Organic Chemistry: Principles and Mechanisms (Second Edition)
2nd Edition
ISBN: 9780393663556
Author: Joel Karty
Publisher: W. W. Norton & Company
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 3, Problem 3.29P
Interpretation Introduction
Interpretation:
Why an s AO from one atom and a p AO from another will not interact in the given orientation is to be explained.
Concept introduction:
According to the Molecular Orbital Theory (MO Theory), when two atomic orbitals overlap significantly, they produce two molecular orbitals. One of these molecular orbitals is produced by overlap and mixing of two AOs that have the same phase. This MO is lower in energy than the individual AOs, and is called the bonding atomic orbital. The second MO is produced by the overlap and mixing of the AOs of opposite phases. It is higher in energy than the individual AOs and is called the antibonding MO.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Given the molecule CH2CHCN Please draw a Lewis structure for this compound with CORRECT GEOMETRY and label all sigma and pi bonds with the orbitals it is made from (what orbitals are overlapping to form the bond). You may draw the hybridized sigma orbitals as sticks and the unhybridized p-orbitals as lobes for clarity. For this question, you DO need to draw out the orbitals.
4.
,A: Briefly describe why the p orbital can contain a positive charge and hybridized
orbital cannot. Use pictures in your answer.
B: Briefly explain why a hybridized orbital can contain a negative charge, and P-orbital cannot.
Use pictures in your answer.
Solve correctly please with some explanation also.
Electron pair geometry(option): Linear,triagonal planar, tetrahedral,trigonal bipyramidal, octahedral.
Chapter 3 Solutions
Organic Chemistry: Principles and Mechanisms (Second Edition)
Ch. 3 - Prob. 3.1PCh. 3 - Prob. 3.2PCh. 3 - Prob. 3.3PCh. 3 - Prob. 3.4PCh. 3 - Prob. 3.5PCh. 3 - Prob. 3.6PCh. 3 - Prob. 3.7PCh. 3 - Prob. 3.8PCh. 3 - Prob. 3.9PCh. 3 - Prob. 3.10P
Ch. 3 - Prob. 3.11PCh. 3 - Prob. 3.12PCh. 3 - Prob. 3.13PCh. 3 - Prob. 3.14PCh. 3 - Prob. 3.15PCh. 3 - Prob. 3.16PCh. 3 - Prob. 3.17PCh. 3 - Prob. 3.18PCh. 3 - Prob. 3.19PCh. 3 - Prob. 3.20PCh. 3 - Prob. 3.21PCh. 3 - Prob. 3.22PCh. 3 - Prob. 3.23PCh. 3 - Prob. 3.24PCh. 3 - Prob. 3.25PCh. 3 - Prob. 3.26PCh. 3 - Prob. 3.27PCh. 3 - Prob. 3.28PCh. 3 - Prob. 3.29PCh. 3 - Prob. 3.30PCh. 3 - Prob. 3.31PCh. 3 - Prob. 3.32PCh. 3 - Prob. 3.33PCh. 3 - Prob. 3.34PCh. 3 - Prob. 3.35PCh. 3 - Prob. 3.36PCh. 3 - Prob. 3.37PCh. 3 - Prob. 3.38PCh. 3 - Prob. 3.39PCh. 3 - Prob. 3.40PCh. 3 - Prob. 3.41PCh. 3 - Prob. 3.42PCh. 3 - Prob. 3.43PCh. 3 - Prob. 3.44PCh. 3 - Prob. 3.45PCh. 3 - Prob. 3.46PCh. 3 - Prob. 3.47PCh. 3 - Prob. 3.48PCh. 3 - Prob. 3.49PCh. 3 - Prob. 3.50PCh. 3 - Prob. 3.51PCh. 3 - Prob. 3.52PCh. 3 - Prob. 3.53PCh. 3 - Prob. 3.54PCh. 3 - Prob. 3.55PCh. 3 - Prob. 3.56PCh. 3 - Prob. 3.1YTCh. 3 - Prob. 3.2YTCh. 3 - Prob. 3.3YTCh. 3 - Prob. 3.4YTCh. 3 - Prob. 3.5YTCh. 3 - Prob. 3.6YTCh. 3 - Prob. 3.7YTCh. 3 - Prob. 3.8YTCh. 3 - Prob. 3.9YTCh. 3 - Prob. 3.10YTCh. 3 - Prob. 3.11YTCh. 3 - Prob. 3.12YTCh. 3 - Prob. 3.13YT
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
- need answer to this onearrow_forwardConstruct, fully label, and populate a MO diagram for the nitrosonium anion, NO+. Based on the diagram, state which of NO+ or NO you expect to have a stronger bond.arrow_forward© Macmillan Leaming Consider two 2p orbitals, one on each of two different atoms, that are oriented side-to-side as in the figure. Imagine bringing these nuclei together so that overlap occurs as shown in the figure. This overlap results in a system of molecular orbitals. Construct an orbital interaction diagram for molecular orbital formation using the images that represent various orbital types (e.g., atomic, bonding, antibonding). Then, identify the number of nodes in each atomic and molecular orbital. Energy Select the number of nodes in the atomic orbital. Select the number of nodes in the bonding molecular orbital. Select the number of nodes in the antibonding molecular orbital. Arawer Bank 96arrow_forward
- Choose the best ending to this statement, given what you have learned about MO Theory. "When two orbitals combine to make a bond... O ..two new orbitals are formed. One is lower energy than the atomic orbitals and the other is higher energy than the starting atomic orbitals." O .only one new orbital is formed which holds the bonding electrons." O .two new orbitals are formed. Both new orbitals are lower energy than the starting orbitals. O .the number of orbitals formed depends on how many electrons are shared between the two atoms."arrow_forwardSolve please.arrow_forwardNeed help, please.arrow_forward
- Please answer as soon as possibly and I will leave a like.arrow_forwardUse the References to access important values if needed for this question. A π bond arises from "sideways" overlap of two parallel p orbitals. The electron density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals. Submit Answer p-orbital p-orbital atom 1 atom 2 What atomic or hybrid orbitals make up the bond between N and O in nitrosyl bromide, NOBr? sp² orbital on N + sp³ 3 orbital on O How many bonds does N have in NOBr? How many bonds does N have? + Retry Entire Group л bond 9 more group attempts remainingarrow_forwardAnswer following questionsarrow_forward
- 4. Match the following MOs drawn to their structure. Note that more electronegative atoms tend to draw more electrons towards themselves.arrow_forwardGive detailed Solution with explanation needed.don't give Ai generated solution. Give Clear handwritten Solutionarrow_forwardConsider the incomplete orbital representation of O2 , below right. a. Identify which lobes are hybrid orbitals (identify the type) and which lobes arep orbitals. b. Use dotted lines to show any bonds. c. Use up or down arrows to show electron occupation of each hybrid orbital or bond.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning
Organic Chemistry: A Guided Inquiry
Chemistry
ISBN:9780618974122
Author:Andrei Straumanis
Publisher:Cengage Learning