Please look at the picture to answer the questions below. 1a. How does the norma
ID: 991609 • Letter: P
Question
Please look at the picture to answer the questions below.1a. How does the normal C-H bond length (Google) compare to the C-F bond length you found for compound 8. My compound 8 bond length was 1.3A.
1 b. What other factor for atom X, needs to be considered besides bond length for the size of C-X group needs to be considered similar to that of C-H?
1c. Please look at the picture. Below is a calculated structure of CH3F showing the surface area with mesh representation of the molecular surface. Is flourine an exact replacement for hydrogen?
2. Please look at the picture for the whole question. The dihedral angle found in Exercise 2, Question 6 was not ideal for decarboxylation. An issue is that compound 8 has tetrahedral geometry at C-3 while intermediate carbocations 6 is trigon all planar. Forming a new Pi bond, we would want to be the p orbital of the carbocation to align with the C1-C2 bond whose electrons are moving from the Pi bond .If we look at structure 6 that is trigonal planar at C-3, what value for C1-C2-C3-C4 dihedral angle to closer to what value?
Answer the following Questions and submit with your lab report. 1. Fluorine is often substituted for hydrogen in structural variants of biologically active molecules, as was done to obtain a crystal structure of Diphosphomevalonate decarboxylase. It allows changing the electronic environment because of the electronegativity without dramatically changing the size requirements of the compound in the active site. How does the normal C-H bond length (Google) compare to the C-F bond length you found for compound 8? when d the bond of c-H bond engtho C-F. howevtn the lenghns ave not hs diRevcht from each othr What other factor for an atom, X, needs to be considered besides bond length for the size of a C-x group to be considered similar to that of C-H?Tent tan The atomic vadius of Flurine is smler than that Pyl ogen this may also rued e censidered Below is a calculated structure of CH3F showing the surface area with the mesh representation of the molecular surface. Is fluorine an exact spatial replacement for hydrogen? 2. The dihedral angle found in Exercise 2, Question 6 was not ideal for decarboxylation. Arn issue is that compound 8 has tetrahedral geometry at C-3, while intermediate carbocation 6 is trigonal planar. For forming a new pi bond, we would want the p orbital of the cationic carbon to align with the Ci-C2 bond whose electrons are moving to form the pi bond. If we look at structure 6 that is trigonal planar at C-3, what value for the C1-C2-C3-C4 dihedral angle to closer to what value?
Explanation / Answer
1-Bond length is the distance between centers of atoms bonded within a molecule.Bond length depends on three main factors- 1) Size of atoms 2) Bond strength 3) Multiplicity of bonds
Normal bond lenth of C-H is 1.09A^0.& C-F is 1.3A^0.Size of F-atom is greater then H-atom so bond lenth of C-F is greater.
2-Other factors are electronegativity, size of atoms , structure of molecule i.e, arrangmet of atom within molecule.
3-str. of CH3F- is tetrahedral.F has three lone pairs, with a deformation pattern different from the CH3.F is more electronegative then H-atom , so it is not exact replacement of H-atom.