c. How many mm Hg are in 3.5 atm? b. How many seconds are in 28 hours?

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1 Chemistry Fall Final Study Guide Unit 1: Matter, Elements & the Periodic Table 1. How many sig figs are in the following numbers? a. 89,501 b c. 5,700 d. 2,000. e Use the Conversion Factor Sheet in your Glossary to solve the following problems. Show your work using bridges and correct amount of sig figs in your answer! a. How many hours is 23,870 minutes? c. How many mm Hg are in 3.5 atm? b. How many seconds are in 28 hours? 3. What is matter? Name 3 things that are matter and 3 things that are NOT matter. 4. What is the different between a physical property and a chemical property? 5. Label the following properties of matter as either physical or chemical: a. Calculating the density of gold d. Bleaching your hair b. Salt dissolving in water e. Shooting off fireworks c. Melting Ice f. Sublimation of dry ice 6. Solve the following density problems. Round to the correct number of sig figs. a. What is the density of a piece of wood that has a mass of 25.0 grams and a volume of 29.4 cm 3? b. Mercury metal is poured into a graduated cylinder that holds exactly 22.5 ml. The mercury used to fill the cylinder weighs g. From this information, calculate the density of mercury. c. What is the weight of the ethyl alcohol that exactly fills a ml container? The density of ethyl alcohol is g/ml. d. What volume of silver metal will weigh exactly g. The density of silver is 10.5 g/cm How is the periodic table organized? What are groups and periods? a. Where are the metals found on the periodic table? Where are the nonmetals found on the periodic table? What is Hydrogen? b. What are the names for the groups 1A, 2A, 3B-12B, 7A and 8A? 8. On the periodic table, what are the trends for atomic mass atomic numbers, atomic radii (size), and reactivity as you move across a period and down a group? Unit 2: Atomic Structure 9. Which part gives the identity of the atom? Which part(s) make up most of the (atomic) mass of the atom? Which makes up very little? 10. What does the periodic table tell us about the parts of the atom: a. Find the following for the atoms Aluminum, Chlorine, and Magnesium: i. Atomic # vi. # of valence electrons ii. # of protons vii. # of core electrons iii. # of electrons viii. # of neutrons for 2 of its iv. Average atomic mass isotopes v. Name of the group it is in ix. Draw the 2 isotopes of the (NOT the #) atom

2 11. What is the atomic number and atomic mass of phosphorus and strontium? a. What is the difference between atomic number and atomic mass? 12. What is an isotope? Name two possible isotopes for carbon and potassium. Use isotope symbol. 13. a. Write the equation for the alpha decay of astatine b. Write the equation for the beta decay of neptunium c. What is more harmful alpha particles, beta particles, or gamma rays? 14. What are valence electrons? a. How many valence electrons do Mg, S, and Al have? 15. Answer the following for the atoms of Carbon, Barium, and Bromine: a. How many total electrons does it have? b. How many valence electrons are there? c. How many core electrons are there? d. How many shells will it have? 16. What elements with the following electron configurations of a. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 1 b. 1s 2 2s 2 2p 6 3s 2 3p Write the electron configuration for each of the following atoms: Be, Si, Tc, I and Cs. Unit 3: Chemical Bonding 18. What are ions? What are cations and anions? 19. In ionic bonds, metals tend to lose electrons and nonmetals gain electrons. What happens to these elements to achieve noble electron configuration? What charge will the element form? a. oxygen b. chlorine c. sodium d. barium 20. Fill in the following chart: Group #A # valence e- Lose/gain e-? Oxidation #? Type of ion? I A II A III A IV A V A VI A VII A VIII A 21. a. What is the chemical formula and name of the compound formed when beryllium reacts with fluorine? b. What is the chemical formula and name of the compound formed when potassium reacts with sulfur? 22. What is a crystal lattice? Why do ionic compounds form a crystal lattice structure? Draw a picture of NaCl in a crystal lattice.

3 23. What are the chemical formula and charge for the following polyatomic ions? a. Sulfate b. Hydroxide c. Nitrate d. Nitrite e. Sulfite f. Chromate g. Carbonate h. Ammonium 24. Write the correct name for the following compounds: a. Fe 2 (SO 3 ) 3 c. Na 3 PO 4 b. RbI d. CuCl 2 e. Ti 3 P What are isomers? Draw the three isomers for C 3 H 9 N. 26. What is the HONC1234 and Octet rule? Which molecules obey the Octet rule? Draw the Lewis Dot structures for the following molecules. a. CF 3 b. PCl 2 c. OCl 2 d. SiI What does VSEPR mean? 28. What is the difference between lone pairs and bonded electron pairs? 29. Fill in table. Molecule Lewis Dot Structure Structural Formula Lone pairs on central atom Bonded pairs on central atom Shape of Molecule CO 2 SeCl 2 NH 3 CH 4 CH 2 O 30. Write the molecular formula, structural formula, Lewis Dot structure, and ball-and-stick formula for water, methane, and carbon dioxide. 31. What are the different characteristics between a polar vs. nonpolar molecules? (ex: dissolve in water, attraction to a negatively charged wand, on wax paper). 32. How do you use the electronegativity values chart to determine nonpolar covalent, polar covalent, and ionic bonds? What is happening to the electrons in these different bonds? 33. Determine type of bond between these atoms: Cl-Cl, As-H, Ca-O, P-I, K-Cl, and F-Si

4 34. Are the following molecules polar or nonpolar molecules? Explain a. SiF 4 b. PI 3 c. SCl 2 d. SiS What are intermolecular forces? 36. What are three types of intermolecular/ van der Waals forces? Which is the strongest? Weakest? 37. Explain how electronegativity can help determine the bond type in a molecule. 38. Explain how you can tell if an entire molecule will be polar or nonpolar. 39. Fill in the following chart: Molecule Lewis Dot Structure (use Octet Rule) Structural Formula (use HONC 1234) Shape 1. sketch ball & stick model 2. Write name of shape 3. Show direction of all dipoles (e- pull) according to electronegativity difference Is the entire molecule Polar or Nonpolar? Can we smell it? Will it dissolve in water? Type of IMF? (Intermolecular Force) CBr 4 H 2 Se CH 2 S AsH 3 HSiF 3 Unit 4: Biochemistry 40. What are the different functional groups, the smells associated for each, and their common names endings? 41. What are chemical reactions? Where do they take place in the molecule? What is happening in the molecules when chemical reactions occur? 42. What are reactants? Products? 43. Explain the collision theory.

5 44. What is activation energy? 45. What is a catalyst? What does it do? 46. What are carbohydrates and how are they used by living organisms? 47. Complete the following chart: Carbohydrate Monosaccharides Disaccharides Polysaccharides Examples 48. What are lipids and how are they used by living organisms? 49. What are proteins and how are they used by living organisms? 50. What is the structure of amino acids? Which functional groups are present? What does the R stand for? 51. What type of bond holds proteins together? 52. What are the 2 types of nucleic acids and what are their functions? 53. What type of bond is found in alkanes? Alkenes? Alkynes?