Question 2 Consider the following Bronsted-Lowry acid/base reaction. (Note that not all hydrogens or lone pair electrons are drawn in) [1] Draw the products of the reaction [2] Use curved arrows to show the movement of electrons to form the products. Be sure to draw in lone pairs of electrons if they are directly involved in a step. [3] Label the acid, base, conjugate acid, and conjugate base [4] Indicate which side equilibrium will favor and explain why. H H N Na NH₂

Question 2 Consider the following Bronsted-Lowry acid/base reaction. (Note that not all hydrogens or lone pair electrons are drawn in) [1] Draw the products of the reaction [2] Use curved arrows to show the movement of electrons to form the products. Be sure to draw in lone pairs of electrons if they are directly involved in a step. [3] Label the acid, base, conjugate acid, and conjugate base [4] Indicate which side equilibrium will favor and explain why. H H N Na NH₂

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter4: Acids And Bases

Section: Chapter Questions

Problem 4.33P: Complete the equation for the reaction between each Lewis acid-base pair. In each equation, label...

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Complete the equation for the reaction between each Lewis acid-base pair. In each equation, label which starting material is the Lewis acid and which is the Lewis base; use curved arrows to show the flow of electrons in each reaction. In doing this problem, it is essential that you show valence electrons for all atoms participating in each reaction. (a) (b) (c) (d)
The following are equivalent ways of asking about the acidity of an H atom: • What is the most acidic H on the molecule? • Which H is associated with the published pKa value? • Which H on the molecule is easiest to remove? • Which H on the molecule takes the least energy to remove? • Which bond to an H is most polarized? • For which H atom is removal least uphill in energy? • Which bond to an H atom, when broken, results in the lowest PE conjugate base? We will often find the last of these questions is easiest to answer. To do this, find all the different Hatoms on the molecule, and draw all possible conjugate bases.Only the lowest-energy one is the “real” conjugate base. Identify this structure, and you have found the most acidic H. Use this strategy to find the most acidic H on each of the following molecules. Note: Each structure hasat least three different kinds of H’s, so draw at least three unique conjugate bases for each.
(E) Label each of the following as strong acid, strong base, or neither.
Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. In addition, write Lewis structures for all starting materials and products. Label the original acid and its conjugate base; label the original base and its conjugate acid. If you are uncertain about which substance in each equation is the proton donor, refer to Table 4.1 for the relative strengths of proton acids. (a) NH3+HCl (b) CH3CH2O+HCl (c) HCO3+OH (d) CH3COO+NH4+
Answer true or false to the following statements about the mechanism of acid-base reactions. (a) The acid and base must encounter each other by a collision in order for the proton to transfer. (b) All collisions between acids and bases result in proton transfer. (c) During an acid-base reaction the lone pair on the base fills the A-H antibonding sigma orbital.
1.Draw the conjugate acid with formal charge(s) below. If there are electrons around any of the atoms ignore them for now. The details will be addressed in the next section. 2. Now specify the details of the structure that was drawn.N with three single bonds and 2 electrons around the atom in the base becomes a N atom with (blank) bonds. (Negative Charge, No Charge, Positive Charge) ,and (BLANK) electron(s) around the atom in the conjugate acid.
a. Which of the acids in the table above has the strongest conjugate base? b. What is the structure of the strongest acid in the table above?
Label the following reactions as Acid, Base, Conjugate Acid and Conjugate base using the Bronsted Lowry Model. Recall that an acid donates a proton to become a conjugate base, and a base accepts and proton to form a conjugate acid. HCO3- + NH3® CO3-2 + NH4+ HCl + H2O ® H3O+ + Cl- CH3COOH + H2O ® H3O+ + CH3COO- HOCl + NH3 ® NH4+ + ClO-
For each pair of bases, identify the stronger base.
List the following in order from strongest base to weakest base:
1.) Please draw all arrows and indicate whether they are breaking or creating a bond 2.) Please draw products and label each as the conjugate base/conjugate acid.