Cut along dotted line. Name Assignment #1 Chemical Bonding (Predicting Bond Types) 1. What is a chemical bond? 2. Why do atoms form chemical bonds? 3. What distinguishes an ionic bond from a covalent bond? 4. What distinguishes a polar covalent bond from a nonpolar covalent bond? 5. What is a dipole? What type of bond produces a dipole? 6. How can you identify the negative and positive dipoles in a polar covalent bond? 7. According to the general rules of electronegativities, what type of bond is formed by each of the following pairs of elements? If the bond is polar covalent, identify the negative dipole (δ-) and the positive dipole (δ+). a. potassium and chlorine b. sulfur and sulfur c. carbon and bromine d. zinc and oxygen 8. Order the following covalent bonds from least to most polar. a. H Cl b. H Br c. H Se d. H C e. F F 9. What type of bond do nonmetals generally form with other nonmetals? 10. What type of bond is generally formed between the alkali metals and the halogens? 11. What type of bond is generally formed between the halogens and the oxygen group?
Assignment #2 Lewis Electron Dot Diagrams 12. Draw the Lewis dot representations for each of the following neutral atoms: a. sodium e. magnesium b. helium f. fluorine c. boron g. nitrogen d. krypton h. oxygen 13. Distinguish between single bonds, double bonds and triple bonds. 14. Explain why the following Lewis structures for CHClO is incorrect. H C O Cl 15. Draw Lewis structures (or structural formulas) for the following molecules: a. Cl 2 e. carbon dioxide (CO 2 ) b. hydrogen sulfide (H 2 S) c. nitrogen trichloride (NCl 3 ) f. methyl chloride (CH 3 Cl) g. ethyne (C 2 H 2 ) d. silicon tetrahydride (SiH 4 ) h. Phosphorus trihydride (PH 3 ) 16. Which molecule(s) in question 15 include double bonds? 17. Which molecule(s) in question 15 have triple bonds?
Cut along dotted line. Name Assignment #3 Binary Molecular Nomenclature 18. Write the correct formula for each of the following compounds. a. carbon monoxide b. sulfur dioxide c. diphosphorus pentoxide d. nitrogen dioxide e. carbon dioxide f. phosphorus trichloride g. dinitrogen pentoxide h. phosphorus pentabromide i. silicon dioxide j. selenium tetrafluoride 19. Write the correct name for each of the following formulas. a. N 2 O b. P 3 N 5 c. NI 3 d. N 2 O 4 e. P 4 O 10 f. SO 3 g. SiI 4 h. N 2 O 3 i. CCl 4 j. As 2 O 5
Assignment #4 Exceptions to the Octet Rule and Coordinate Covalent Bonding 20. What is a coordinate covalent bond? 21. Draw Lewis sructures (or structural diagrams) for the following polyatomic ions. a. OH - b. ClO 3-22. State the Octet Rule. Name a compound in which the central atom does not follow this rule. 23. Draw Lewis structures (or structural diagrams) for the following molecules. a. BeH 2 c. PCl 5 b. SF 6 d. BH 3 24. What are resonance structures? Write the possible resonance structures for NO 3 -.
Assignment #5 Molecular Shapes and Polarity 25. What do the letters VSEPR stand for? What is the basic assumption of this theory? 26. How can you distinguish between a 3-atom linear molecule and a bent molecule? Give an example of each. 27. How can you distinguish between a trigonal pyramidal molecule and a trigonal planar molecule? Give an example of each. 28. Why is the bond angle in a trigonal pyramidal molecule different from that in a tetrahedral molecule? 29. What is the difference between a polar molecule and a nonpolar molecule? 30. What makes a molecule polar? 31. Give two examples of polar molecules that contain polar bonds. Give two examples of nonpolar molecules that contain polar bonds.
32. Complete the following table: Formula Lewis Structure (or Structural Formula) Name of Shape Molecular Polarity SbH 3 Cl 2 O BeH 2 SiF 4 PI 5 SCl 6 CO 2 HCN AsCl 3 BH 3
Assignment #6 Intermolecular Forces of Attraction 33. What is a van der Waals force? Is it an example of a chemical bond? Why or why not? 34. What is hydrogen bonding? Is it an example of a chemical bond? Give an example of a substance that would exhibit hydrogen bonding. 35. Arrange the following intermolecular attractions in order of increasing strength: dipole-dipole interactions, London dispersion forces, hydrogen bonds. 36. What is a temporary dipole? What types of molecules are capable of having temporary dipoles? What is the name of the van der Waals force that involves temporary dipoles? 37. For different substances of similar molar mass, which type of intermolecular force is the weakest? Give an example of a molecule that would exhibit this force. 38. What type of intermolecular forces of attraction would be exhibited by each of the following substances? a. PF 3 b. HF c. N 2 d. BeH 2 39. The following substances have roughly the same molar mass. Which one is most likely to have the highest boiling point: H2S, F2, or CO2? Explain your choice.