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Name____________________________________________ Date________________ Hour______ Chemistry Semester 1 Review Unit 1: Introduction and Review 1. What is the proper procedure if you get a chemical in your eye? 2. Draw a picture of and describe how to use the following pieces of laboratory equipment: a. Beaker d. crucible tongs b. Graduated cylinder e. beaker tongs c. Evaporating dish f. test tube holders 3. Convert the following units: 10.64 mL __________L 3200 m __________mm 14.32 L __________kL 418 µg __________g 0.000435 km __________mm 13.2 kg 0.543 mm 53 mL 0.312 cg 10.555 L __________g __________km __________cL __________kg __________µL 4. How many significant figures are in each of the following measurements? a. 4.09 cm____ b. 10.450 L____ c. 0.00028 g____ d. 10 m____ 5. What are the SI units for the following: time, temperature, length, volume, mass? 6. Define precision and accuracy. 7. Which measurement is most precise? Why? 12.3 g or 12.336 g 8. In a lab a student finds the density of copper to be 9.32g/cm3. If the actual density of copper is 8.96 g/cm3, what is the percent error? 9. Differentiate between physical and chemical properties. 10. List five physical properties of water. 11. List two chemical properties of gasoline. 12. Differentiate between physical and chemical changes. 13. List five ways you could physically change a piece of paper. 14. What are the five indicators of chemical change? 15. List three indicators of chemical changes when a steak is cooking. 16. State the Law Conservation of Mass (Matter). Unit 2: Periodic Table, Atomic Structure, and Nuclear Chemistry 17. Label this blank periodic table using the terms underneath it. group and family numbers period numbers representative elements transition elements inner transition elements metals nonmetals s-block d-block 18. Define the following terms: atomic number mass number isotope ion metalloids alkali metals alkaline earth metals halogens noble gases lanthanide series actinide series p-block f-block 19. Complete the following table: Shorthand Atom/Ion Notation Name Atomic # Mass # # p+ # no # e- 8 8 82 10 56 2H Carbon Calcium ion Sulfide 20 32 20. Silver has two isotopes: Ag-107 and Ag-108. Looking at the atomic mass of silver, which isotope is more abundant? How do you know this? 21. Lead has four isoptopes. The percent abundances of the isotopes are: 1.37% 204Pb, 26.26% 206Pb, 20.82% 207Pb, and 51.55% 208Pb. What is the average atomic mass of lead? 22. Nitrogen-13 emits beta radiation and decays to Carbon-13 with a half-life of 10 min. Assuming a starting mass of 2.00 grams of Nitrogen-13, how many grams will be present at the end of three half-lives? 23. Write an equation for the alpha decay of Pa-231. 24. Write an equation for the beta decay of H-3. 25. Write an equation for the beta capture of Hf-180. 26. Why is mass not conserved in a nuclear reaction, yet it is in a chemical reaction? Unit 3 – Electronic Structure and Periodicity 27. Define the following: atomic orbital energy level sublevel quantum ionization energy atomic radius electronegativity 28. List all the types of electromagnetic radiation in increasing WAVELENGTH. 29. List the colors of visible light in decreasing ENERGY. 30. Draw the 1s, 2s, 2p, 3s, and 3p orbitals on the same set of axes. 31. What is the maximum number of electrons allowed in each orbital type (s, p, d, f)? 32. What is the maximum number of electrons allowed in each energy level (1-4)? 33. Describe all of the things that happens to an electron in a copper atom when it absorbs a quantum of energy. 34. Write electron configurations (no noble gas configurations) for the following: a. Au b. Ca2+ 35. Write noble gas configurations for the following: a. W b. Te236. What types of elements often have exceptional (i.e. they do not follow the rules for filling atomic orbitals) configurations? 37. Ca2+ has the same electron configuration of which noble gas? 38. Place the elements P, Sc, Cl, Sr, Ba, and F in order of: a. Increasing size b. Increasing ionization energy c. Decreasing electronegativity 39. Ca2+ has the same electron configuration as which noble gas? Unit 4 - Bonding 40. What are valence electrons? 41. How many valence electrons for S? For Ca? For S2-? For Ca2+? 42. How many electrons does nitrogen gain in order to achieve a noble gas electron configuration? 43. How do you know how many valence electrons are in any representative element? 44. Show the ionic bonding between calcium and iodine. 45. How many total electrons are transferred from calcium to iodine when forming the compound above? 46. Which of the following pairs of elements is most likely to form an ionic compound? a) magnesium and fluorine, b) sodium and aluminum, c) bromine and nitrogen, and d) chlorine and lithium 47. What is the octet rule? 48. Draw the Lewis dot structures for the following: CH4, PF3, C2H2, O3, I3-,NO349. Write the shape of each molecule in the previous question next to its Lewis dot structure. 50. Why do atoms share electrons in covalent bonds? 51. How many lone pairs of electrons are there in the NH3 molecule? Unit 5: Chemical Names and Formulas (Nomenclature) 52. List five properties of ionic compounds. 53. What are the chemical characteristics of covalent compounds? 54. Fill in the following table. Ionic, Molecular, Acid, or Base? Name Formula dinitrogen hexabromide ammonium carbonate potassium phosphide mercury (II) acetate sulfuric acid copper (II) sulfate iron (III) dichromate calcium hydroxide carbon tetrachloride aluminum sulfide SrO Cl2O AgC2H3O2 NiF2 H2CO3 Ba3(PO4)2 As2S5 Mg(OH)2 HNO3 Dimensional Analysis 55. The tires on a car are to be inflated to a pressure of 2251 g/cm2. Convert this to lbs/in2 (1kg=2.2lbs) (1in=2.54cm). 56. It took 32,409 kilograms of steel to make the Mackinac Bridge. If the price of steel today is $2.17 per pound, how much would it cost to purchase the steel in today’s market? (1kg=2.2lbs)