Concept explainers
Interpretation: The use of arrow type 3 to draw resonating structures of cation should be explained.
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.
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
Organic Chemistry: A Guided Inquiry
- stuck on a questionarrow_forwardI need the answer as soon as possiblearrow_forwardhelp Be sure to answer all parts. Chloral, Cl3C―CH═O, reacts with water to form the sedative and hypnotic agent chloral hydrate, Cl3C―CH(OH)2. Draw Lewis structures for each of these substances. Draw them in decreasing molecular weight from left to right.arrow_forward
- Here's an electrostatic potential map for water (H₂O): Draw and upload here as an attachment (remember no heic files!) a Lewis structure that represents a water molecule (H₂O). Label with partial charges (8* and 8) the relative polarities of the atoms, if any. How did you determine whether there are partial charges and how did you determine where to put them?arrow_forwardTwo major contributing resonance structures are possible for the anion shown. One is given, but is incomplete. Complete the given structure by adding non-bonding electrons and formal charges. Draw the remaining structure, including non-bonding electrons and formal charges. Omit curved arrows. Draw formal charges and lone pairs to structure 1. H H H I. с | H H Complete structure 2. Add the pi bond, lone pairs and charges. H H H 1. A | 1 H H Harrow_forwardNow that you are familiar with electron density representations (like these electrostatic potential maps, EPMs)... Here's an electrostatic potential map for hydrogen molecule (H₂): HH Draw and upload here as an attachment (remember no heic files!) a Lewis structure that represents a hydrogen molecule (H₂). Label with partial charges (S* and 8) the relative polarities of the atoms. if anv.arrow_forward
- Please provide only typed answer solution no handwritten solution needed allowedarrow_forwardIn an ammonium, nitrogen has a valence of 4, and zero nonbonding electrons. What is the correct formal charge of nitrogen with 4 covalent bonds?arrow_forwardMake sure you read the questions very carefully to answer correctly. 1. Do the oxygen atoms have the same formal charge? VWrite "yes" or "no" in the blank. 2. If they have the same formal charge, what is the formal charge of the oxygen atoms? Write the number of formal charge with the sign. For example, +1 or -1 in the blank. If they do not have the same formal charge write "N/A" in the blank. 3. If they do not have the same charge, what are the formal charges of the oxygen atoms? Write the number of formal charges with the sign. For example, +1 or -1 in the blanks. If they do have the same formal charge write "N/A" in the blank. andarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY