Acidity of the molecule can be explain based on the resonance stability of the corresponding conjugate base
More stable the conjugate base more the acidity of the molecule
so benzene sulphonic acid is more acidic than benzoic acid
second problem
Determine the stronger acid in each of the following resonance structures. Tohowing pairs. Explain your answer...
Draw two additional resonance structures for the following compound. Include Lone Pairs in your answer. Do not include initial structure and resonance arrow in your answer.
D) For each pair of molecules below: - draw the stronger acid - explain your choice - for the stronger acid of each pair, also draw and label its conjugate base (including any major resonance structures, if appropriate) i) NHy NHs v)
Predict which acid is stronger (circle it) and use chemical structures to explain why. I am assuming I did not pick the right acid because I got this question wrong. Please explain. This molecule has more resonance
EO 3- resonance structures, formal charges, stability 1. Draw ONE possible significant additional resonance structure for each of the following ions. Use curved arrows to show the movement of electrons that creates each new resonance structure. (Hint: lone pairs are not shown. Start by drawing in all one pairs, and include all lone pairs and formal charges in your additional resonance structure.) Page 1 of 3 2. For each structure, draw the resonance structure that is indicated by the curved...
Draw the curved arrows and the resulting resonance structure for the following structures. Include lone pairs and charges in your structure. Edit CH
Using resonance structures as part of your answer, explain why Br in bromobenzene is: a. A mild ring deactivator b. An o-, p-director. [Note: It is not enough to use resonance structures from part "a" to "prove" part "b". One must show that o-, p-attack is faster, i.e. has lower Ea (AGa) by actually showing an electrophile, e.g. the generalized E+, attacking at the o-, m-& p-positions and, using Hammond's Principle, explain why the o-, p-attacks are favored.] Explain what...
ch 22 Draw a resonance structure, complete with all formal charges and lone (unshared) electron pairs, that shows the resonance interaction of the carboxy with the para position in benzoic acid. OH benzoic acid • You do not have to consider stereochemistry. • Include all valence lone pairs in your answer. • In cases where there is more than one answer, just draw one. с P opy to // [Review Topics IReferences Draw a resonance structure, complete with all formal...
explain please In which of the following pairs of acids is the first compound the stronger acid? a. HBr HC1 d. HBrO2 HC102 e. H Se HBE b. H,502 HNO3 Cl C- E-O- - c. H- H-C- OH "o=o - OH
5. Draw the number of resonance structures indicated, your structures must fulfill the octet rule. This exercise serves to develop a sense of which Lewis Structures are reasonable so think whether what you are proposing makes sense. Assign formal charges and determine which structure is more likely, major contributor. Draw a box around this structure. Note: it is possible to have more than one major contributor. In that case, indicate these equivalent structures by drawing a box around all of...
In each of the following ion pairs, determine which ion is more stable. Use resonance structures to justify your answers. C) Etz-CH2 CH-CEN i