ions isoelectronic with carbon suboxide, C3O2...Ch. 3 - Explain the following: a. Ethylene, C2H4 , is a...Ch. 3 - Explain the following: a. PCI5 is a stable...Ch. 3 - X-ray crystal structures of ClOF3 and BrOF3 have...Ch. 3 - Make the following comparisons about the molecules...Ch. 3 - Prob. 3.20PCh. 3 - A solution containing the lO2F2 ion reacts slowly...Ch. 3 - The XeOF3 anion has been reported recently (D. S....Ch. 3 - Predict the structure of l(CF3)Cl2 . Do you expect...Ch. 3 - a. Which has the longer axial PF distance, PF2(...Ch. 3 - Prob. 3.25PCh. 3 - SeCl62,TeCl62 , and CIF6 are all octahedral, but...Ch. 3 - Prob. 3.27PCh. 3 - The thiazyldichloride ion, NSCl2- , is...Ch. 3 - Sketch the most likely structure of PCl3Br2 and...Ch. 3 - a. Are the CF3 groups in PCl3( CF3)2 more likely...Ch. 3 - Of the molecules C1SO2CH3,C1SO2CF3 , and ClSO2CCl3...Ch. 3 - Prob. 3.32PCh. 3 - Prob. 3.33PCh. 3 - Prob. 3.34PCh. 3 - Prob. 3.35PCh. 3 - Although the CF distances and the FCF bond angles...Ch. 3 - The Cl...Cl distance in CCl4 is 289 pm, and the...Ch. 3 - The FCF angle in F2CO , shown here, is 109.5°; the...Ch. 3 - Compounds in which hydrogen is the outer atom can...Ch. 3 - For each of the following bonds, indicate which...Ch. 3 - Give Lewis dot structures and shapes for the...Ch. 3 - Give Lewis dot structures and sketch the shapes...Ch. 3 - Which of the molecules in Problem 3.41 are polar?Ch. 3 - Which of the molecules in Problem 3.42 are polar?Ch. 3 - Prob. 3.45PCh. 3 - Prob. 3.46P
Additional Science Textbook Solutions
Find more solutions based on key concepts
The structural formula of 1, 2-dimethylbenzene needs to be drawn. Concept introduction: The ring structures of ...
Chemistry: Matter and Change
Practice Problem 1.22 Which of the following alkenes can exist as cis-trans isomers? Write their structures. Bu...
Organic Chemistry
45. Calculate the mass of nitrogen dissolved at room temperature in an 80.0-L home aquarium. Assume a total pre...
Chemistry: Structure and Properties
The chapter sections to review are shown in parentheses at the end of each problem. A "chemical-free” shampoo i...
Basic Chemistry
Write a Lewis formula for each of the following organic molecules: C2H3Cl (vinyl chloride: starting material fo...
Organic Chemistry - Standalone book
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
- The compound NF3 is quite stable, but NCl3 is very unstable (NCl3 was first synthesized in 1811 by P. L. Dulong, who lost three fingers and an eye studying its properties). The compounds NBr3 and NI3 are unknown, although the explosive compound NI3 NH3 is known. Account for the instability of these halides of nitrogen.arrow_forwardConsider the element Work (Wr) with an atomic number of 33 and an atomic mass of 81.03 g/mol. The following information was collected for this element Molecule/ Ion Names Wr-2 Workide WrO3-2 Workate WrO2-2 Workite WrO-3 hydroworkite a. Draw the Lewis structure of the molecule Workous acid and determine its electron geometry and molecular geometry. b.What is the mass % of work in Calcium hydroworkite.arrow_forwardAlthough PF5 and AsF5 are stable, nitrogen does not form NF5 molecules. Explain this difference among members of the same group.arrow_forward
- 28. Estimate the enthalpy (change in energy) of reaction for 2 SO(g) + O2(g) →2 SO2(g) using bond energies. Assume that sulfur in SO2 (g) has an expanded octet. -> Bond Energy (kJ/mol) 498 265 a. 498 kJ/mol c. -498 kJ/mol bь. 731 kJ/mol d. -32KJ/molarrow_forward2. X is isoelectronic with Xe. It reacts with Na ion and forms Na2X.a. Give the electronic configuration (EC) and orbital diagram (OD) of the NEUTRAL atom of X. b. X forms an oxide, XO2. Give the chemical name, draw the Lewis structure of XO2 and predict its shape.arrow_forwardRecall that nitrogen triiodide (NI3) is very shock-sensitive. Forming F2(g) from F− ions releases much more energy than forming I2(s) from I− ions. Why is nitrogen trifluoride (NF3) a stable compound?arrow_forward
- 2. Identify the true statement. a. Polar covalent compounds result from a complete transfer of at least one electron. b. Sodium is unlikely to form a bond with lithium. c. Covalent compounds exist in large lattices. d. The smallest unit of an ionic compound is a molecule. 3. A piece of zinc metal is placed in an aqueous solution of magnesium sulfate. The products of this reaction are a. ZnMg(s) + SO4(aq) b. Mg(s) + ZnSO4(aq) c. MgS(s) + ZnO4(aq) d. ZnO(s) + MgSO4(aq) e. There will be no reaction. 4. The shape of the NC13 molecule is a. linear b. trigonal planar c. tetrahedral d. trigonal pyramidal e. V-shaped Imi 5. Which of the following would have the highest boiling point? a. NH3 b. PH3 c. AsH3 d. They would all have approximately the same boiling point. 20 6. Aqueous solutions of silver nitrate and sodium sulfate are mixed. The products of the reaction are a. Ag2SO4(aq) + 2 NaNO3(aq) b. AgSO4(s) + Na2(NO3)2(aq) c. Ag2SO4(s) + 2 NaNO3(aq) d. AgSO4(aq) + Na2(NO3 e. There will be no…arrow_forward9. Provide the electron configuration for the B2, C22, and N₂ ions. What are their magnetic properties?arrow_forwardGive an example of Interhalogen Compounds?arrow_forward
- How does CO2 cause more heat to be retained in the Earth's atmosphere? Which one of the options?1. it reacts with oxygen to produce ozone, which retains more heat than oxygen. 2. Carbon dioxide when dissolved in water forms carbonic acid. 3. It is a greenhouse gas that absorbs infrared radiation due to its shape and size.arrow_forwardA. Calculate the total of free electrons in 2.5 x 10' g of. Co ( Cobalt-60) if 1 atom give 3 electronsarrow_forward3. In this experiment, you will be studying the oxidation strength of the halogens. a. What is the color of each of the halogens that you will be working with in this experiment? b. Write Lewis dot structures for each of the halogen molecules: F2, Cl2, Br2, and I2. c. On the basis of periodic trends, which of the halogen molecules do you expect to have the shortest bond? Explain why.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
NEET Chemistry | Group 14 Carbon Family | Theory & Problem Solving | In English | Misostudy; Author: Misostudy;https://www.youtube.com/watch?v=enOGIrcHh54;License: Standard YouTube License, CC-BY