Practice Problems Compilation

Rank the highlighted bonds below in order of increasing length and in order of increasing strength. F (a) Length: shortest (Choose one) Strength: weakest (Choose one) (c) Cl (b) Br <(Choose one) <(Choose one) <(Choose one) <(Choose one) longest strongest X

Paraphrasing .ewriting Tool Car note Pirate Ship BLACKBOARD [Review Topics] [References) For each example, specify whether the two structures are resonance contributors to the same resonance hybrid. a) H,C=CH-CH2 H3C-CH=CH2 b) yes e c) Submit Answer Retry Entire Group 9 more group attempts remaining reg (Previous Next) Show Hint nortal stv MacBook Air So F10 23 F12 2$ & 4 del P { } J K > ? command option

Solve correctly please. Should correct

Choose the resonance structure that results from the arrow pushing scheme below: A H OH Give detailed Solution with explanation needed of all options.don't give Handwritten answer

Organic chem question please help

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H3C-C-0 - O Below is the Lewis structure of CH3CO2, which has one other resonance structure. H₂C-C=Ö 1 :0: Check Complete the resonance structure by dragging bonds and electron lone pairs to their appropriate positions. Then click Check. Submit Answer Next) (3 of 3) Clear Retry Entire Group Show Hint 9 more group attempts remaining Cengage Learning | Cengage Technical Support Previous Next Save and Exit

Using electrons and/or lone pairs in the following conjugated system, create a resonance form by moving electrons as far as possible. Be sure to include all lone pairs and charges. Part: 0 / 2 Part 1 of 2 Add curved arrow notation to show how electrons will move to form a different resonance form. + 0:

I got the net charge -1 but the system shows it wrong.  The formula I used:  Formal charge= Valence electron-(bonding electrons +individual lone pair)

Please don't provide handwritten solution .....

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Show work with explanation needed..don't give Ai generated solution. don't give Handwritten answer. don't copy the answer anywhere

Give correct detailed Solution with explanation needed...don't give Handwritten answer

None

Answer all parts (A, B, & C) a) Draw the Lewis structure of the nitrate ion, NO3 -, including all resonance forms and formal charges. What is the geometry of the nitrate ion? b) True or False: Because of the double bond in the nitrate ion, two bond angles are greater than 120° and one bond angle is less than 120°. Explain your answer. c) What is the hybridization of the N in nitrate?

Please help

121) Which of these would you expect to have significant resonance stabilization energy? a) I b) II I N: II c) III d) All of these choices. e) None of these choices. Answer: D III

please answer letter g, h, and i

Draw and explain how, with arrows indicating reasonance

Hello can I get help with the following question please? I am confused and do not understand. Question: Given the following compound draw curved arrows and the resonance forms that result

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I am wondering why there is a need for resoance structures if the molecule already has a neutral charge. Wouldn't these all be insignificant resonance structures (as there is unnecessary charge separation)? Perhaps they are only depicting these structures for the purpose of showing high/low electron density (which was what the question was asking for)?  1 picture shows answer, another shows problem (it is (b)).

please answer letter j, k, and l

Give all possible resonance structures for the given molecule and identify the major contributor (just give the corresponding number level) to the resonance. Also draw the resonance hybrid for the molecule. Show curved arrow notation to indicate the movement of electrons.

For each bond, show the direction of polarity by placing a + sign next to the atom expected to have a partial positive charge and a-sign next to the atom expected to have a partial negative charge. (A) (B) Br (C) For The most polar bond is Submit Answer Try Another Version 4 hem attempts remaining

Question: Which carbenium ion is most stable * (CH,),cCH, (CH,),CCH,CH, B) C) (CH,),CHCHCH, D) CH,CH,CHCH,CH, A) O (A) O (B) O (C) O (D)

Part B How many equivalent resonance structures can be drawn for the SO, molecule where the central sulfur obeys the octet rule (including the one you've drawn)? ? Submit Request Answer Part C What is the formal charge on the central sulfur atom in the Lewis Structure for SO, where the octet rule is obeyed? Submit Request Answer

give reason for both correct and incorrect option

Please quick answer

Question attached

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Q)4

Does +I effect help in resonance and -I effect reduce the effect of resonance? Answer Follow · 1 Request

Criteria for success All molecular drawings must be valid Lewis structures (octet rule, formal charge, valence, geometry). Curved arrows will be interpreted very strictly. Thus, they must clearly indicate the origin and destination of electron delocalization. Tasks 1. Generate at least three reasonable resonance contributors of the molecule in Fig. 3. 2. Rank reasonance contributors from least significant to most significant (#1 = most significant) and explain your choice. 3. Are the lone pairs of electrons on alcohol groups localized or delocalized? Briefly explain. HO OH F Figure 3: Molecule with delocalized electrons