swer the following questions about the Lewis structure for the organic molecule CH₂CHCHCH₂ (see examples in Chapter 10) ere are valence electrons. The molecule has single bonds, ch central C has nce there are 0 b. 1 c. 2 triple bonds. d. 3 e. 4 REDS, the shape is polar covalent bonds, the molecule is f. 5 h. 10 i. 12 j. 14 k. 16 s. 36 t. diatomic u. pyramidal y. trigonal planar z. bent aa. 120° ff. nonpolar ee. polar gg. ionic 22 n. 24 o. 26 p. 30 q. 32 linear w. monoatomic ions x. tetrahedral no bond angles, no central atom dd. 109.5° g. 7 r. 34 and the bond angles are I. 18 bb. 180° hh. C and C double bonds, and

Which of the following compounds is likely to have the strongest H-X bond? a.HBr (141 pm) b.HI (161 pm) c.HF (92 pm) d.H2S (134 pm) e.HCl (127 pm)

ents V Soul (TV series) O REPRESENTATIONS OF ORGANIC MOLECULES Drawing a skeletal structure from a Lewis structure Convert the Lewis structure below into a skeletal structure. Н—С— Н H. H- H- Н—С—Н H. HH H. H- Н—С—С—С—С—С—С—С- Н C=C H- H. H. H. Н—С— Н H. ct+ Click and drag to start drawing a structure. HIC CIH HIC

Consider the molecules — BrF5. A. Draw the best Lewis structure for this molecule. Label any atoms with nonzero formal charge. B. Label each bond angle. As part of your answer be sure to include if it is more or less than the ideal bond angle.  C. What is the electron geometry around the bromine atom? D. Are the bonds in the molecule polar? E. Is the overall molecule polar? — CH2 F2 . A. Draw the best Lewis structure for this molecule. B. Label each bond angle. Answers for A-D here: C. Redraw the shape of the molecule. Draw all dipoles. D. Is the overall molecule polar? — Consider the molecule CH2 CF2 . A. Draw the best Lewis structure for this molecule. B. Label each bond angle. C. Redraw the shape of the molecule (according to the exacting specifications of your instructor). Draw all dipoles. D. Is the overall molecule polar?

The formula for nitryl chloride is CINO2 (in which N is the central atom). a.Draw the Lewis structure for the molecule, including all resonance structures. b.What is the N-O bond order? c.Describe the electron-pair and molecular geometries and give values for all bond angles. d.What is the most polar bond in the molecule? Is the molecule polar? e.The computer program used to calculate electrostatic potential surfaces gave the following charges on atoms in the molecule: A =-0.03, B = -0.26, and C = +0.56. Identify the atoms A, B, and C. Are these calculated charges in accord with your predictions?

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

Help

8. For each molecular fomula, detem ine the electron pair geom etry (EPG), make a 3-dimensional representation, and determ ine the molecular geometry. Determine whether the molecule is polar or non- polar. All of these have central atoms surounded by term inal atom s/one pairs only. Formula A. CHF3 Lewis structure EPG 3-D drawing Mol Geom. Polar molecule? B. SF2

5 c

What's the answer?