6. Breaking peptide bonds is hard.a) Draw steps for (i) addition of water and (ii) elimination of the amine from the CO-NH bondof R-CO-NH-R' ("the reactant"). Include any intermediate steps like proton transfer.b) Draw a resonance structure for the reactant.c) What is the hybridization of the reactant's indicated (i) C, (ii) N, and (iii) O?d) What 2 factors make this hydrolysis reaction slower than hydrolysis of R-co-S-R'-?e) In nature, peptide bonds are hydrolyzed by enzymes including cysteine proteases. Cysteine'sstructure isHSHOÑH2Draw nucleophilic attack of cysteine's thiol on the reactant with the arrow formalism.f) In the resulting tetrahedral intermediate, what is the best leaving group?g) Show how an acidic residue of an enzyme (which you can draw as HA) might help facilitatedeparture of the amine as the leaving group, by drawing a suitable reaction mechanism(including the acid proton) using the arrow formalism.

Peptide bond are hard to hydrolyse because of the Resonace occuring in peptide bond . Removal of…

Answered: 6. Breaking peptide bonds is hard. a)…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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a) Which atom is most likely to be protonated on the structure below? Explain. b) Which atomic/hybrid orbitals are combining to form the indicated bonds? H₂N OH
a) Consider a molecule of acetone cyanohydrin, shown below. What is the hybridization and molecular geometry at CA, CB, and O? (b) For Carbon B (CB) and nitrogen (N), draw orbital energy diagrams showing the orbitals involved in bonding after hybridization. Be sure to fill the orbitals appropriately with valence electrons. c) In your diagrams in part (b), which orbitals are involved in sigma and pi bonding? Orbitals Involved in Sigma Bonding Orbitals Involved in Pi Bonding 2p sp sp2 sp3 2p sp sp2 sp3 (d) In a sample containing many molecules of acetone cyanohydrin (and no other substances), what type(s) of intermolecular forces could be present? Choose all that apply. Covalent Bonds Hydrogen Bonds Dipole-Dipole Forces London Dispersion Forces
What is the hybridization of the N atom in this molecule? What are the hybridizations of the other 4 atoms indicated? ............................ H-G-C-ċ-ċ-ö-H H H :N-H 2 E→:ö: HHO: A H
Using Valence Bond Theory, NOT the VSEPR model, show what orbitals the central carbon atom is using in the compound HCN (Drawing a Lewis Structure is good, but not enough). What is the bond angle and molecular geometry in the HCN molecule? DRAW AND NAME THE ORBITALS FOR ALL 3 ATOMS BEFORE AND AFTER BONDS FORM. A FEW DRAWINGS SHOWING PARTS OF YOUR ANSWER WOULD BE A LOT BETTER THAN ONE DRAWING ATTEMPTING TO SHOW ALL OF IT !! a) b) c) a)
Use valence bond theory to describe the hybridized bonding in the following molecule. (i) What is the shape of this molecule? (ii) What is the hybridization of the central atom? (iii) Indicate which orbitals are used to form the following bonds: a) Br-CI b) Br-O (o-bond) c) Br-O (1T- :Br. bond) ČI contain the non-bonding electrons on (iv) Indicate which orbital the central atom. (v) Is this molecule hypervalent or hypovalent?
The Lewis structure of an organic compound is shown below. Determine the orbitals used in bonding, as well as the number of sigma and pi bonds. 1サー= 10 H. N: H. 11 Total sigma bonds: [Select] Total pi bonds: [Select ] Write "none" if no orbital of that type is used to bond. Unhybridized orbital used to Hybridized orbital used to Atom bond bond [ Select ] [ Select ] [ Select] [ Select ] C # 2 [ Select ] [ Select ] [ Select ] [ Select]
a) Construct the molecular orbitals of NO-. b) Between the molecular HNO and HON, on the basis of your estimation and your answer to part a, which structure is favored?
Complete the following table by providing theVSEPR-name and hybridisation (sp, sp2 or sp3) ofthe atom indicated by the arrow.
3. For each of the following compounds, indicate the total number of valence electrons - VE, draw the Lewis structure(s), calculate the bond order - BO- of the central ion, calculate the formal charge of each atom in the molecule, and determine the hybridization of the central ion. Show the formal charges in () to the upper right of each atom, then put the bond order and central atom hybridization (CAH - Ex. sp) on the lines provided. Under the structure (resonance structures if the molecule has them), name the general and specific shapes of the molecule. a) BF3 in novaw VE = b) XeF4 c) SO3 General Shape (Electron Domain Geometry) = Specific Shape (Molecular Geometry) = d) SO3²- (latot) 9V General Shape (Electron Domain Geometry) = Specific Shape (Molecular Geometry) = noi General Shape (Electron Domain Geometry)=niku (1) Specific Shape (Molecular Geometry) = Syriw bo sidodong pnom srit ai esutaunta General Shape (Electron Domain Geometry) = Specific Shape (Molecular Geometry) = BO =…
Consider a molecule AB, where element A has 6 valence electrons and B has 7 valence electrons. If the AEn for each bond = 1.2, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity.
In the spaces provided below, use Lewis structures to show each entire chemical reaction between the two given reactants. Then, indicate the hybridization of each central atom. Do not name the products
Consider a molecule AB3, where both element A and B have 7 valence electrons. If the AFn for each bond = 0.4, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity. F8 F9 F11 F12 % * 5 7 8 9 Y P CO

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