Answer the following questions about compound A.a. Label the shortest C-C single bond.b. Label the longest C-C single bond.c. Considering all the bonds, label the shortest C-C bond.d. Label the weakest C-C bond.e. Label the strongest C-H bond.f. Explain why bond (1) and bond (2) are different in length, even though they are both C-Csingle bonds.(2)

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Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter3: Electron Orbitals

Section: Chapter Questions

Problem 11CTQ: On the left side of Figure 3.6, label the areas shown with a dotted line where... one bond can...

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Answer the following questions about compound a. Label the shortest C–C single bond. b. Label the longest C–C single bond. c. Considering all the bonds, label the shortest C–C bond. d. Label the weakest C–C bond. e.Label the strongest C–H bond. f.Explain why bond [1] and bond [2] are different in length, even though they are both C–C single bonds.
. Answer the following questions about compound A. [2] [1] A Label the shortest C- C single bond. Explain b. Label the longest C – C single bond. Explain c. Considering all the bonds, label the shortest C – C bond. Explain. d. Label the weakest C – C bond. Explain. e. Label the strongest C - H bond. f. Explain why bond [1] and bond [2] are different in length, even though they are both C– C single а. lain. bonds.
A. CHF i. Best Lewis Structure B. HNO (H is connected to one of the O's) i. Best Lewis Structure ii. Electron geometry on the C atom ii. Electron geometry on the N atom iii. Approximate bond angles about the C atom iii. Approximate bond angles around the N atom v. Draw the shape with in and out wedges (as necessary) and dipole arrows around the C atom. v. Draw the shape with in and out wedges (as necessary) and dipole arrows around the N atom. vi. Is the molecule polar or nonpolar? vi. Is the molecule polar or nonpolar?
2. NH₂ a. Lewis structure e. Electronic geometry_ d. Molecular shape_ Bond angle? b. Draw the different bonds and label their polarity.
3. H₂S a. Lewis structure c. Electronic geometry_ d. Molecular shape_ e. Bond angle? b. Draw the different bonds and label their polarity. bl ob veluoslem dovi
Draw a second resonance structure for each species in parts (a) and (b). Draw two additional resonance structures for the ion in part (c). ci: a. CH3 C H H I C H CH3 b. H H H c. CH3 :O: :O: II C. || C. I H CH3
Draw a Lewis structure for SiF5- and answer the following questions based on your drawing. 1. For the central silicon atom: ... The number of lone pairs = ____ The number of single bonds = ____ The number of double bonds = ____ 2. The central silicon atom (A,B, or C) ... A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet.
Question 48 48. Which of the following statements are true? 1. 11. III. IV. The electrons in each molecule tend to orient themselves around the most electronegative element. Each molecular drawing follows the localized electron model. Both HF and CO₂ are linear molecules and therefore polar. The bond angles of NH3 are slightly less than 109.5° because the lone pair compresses the angles between the bonding pairs. a. I, III, IV b. I, II, IV c. I, II, III d. II, IV e. All of the above statements are correct. C B esc E Q @ 2 W # 3 E $ 4 * R % 5 T < 6 Y & 7 8 U
1. Consider the structure shown below and then answer the following questions. a. Complete the structure by adding the missing formal charges. All atoms and lone pairs are explicitly shown. (Hint: Consider the number of bonds neutral atoms have.) :Ö: H ‚H H H b. Draw two more resonance structures of the molecule from part a by adding the missing î bonds, lone pairs, and formal charges. All atoms in both structures should possess an octet. (All atoms and o bonds are drawn for you; remember, only lone pairs and bonds move in resonance structures.) Additional guidelines are given for each structure. All atoms in this structure will be neutral (no formal charges). One oxygen atom has a +1 formal charge and one oxygen atom has a -1 formal charge. H H H H H H H H H
2. NH3 a. Lewis structure c. Electronic geometry_ d. Molecular shape_ Bond angle? e. pos b. Draw the different bonds and label their polarity. di Sant sqyp brod dainy
For each molecule below, a. Draw the lewis structure, using wedges and dashes to indicate the VSEPR shape as necessary. b. Draw the bond dipole for all polar bonds. c. Determine if the overall molecule is polar or nonpolar. first molecule: H₂ second molecule: CO₂ third molecule: H₂O
1. How do you know which covalent bond is stronger? 2. Which is the strongest bond and why?

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