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- 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 doviA. 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?Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules land ions. Draw a Lewis structure for CH4 and answer the following questions based on your drawing. 1. For the central carbon atom: The number of lone pairs The number of single bonds The number of double bonds= 2. The central carbon atom î A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet. = | =
- 1. Which of the following paired atoms 1 point is non-polar? * a. Br-F b. H-CI c. H-F d. H-P 2. Which of the following bonds has the highest polarity? * a. N-H b. C-H c. N-H d. C-O 3. Which of the following bonds has the lowest polarity? * a. N-H b. C-O c. C-H d. O-H 4. Which of the following is the correct decreasing electronegativity values? * a. F, O, N, C b. CI, S, Si, P c. As, Se, Br, F Od. H, Si, P, S 5. Which molecule has an ionic bond? а. Н-F b. Na-F c. F-F d. Cl-F 6. Which best describe the shape and 1 point polarity of CH4? * a. Tetrahedral polar b. Linear non-polar c. Tetrahedral non-polar d. Linear polar 7. Which statement is true about the non-polar molecules? * a. They are symmetric. b. They are asymmetric. c. They have lone pair on the central atom. d. They have charges 8. If a molecule has this symbol -, it means a. Negative b. Neutral C. Positive d. Cancel out 9. If a molecule has this symbol +, it means a. Charge b. Positive c. Negative d. Neutral 10. If a molecule…Use the symbols &* and & to indicate the polarity of the labeled bonds. a. Br-CI b. NH,OH c. CH3, NH2 d.4. Draw the Lewis dot structures for: (Note: make sure it satisfies the octet rule) a. NI3 b. CS2 c. N₂F2 d. CH₂Cl2 5. a. Which bond is more polar, H-Cl or H-O? b. Which of the following bonds is the most polar, that is, has the greatest ionic character: H-Br, N-H, N-O, P-Cl? 6. Write the formulas and names for the compounds of the following ions: 0²- F p3- K+ Ga³+
- 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 dainy1-What is the formal charge of the nitrogen atom in hydrogen cyanide (HCN)? a.5 b.−1 c.0 d.1 e.2 2-Which of the following diatomic molecules has the least number of valence electrons? a.N2 b.F2 c.O2 d.Cl2 e.NOWhich of the following bonds is least polar? Select one: a. Br-Br b. They are all nonpolar. C. C-O d. Н-С e. S-CI
- Why do covalent bonds form? 1. Because atoms always want to share electrons. II. Because electrons from one atom are attracted to the nucleus of another atom. III. Because the formation of a bond results in a stable system that would require the input of energy to change. IV. Because atoms always want an octet of electrons around them. 1. I only 2. II and IV 3. Ill only 4. I and II 5. II and III O O O O 1 3 2 5 42. NH₂ a. Lewis structure e. Electronic geometry_ d. Molecular shape_ Bond angle? b. Draw the different bonds and label their polarity.OM -. CH₁ a. Lewis structure c. Electronic geometry_ d. Molecular shape_ e. Bond angle? 2. NH3 b. Draw the different bonds and label their polarity.
