Custom eBook for Organic Chemistry
2nd Edition
ISBN: 9798214171104
Author: Straumanis
Publisher: Cengage Custom
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 5, Problem 12CTQ
Interpretation Introduction
Interpretation: The reason that explains zero possibility for resonance structure of following anion should be determined.
Concept introduction: Lewis structure is a representation of molecules in which dots are shown to represent unshared electrons and lines are shown to represent bonds. These lines and dots represent distribution of electrons in the molecule.
When one single structure is unable to describe all the properties of a single-molecule, a phenomenon called resonance comes into play. This arises when two or more than two Lewis structures are possible for one molecule. All such structures are called resonating structures and have same placement of atoms in them but these have different locations of bond pairs and lone pairs. The resonating structures are inter-convertible with each other. The resultant of all the resonating or contributing structures is called the resonance hybrid.
Rules to form resonance structure are as follows:
1. Use arrow types 1 and 2 for the resonance structure of anions in the movement of negative charge.
2. Use only arrow type 3 to move a positive charge for the resonance structure of cations.
3. The sigma bond should not be broken. Any atom must not move from its place and total number of electrons must be the same in all resonance structures.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Draw three resonance structures for CS,. This species has its three atoms bonded sequentially in the following fashion: S-C-S.
Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important
resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have
drawn. Select the choices from below which make the statements true about this (most important) resonance structure.
(a) The leftmost bond (between S and C) is a single
v bond.
(b) The rightmost bond (between C and S) is a single
v bond.
(c) The formal charge on the leftmost (S) atom is
-Select-v
(d) The formal charge on the central (C) atom is
-Select---v
(e) The formal charge on the rightmost (S) atom is
Select-v
(f) The number of nonbonding pairs (lone pairs) of electrons in the leftmost (S) atom is
Select-v pairs.
(g) The number of nonbonding (lone) pairs of electrons in the rightmost (S) atom is -Select-- v pairs.
Question
Provide each unique Lewis structure for the HONO molecule that maintains the H-O-NO connectivity and where all atoms have an octet (hydrogen a duet).
Your structures should explicitly show ALL bonds, all lone pairs, and all formal charges.
Which Lewis structure contributes more to the real hybrid structure of HONO?
What is the relationship between these Lewis structures and what type of arrow is used to show their relationship?
This question is confusing to me. Please explain your answer.
Are the bond lengths data consistent with a resonance model? Yes or no? Please explain thank you.
Chapter 5 Solutions
Custom eBook for Organic Chemistry
Ch. 5 - Which elements on the periodic table (other than...Ch. 5 - You will not find “hydroxide” in the stockroom,...Ch. 5 - Prob. 3CTQCh. 5 - Prob. 4CTQCh. 5 - Prob. 5CTQCh. 5 - Prob. 6CTQCh. 5 - On which do you expect to have a more intense and...Ch. 5 - Prob. 8CTQCh. 5 - Prob. 9CTQCh. 5 - Prob. 10CTQ
Ch. 5 - Prob. 11CTQCh. 5 - Prob. 12CTQCh. 5 - Prob. 13CTQCh. 5 - Prob. 14CTQCh. 5 - Prob. 15CTQCh. 5 - Prob. 16CTQCh. 5 - For each proposed set of resonance structures: a....Ch. 5 - Consider the polarization of the C=O bond in the...Ch. 5 - The C=O double bond is called a “carbonyl bond.”...Ch. 5 - Prob. 20CTQCh. 5 - Prob. 21CTQCh. 5 - Prob. 22CTQCh. 5 - Prob. 23CTQCh. 5 - Prob. 24CTQCh. 5 - Prob. 25CTQCh. 5 - Prob. 26CTQCh. 5 - Prob. 27CTQCh. 5 - Prob. 28CTQCh. 5 - Prob. 29CTQCh. 5 - Prob. 30CTQCh. 5 - Prob. 31CTQCh. 5 - Confirm that there is no legitimate Lewis...Ch. 5 - Draw all resonance structures of the molecule...Ch. 5 - Prob. 34CTQCh. 5 - Prob. 35CTQCh. 5 - Prob. 36CTQCh. 5 - Occasionally, we will see an ionic compound that...Ch. 5 - Prob. 2ECh. 5 - Prob. 3ECh. 5 - Prob. 4ECh. 5 - Is it possible to draw a resonance structure of...Ch. 5 - Prob. 6ECh. 5 - Prob. 7ECh. 5 - Prob. 8ECh. 5 - Phenol (shown below) has a pKa10 . a. Based on pKa...Ch. 5 - Use curved arrows to show the most likely...Ch. 5 - Prob. 12ECh. 5 - Complete each Lewis structure, draw all important...Ch. 5 - Use curved arrows to show the most likely...Ch. 5 - Construct an explanation for why sulfuric acid is...Ch. 5 - Prob. 16ECh. 5 - Prob. 17ECh. 5 - Prob. 18E
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
- 1. Molecule: CF4 indicate the number of available electrons that electrons ae = are in the molecule. in the space to the right connect all of the atoms to the central atom and then make each atom follow the octet rule Trial Structure: (duet rule for hydrogen). How many electrons are necessary in the trial ne = structure? Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geOm Hybridization:arrow_forwardTHE COMPLETE QUESTION IS HEREarrow_forwardChem Helparrow_forward
- What is the formal charge on chlorine in the best Lewis structure for chloric acid? type your answer...arrow_forwardExplaine why, in Part I, the formal charge is equal to the number of valence electrons. Match the words in the left column to the appropriate blanks in the sentences on the right. minus The formal charge on each atom is the number of valence electrons the number of plus lone pair electrons and the number of bonding electrons. The formal charge is equal to the number of valence electrons because there are bonds. one-half two times no multiplearrow_forwardWould you mind to check all the answer on this table because I try to understand the line bond structure and re-draw structure my homework? Could you help me with this question CS2?arrow_forward
- How do you know when to draw a solid wedge vs a dashed wedge when drawing 3D bond-line structures? I know that solid-wedge means the atom is pointing towards you and dashed wedge means it's in the back, but how do you know which atoms are in the front as opposed to the back? How can you tell what the configuration will look like in space just by looking at the lewis structure or name?arrow_forwardPlease help me answer this with complete solutionarrow_forwardWhat is the formal charge (FC) of nitrogen and Carbon in the following molecule/ion? Show your work in a seperate sheet. Include all steps (drawing lewis structure by calculating total valence, and calculating formal charge). a) FC of nitrogen in NO3-= b) FC of carbon in CO2 =arrow_forward
- Clear my choice With regard to resonance structures that are drawn for a real species, which of the following statements is NOT TRUE? Select one: A. Resonance structures all have electron localized structures, while the real species that is described by them has delocalized electrons. OB. Resonance structures are real molecules that co-exist in equilibrium with each other. O C. Resonance structures differ in the location of their electrons, not the positions of their atoms. O D. Resonance structures are only drawings; each structure alone does not represent an existing molecule. Clear my choice What type of hybrid orbitals is used by the nitrogen atom in the following molecule? HO-N=0: hparrow_forwarda) Draw the Lewis structure for the molecule on the left (labeled as Molecule A above). Draw the Lewis structure which has minimum formal charges. b) Draw the correct Lewis structure for the molecule on the right (labeled as Molecule B above). Draw the Lewis structure which has minimum formal charges. c) Select the three TRUE statements from those provided below. The molecule on the right (Molecule B) is planar (all atoms lie within the same plane). The molecule on the left (Molecule A) is planar (all atoms lie within the same plane). The molecule on the right (Molecule B) has polar bonds. The molecule on the left (Molecule A) has polar bonds. We can distinguish between the two molecules (Molecule A and Molecule B) based upon their dipole moment.arrow_forwardCould someone help me?? The answer to this question must look similar to the example attached. Back ground info: Atoms of different elements combine with one another to form compounds. It is important to be able to explain how atoms actually come together to form these compounds or chemical bonds. One of the three types of bonds is an ionic bond which is a bond between a metal atom and a nonmetal atom, or a cation and an anion. The Octet Rule is the driving force behind ionic bond formation. The octet rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds. When discussing the octet rule, we do not consider d or f electrons. Only the s and p electrons are involved in the octet rule, making it useful for the main group elements (elements not in the transition metal or inner-transition metal blocks); an octet in these atoms corresponds to an electron…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