Draw all the reasonable lewis structures for the

This preview shows page 2 - 5 out of 10 pages.

We have textbook solutions for you!
The document you are viewing contains questions related to this textbook.
Organic Chemistry
The document you are viewing contains questions related to this textbook.
Chapter 5 / Exercise 5.12
Organic Chemistry
Brown
Expert Verified
6. Draw all the reasonable Lewis structures for the following molecules. Also give the name of each molecule’s shape around the central atom and predict all bond angles. (a) [SbF 5 ] 2- (b) I 3 - (c) ClO 2 7. Observe the drawing of the arginine (C 6 H 15 N 4 O 2 ) + below. Give the bond angle for each of the five bonds indicated by arrows. Also give the molecular geometry around the central atom of each of the five labeled bonds. Bond Bond Angle Geometry at Central Atom a b c d e 8. Determine the formal charge on each of the oxygen (O) and nitrogen (N) atoms in the arginine molecule in the problem above. Does this seem like a reasonable Lewis structure for arginine? Why or why not?
We have textbook solutions for you!
The document you are viewing contains questions related to this textbook.
Organic Chemistry
The document you are viewing contains questions related to this textbook.
Chapter 5 / Exercise 5.12
Organic Chemistry
Brown
Expert Verified
9. Give name of the molecule shape and the bond angle around the atom in boldface type in the following molecules. (a) B F 3 (b) As F 3 (c)H 3 C Be CH 3 (d) S F 6 (e) Se F 3 + (f)H 3 C N = N CH 3 (g) (CH 3 ) 2 C =C(CH 3 ) 2 (h) H 3 C C C CH 3 (i) C O 2 (j) S F 4 10. The first ionization energy of chlorine (Cl) is 2.08 aJ. Which orbital’s Z eff can be determined from this value and what is the Z eff of this orbital? 11. The Z eff for a 3s orbital in phosphorous (P) is 5.64. The Z eff for a 3p orbital in the same atom is 4.89. How much energy is required to promote an electron from the 3s to the 3p orbital in phosphorous? 12. Draw two-dimensional cross-sections of a surface enclosing 95% of the electron probability for a 1s orbital in Ar, C and Na. Your labeled sketches should indicate any differences among the surfaces for these atoms. 13. (a) The complex [PtBrClFI] 2- is square planar. Draw all the different isomers of this complex. (b) The complex [ZnBrClFI] 2- is tetrahedral. Draw all the isomers of this complex. 14. How many unpaired electrons would you expect for the following complex ions? For each complex ion draw the d orbitals after splitting and represent electrons with arrows. (a) [RhCO 6 ] 3+ (low spin) (b) [Co(OH) 6 ] 4- (high spin) (c) [Co(CO) 4 ] 2- 15. The complex [Co(H 2 O) 6 ] 2+ is pink. The complex [CoCl 4 ] 2- is blue. Explain this difference in color. 16. One of the following complexes is green and the other is yellow: [Fe(H 2 O) 6 ] 2+ and K 4 [Fe(CN) 6 ]. Indicate which is which and explain your reasoning. 17. Draw two possible Lewis structures for C 3 H 4 . Is either structure linear? Explain.

  • Left Quote Icon

    Student Picture

  • Left Quote Icon

    Student Picture

  • Left Quote Icon

    Student Picture