Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 8, Problem 21E
Write Lewis structures for NF3 and PP5. On the basis of hybrid orbitals, explain the fact that NF3, PP3, and PP5 are stable molecules, but NP5 does not exist.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Draw the molecular orbital diagrams
for Ne(2), N(2) ^2- and Be(2). Are they
stable or unstable?
the three stable oxides of carbon monoxide (CO), Carbon dioxide(CO2), and carbon suboxide (C3O2). for each oxide draw the Lewis structure, predict the molecular structure, and described the bonding in terms of the hybrid orbitals for carbon atoms.
Write Lewis structures for NF3 and PF5. On the basis of hybrid orbitals, explain the fact that NF3, PF3, and PF5 are stable molecules, but NF5 does not exist.
Chapter 8 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 8 - Explain how and bonds are similar and how they...Ch. 8 - Draw a curve that describes the energy of a system...Ch. 8 - Explain why bonds occur at specific average bond...Ch. 8 - Use valence bond theory to explain the bonding in...Ch. 8 - Use valence bond theory to explain the bonding in...Ch. 8 - How many and bonds are present in the molecule...Ch. 8 - A friend tells you N2 has three bonds due to...Ch. 8 - Draw the Lewis structures for CO2 and CO, and...Ch. 8 - Why is the concept of hybridization required in...Ch. 8 - Give the shape that describes each hybrid orbital...
Ch. 8 - Explain why a carbon atom cannot form five bonds...Ch. 8 - What is the hybridization of the central atom in...Ch. 8 - A molecule with the formula AB3 could have one of...Ch. 8 - Methionine, CH3SCH2CH2CH(NH2)CO2H, is an amino...Ch. 8 - Sulfuric acid is manufactured by a series of...Ch. 8 - Two important industrial chemicals, ethene, C2H4,...Ch. 8 - For many years after they were discovered, it was...Ch. 8 - Consider nitrous acid, HNO2 (HONO). (a) Write a...Ch. 8 - Strike-anywhere matches contain a layer of KClO3...Ch. 8 - Identify the hybridization of each carbon atom in...Ch. 8 - Write Lewis structures for NF3 and PP5. On the...Ch. 8 - In addition to NF3, two other fluoro derivatives...Ch. 8 - The bond energy of a C—C single bond averages 347...Ch. 8 - For the carbonate ion, CO32, draw all of the...Ch. 8 - A useful solvent that will dissolve salts as well...Ch. 8 - For the molecule allene, H2C=C=CH2, give the...Ch. 8 - Identify the hybridization of the central atom in...Ch. 8 - Describe the molecular geometry and hybridization...Ch. 8 - For each of the following molecules, indicate the...Ch. 8 - For each of the following structures, determine...Ch. 8 - Draw the orbital diagram for carbon in CO2 showing...Ch. 8 - Sketch the distribution of electron density in the...Ch. 8 - How are the following similar, and how do they...Ch. 8 - If molecular orbitals are created by combining...Ch. 8 - Can a molecule with an odd number of electrons...Ch. 8 - Can a molecule with an even number of electrons...Ch. 8 - Why are bonding molecular orbitals lower in energy...Ch. 8 - Calculate the bond order for an ion with this...Ch. 8 - Explain why an electron in the bonding molecular...Ch. 8 - Predict the valence electron molecular orbital...Ch. 8 - Determine the bond order of each member of the...Ch. 8 - For the first ionization energy for an N2...Ch. 8 - Compare the atomic and molecular orbital diagrams...Ch. 8 - Which of the period 2 homonuclear diatomic...Ch. 8 - A friend tells you that the 2s orbital for...Ch. 8 - True or false: Boron contains 2s22p1 valence...Ch. 8 - What charge would be needed on F2 to generate an...Ch. 8 - Predict whether the MO diagram S2 would show s-p...Ch. 8 - Explain why N22+ is diamagnetic, while O24+, which...Ch. 8 - Using the MO diagrams, predict the bond order for...
Additional Science Textbook Solutions
Find more solutions based on key concepts
Two identical pucks collide on an air hockey table. One puck was originally at rest. (a) If the incoming puck h...
College Physics
Determine whether each molecule is polar or nonpolar. ClO3- SCl2 SCl4 BrCl5
Chemistry: A Molecular Approach
53. Write a formula for the ionic compound that forms from each pair of elements.
a. sodium and sulfur
b. stro...
Introductory Chemistry (5th Edition) (Standalone Book)
Which compound is more easily decarboxylated?
Organic Chemistry
a. Find potassium (K) in the periodic table and predict how many valence electrons it has. b. What orbital does...
Essential Organic Chemistry (3rd Edition)
a. How does increasing the temperature increase the rate of a chemical reaction? b. How does increasing the amo...
General, Organic, and Biological Chemistry (3rd Edition)
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
- Describe the hybridization around the central atom and the bonding in SCl2 and OCS.arrow_forwardIt is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forwardDraw the Lewis structures and molecular orbital diagrams for CO and NO. What are their bond orders? Are they similar to their Lewis structures? Explain.arrow_forward
- Draw the Lewis structure of ICl4 and then determine its electron domain and molecular geometries.arrow_forwardWhat is the hybridization of the central phosphorus atom of PO43− ?arrow_forwardIodine and oxygen form a complex series of ions, among them IO4^- and IO5^3-. Draw the Lewis structures for these ions, and specify their electron-pair geometries and the shapes of the ions. What is the hybridization of the I atom in these ions?arrow_forward
- Boron trifluoride (BF3) has no dipole moment (u = 0 D). Explain how this observation confirms the geometry of BF3 predicted by VSEPR theory.arrow_forwardDraw the structural formula of bis(dimethylglyoximato)nickel(1I) and describe the type of hybridization involved ?arrow_forwardThe existence of compounds of the noble gases was once a great surprise and stimulated a great deal of theoretical work. Sketch the molecular orbital energy level diagram for XeF and deduce its ground-state electron configurations. Is XeF likely to have a shorter or longer bond than XeF+?arrow_forward
- Compare the molecular shapes and hybrid orbitals of P F 3 and P F 5 molecules .Explain why their shapes differ.arrow_forwardFor a N H 4 + ion, identify its molecular shape, bond angle, and hybrid orbitals.arrow_forwardDescribe the structure of a P2 molecule in valence-bond terms. Why is P4 a more stable form of molecular phosphorus than P2?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
INTRODUCTION TO MOLECULAR QUANTUM MECHANICS -Valence bond theory - 1; Author: AGK Chemistry;https://www.youtube.com/watch?v=U8kPBPqDIwM;License: Standard YouTube License, CC-BY