Student Solutions Manual for Oxtoby/Gillis/Butler's Principles of Modern Chemistry, 8th
8th Edition
ISBN: 9798214170251
Author: David W. Oxtoby, H. Pat Gillis and Laurie J. Butler
Publisher: Cengage Learning US
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 3, Problem 61P
For each of the following molecules or molecular ions, give the steric number, sketch and name the approximate molecular geometry, and describe the directions of any distortions from the approximate geometry due to lone pairs. In each case, the central atom is listed first and the other atoms are all bonded directly to it.
(a)
(b)
(c)
(d)
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Chemical species are said to be isoelectronic if they have the same Lewis structure (regardless of charge). Consider these ions and write a Lewis structure for a neutral molecule that is isoelectronic with them. (a) CN–, (b) NH4+ (c) CO3 2–
Determine the electron-group arrangement, molecular shape, and ideal bond angle(s) for each of the following:(a) SO₄²⁻(b) NO₂⁻(c) PH
Compounds such as NaBH4, Al(BH4)3, and LiAlH4 are complexhydrides used as reducing agents in many syntheses.(a) Give the oxidation state of each element in these compounds.(b) Write a Lewis structure for the polyatomic anion in NaBH4, and predict its shape.
Chapter 3 Solutions
Student Solutions Manual for Oxtoby/Gillis/Butler's Principles of Modern Chemistry, 8th
Ch. 3 - Before the element scandium was discovered in...Ch. 3 - Prob. 2PCh. 3 - Prob. 3PCh. 3 - Prob. 4PCh. 3 - Prob. 5PCh. 3 - A gold nucleus is located at the origin of...Ch. 3 - Prob. 7PCh. 3 - A gold nucleus is located at the origin of...Ch. 3 - Prob. 9PCh. 3 - Prob. 10P
Ch. 3 - Use the data in Table 3.1 to plot the logarithm of...Ch. 3 - Use the data in Table 3.1 to plot the logarithm of...Ch. 3 - Prob. 13PCh. 3 - Prob. 14PCh. 3 - Prob. 15PCh. 3 - Prob. 16PCh. 3 - Prob. 17PCh. 3 - Prob. 18PCh. 3 - HF has equilibrium bond length of 0.926 A and bond...Ch. 3 - Prob. 20PCh. 3 - For each of the following atoms or ions, state the...Ch. 3 - Prob. 22PCh. 3 - Use the data in Figure 3.11 and Table 3.2 to...Ch. 3 - Use the data in Figure 3.11 and Table 3.2 to...Ch. 3 - Prob. 25PCh. 3 - In a gaseous RbF molecule, the bond length is...Ch. 3 - The bond lengths of the XH bonds in NH3,PH3 , and...Ch. 3 - Arrange the following covalent diatomic molecules...Ch. 3 - The bond length in HI(1.62) is close to the sum of...Ch. 3 - Prob. 30PCh. 3 - Use electronegativity values to arrange the...Ch. 3 - Use electronegativity values to rank the bonds in...Ch. 3 - Prob. 33PCh. 3 - Prob. 34PCh. 3 - Prob. 35PCh. 3 - Estimate the percent ionic character of the bond...Ch. 3 - The percent ionic character of a bond can be...Ch. 3 - The percent ionic character of the bonds in...Ch. 3 - Assign formal charges to all atoms in the...Ch. 3 - Assign formal charges to all atoms in the...Ch. 3 - Determine the formal charges on all the atoms in...Ch. 3 - the formal charges on all the atoms in the...Ch. 3 - Prob. 43PCh. 3 - In each of the following Lewis diagrams, Z...Ch. 3 - Draw Lewis electron dot diagrams for the following...Ch. 3 - Prob. 46PCh. 3 - Prob. 47PCh. 3 - Acetic acid is the active ingredient of vinegar....Ch. 3 - Under certain conditions, the stable form of...Ch. 3 - White phosphorus (P4) consists of four phosphorus...Ch. 3 - Draw Lewis electron dot diagrams for the following...Ch. 3 - Draw Lewis electron dot diagrams for the following...Ch. 3 - Draw Lewis diagrams for the two resonance forms of...Ch. 3 - Draw Lewis diagrams for the three resonance forms...Ch. 3 - Methyl isocyanate, which was involved in the...Ch. 3 - Prob. 56PCh. 3 - Draw Lewis diagrams for the following compounds....Ch. 3 - Draw Lewis diagrams for the following ions. In the...Ch. 3 - Prob. 59PCh. 3 - Prob. 60PCh. 3 - For each of the following molecules or molecular...Ch. 3 - For each of the following molecules or molecular...Ch. 3 - Give an example of a molecule or ion having a...Ch. 3 - Give an example of a molecule or ion having a...Ch. 3 - For each of the answers in Problem 59, state...Ch. 3 - For each of the answers in Problem 60, state...Ch. 3 - Prob. 67PCh. 3 - Mixing SbCl3 and GaCl3 in a 1:1 molar ratio (using...Ch. 3 - (a) Use the VSEPR theory to predict the structure...Ch. 3 - Ozone (O3) has a nonzero dipole moment. In the...Ch. 3 - Assign oxidation numbers to the atoms in each of...Ch. 3 - Prob. 72PCh. 3 - Prob. 73PCh. 3 - Prob. 74PCh. 3 - Prob. 75PCh. 3 - Prob. 76PCh. 3 - Prob. 77PCh. 3 - Prob. 78PCh. 3 - Prob. 79PCh. 3 - Prob. 80PCh. 3 - Prob. 81PCh. 3 - Prob. 82PCh. 3 - Prob. 83PCh. 3 - Prob. 84PCh. 3 - Prob. 85APCh. 3 - Prob. 86APCh. 3 - At large interatomic separations, an alkali halide...Ch. 3 - Prob. 88APCh. 3 - Prob. 89APCh. 3 - Two possible Lewis diagrams for sulfine (H2CSO)...Ch. 3 - There is persuasive evidence for the brief...Ch. 3 - The compound SF3N has been synthesized. (a) Draw...Ch. 3 - Prob. 93APCh. 3 - The molecular ion S3N3 has the cyclic structure...Ch. 3 - Prob. 95APCh. 3 - Prob. 96APCh. 3 - Prob. 97APCh. 3 - Prob. 98APCh. 3 - A stable triatomic molecule can be formed that...Ch. 3 - The gaseous potassium chloride molecule has a...Ch. 3 - (a) Predict the geometry of the SbCl52 ion, using...Ch. 3 - Prob. 102APCh. 3 - Predict the arrangement of the atoms about the...Ch. 3 - Prob. 104APCh. 3 - Prob. 105APCh. 3 - Prob. 106APCh. 3 - Prob. 107APCh. 3 - Prob. 108APCh. 3 - (a) Determine the oxidation number of lead in each...Ch. 3 - Prob. 110APCh. 3 - Prob. 111CPCh. 3 - Prob. 112CPCh. 3 - A compound is being tested for use as a rocket...Ch. 3 - Prob. 114CP
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 Lewis structure of BH2Cl (a) Is the molecule polar or nonpolar? (b) What is the hybridization of the carbon atom? (c) What is the geometric shape of the molecule?arrow_forwardIdentify the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) IF6+(b) CF4(c) BF3(d) SiF5−(e) BeCl2arrow_forwardCyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.arrow_forward
- 1. Draw the Lewis structures for each of the following ions or molecules. For each, give (i) the molecular shape, (ii) the electron pair geometry at the central atom, and (iii) the hybridization of the central atom. (a) POF3 (b) XeO₂F3+ (c) BrCl₂ (d) N3 (the central atom is N; two other N's are bonded to it) (e) PF3arrow_forwardPredict the molecular geometries and draw Lewis structures for each of the following. (a) IF5(b) I3−(c) PCl5(d) SeF4(e) ClF3arrow_forwardWhich of these statements about resonance is true?(a) When you draw resonance structures, it is permissibleto alter the way atoms are connected.(b) The nitrate ion has one long N¬O bond and two shortN¬O bonds.(c) “Resonance” refers to the idea that molecules areresonating rapidly between different bonding patterns.(d) The cyanide ion has only one dominant resonancestructure.(e) All of the above are true.arrow_forward
- 19. :O: || :0-N- O: Which of the following statements, if true, would support the claim that the NO3 ion, represented above, has three resonance structures? (A) The NO3 ion is not a polar species. (B) The oxygen-to-nitrogen-to-oxygen bond angles are 90°. (C) One of the bonds in NO3 is longer than the other two. (D) One of the bonds in NO3¯ is shorter than the other two.arrow_forwardGive the hybridization of the metalloid and the molecular geometry for each of the following compounds or ions. (a) GeH4(b) SbF3(c) Te(OH)6(d) H2Te(e) GeF2(f) TeCl4(g) SiF62−(h) SbCl5(i) TeF6arrow_forwardWhich of the following would you expect to have the highest bond energy (strength)? (a) 02 (b) Cl2 N₂ F2 3 (d)arrow_forward
- Two substances with empirical formula HNO are hyponi-trous acid ( μ=62.04 g /mol) and nitroxyl (μ=31.02 g/mol).(a) What is the molecular formula of each species?(b) For each species, draw the Lewis structure having the lowestformal charges. (Hint:Hyponitrous acid has an N=N bond.)(c) Predict the shape around the N atoms of each species.(d) When hyponitrous acid loses two protons, it forms the hy-ponitrite ion. Draw cisand transforms of this ion.arrow_forwardWrite a Lewis structure for each of the following molecules and ions:(a) (CH3)3SiH(b) SiO44−(c) Si2H6(d) Si(OH)4(e) SiF62−arrow_forwardSulfur tetrafluoride (SF4) reacts slowly with O2 to form sulfurtetrafluoride monoxide (OSF4) according to the followingunbalanced reaction: SF4(g) + O2(g)---->OSF4(g)The O atom and the four F atoms in OSF4 are bonded to acentral S atom. (a) Balance the equation. (b) Write a Lewisstructure of OSF4 in which the formal charges of all atomsare zero. (c) Use average bond enthalpies (Table 8.3) to estimatethe enthalpy of the reaction. Is it endothermic or exothermic?(d) Determine the electron-domain geometry ofOSF4, and write two possible molecular geometries for themolecule based on this electron-domain geometry. (e) Foreach of the molecules you drew in part (d), state how manyfluorines are equatorial and how many are axial.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
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
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY