why are there 0 sites of unsaturation? wouldnt there be 1? 14.2. To calculate the number of л bonds and rings in a molecule-collectively called the “sites ofunsaturation" apply the formula given below:-n = number of C atoms(2n+2)-m-p+qm = number of H atomsNo. of sites of unsaturation =p = number of halogen atoms2q = number of N atomsFor the molecule under consideration,C6H13 NO2n = 6m = 139 = 1No. of sites of unsaturation =2(6)+213 +12= 0 sites of unsaturationThis molecule has no rings or л bonds.

Molecular Formula: C6H13NO2D.O.U = (2C + 2 - H + N)/2 = [2(6) + 2 - 13 +1]/2 = (12 + 2 -…

Answered: 14.2. To calculate the number of л…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter7: Molecular Structures

Section: Chapter Questions

Problem 7.BCP

See similar textbooks

Similar questions

indicate the approximate values for the indicated bond angles in the following molecules. 1 (a) H 0-N=ö 2. Н 4 H. (b) H C-c=0 H H H (c) H-N-O–H . H. (d) H-C-C=N: H.
Specify the local electron geometries about the atoms labelled a-d. Unshared electron pairs affect local geometry and are included in the structural formula.For each atom enter one of the following:tetrahedral, square planar, trigonal planar, trigonal pyramidal, or linear.a b c and d???
Draw a Lewis structure for the C4Hg molecule usıng the connectivity shown in the spacefillıng model in the window. Gray = C; white = H; red = 0; blue = N; dark green = Cl; brown = Br; light green = F; purple = I; yellow = S; orange = P. %3D Use your drawing to answer the following questions. The total number of electrons in C-H bonds = The number of C-C single bonds =| The number of C=C double bonds = Previous Next The total number of unshared pairs %3D
2. In measurements of the structure of molecules, some interesting trends are observed. The bond angle (H-C-H) in CH4 is 109°, as we would expect for a molecule in the tetrahedral VSEPR class. However, other molecules in the same VSEPR class, such as ammonia (NH3, H-N-H= 107°) and water (H2O, H-O-H = 105°), have smaller bond angles than expected. Explain the basis for the bond angle trend: CH4 > NH3 > H2O. %3D
13. (a) For the following condensed formulas draw the Lewis structures. Include lone pairs in your drawing, 03 (ozone) CH3COOH (b) Write in any non-zero formal charge (c) Give the molecular geometry around the second carbon in CH3COOH (d) What is the hybridization of the second carbon in CH3COOH (e) Give the molecular geometry around the middle O in O3. (f) What is the hybridization of the middle O in O3 14. Draw the line structure of the following compounds? a) (CH3)3CCH₂CH₂NHCH3 15. a. Draw two constitutional isomers with the formula C₂HgBrCl Isomer 1 16. For the molecule below, b) CH3CHO b. Describe ALL the intermolecular forces isomer 1 can participate in OH Isomer 2 3 (a) Circle all functional groups present. (b) Label two of the functional groups next to where you circled them
Use the following set of assumptions to estimate the CN bond length in fulminic acid: 1) only the two best structures contribute to the true structure 2) the best structure contributes 75%, 3) the CN single bond is 1.47 pm, the double is 1.32 pm and the triple is L.16 pm. Enter your answer with 2 significant figures as a number with no units. Structure I Structure II Structure III H-C=N=0 H-C=N-0 ŌI H-C-N=01 VFullsc 10:41 PM
5.) a.) F-S-F bond angles in OSF4 are 115° and 164° while F-S-F bond angles in SF4 are 101° and 173°. Draw the structure you would expect for OSF4 and SF4, and suggest a reasonable explanation for the observed F-S-F bond angles. b.) predict the shapes of the molecule (Me3P) SBCI3 and indicate approximate bond angles (ex. >180 or <180, etc.) around the central atom. Explain your reasoning.
Need help figuring out the correct angles and the structure of letter C
3.
1. What are the VSEPR shapes (i.e., molecular geometries) associated with the nitrogen atoms in this molecule? (A) (B) (C) (D) I bent bent bent tetrahedral 2. How many sp² hybridized carbon atoms are present in this structure? (A) 1 HO. Br II trigonal pyramidal N. bent trigonal pyramidal I bent (A) aldehyde, ether, sulfide (B) aldehyde, ketone, thiol (C) amide, ketone, sulfide (D) amide, ether, ester II NH₂ III III trigonal pyramidal (B) 4 (C) 5 (D) 6 3. Which functional groups are NOT present in this molecule? trigonal pyramidal tetrahedral trigonal pyramidal
Im supposed to draw diasteromers of this and dont know why its wrong
Please explain the following!

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS