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Name _________________________________________________ Period 1 2 3 4 5 6 7 8 Quarter 3: Post Test Review A. Scientific Foundations 1. Figure out protons, electrons, neutrons and mass number of the following atoms: 18 209 +1 -2 b. 25 a. c. 8 11 82 O Na Pb 2. How many significant figures are in the following? a. 8 b. 800 c. 0.08 d. 8008 e. 0.080 f. 800. g. 800.0 3. Convert the following: a. 5.72 mg to Kg b. 275.6mL to L c. 4.50 cm to km 4. _____________ or ______________ = horizontal on the periodic table 5. ___________ , ______________, or ________________ = vertical on periodic table 6. What is the trend in periodic size as you move across the periodic table? ________ down? _______ 7. What is the trend in electronegativity as you move across the periodic table? _____ down? _______ 8. Classify the following as physical or chemical properties/changes a. reacts with water b. burns in the presence of oxygen c. density d. evaporation e. melting point f. blue in color B. Chemical Formulas and Equations Write the following chemical formulas: 9. Calcium chloride 10. Chromium (II) sulfate 12. Disulfur tetraoxide 13. Magnesium iodide 11. Zinc phosphate 14. Hydrobromic acid Write the following names of the chemical formulas: 15. BeF2 16. N3Br 18. NaClO3 19. NaCl 17. H3PO3 20. Cu(NO3)2 Balance the following equations: 21 ___Al + ___Pb(NO3)2 ___Pb + ____Al(NO3)3 22. ___Mg(OH)2 + ___HCl ___H2O + ___MgCl2 23. ___Al2(SO4)3 ____Al2O3 + _____SO3 Chemical Reactions Types: 24. What are the products of an acid/base reaction ________________ and _______________ 25. What are the reactants of a combustion reaction _______________ and _______________ 26. What are the products of a combustion reaction ________________ and _______________ 27. NaBr + Ca(OH)2 CaBr2 + NaOH Type of reaction: ____________ 28. C5H9O + O2 CO2 + H2O Type of reaction: ____________ 29. Pb + H3PO4 H2 + Pb3(PO4)2 Type of reaction: ____________ 30. NH4OH NH3 + H2O Type of reaction: ____________ 31. HBr + Al(OH)3 H2O + AlBr3 Type of reaction:_____________ C. Quantifying Matter 32. What is the molar mass of H2SO4? _________ b. CoCl2? _________ c. Ni3(PO4)2?_____ 33. Determine the mass in grams of 40.0 moles of sodium 34. Calculate the moles in 510.0 g of aluminum sulfide 35. Calculate the number of moles in 1.00 grams of barium hydroxide 36. The octane present in gasoline burns according to the equation: 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O a. What is the mol to mol ratio of oxygen to water? _____: _____ 37. When completing the above reaction (in number 28), the reaction runs out of the propane reactant before it runs out of the oxygen reactant. Therefore, propane is called the ___________ ____________ D. Gas Laws 38. What is the kinetic molecular theory? 39. What is Boyle’s law? _______________________________ b. What is the relationship between pressure and volume? 40. What is Charles’s law? _______________________________ b. What is the relationship between volume and temperature? 41. What is the ideal gas law? ______________________________ 42. When using the ideal gas law what are the units for the following? Temperature = Pressure = Volume = n= r= 43. What is STP? 44. ________ mmHg = __________torr = _________Pascals = __________kilopascals Convert 2983.4 mmHg into torr. ___________________ convert in Pascals ________________ E. Bonding and Electron Configurations 45. Besides metallic, what are the other two types of bonding. _____________ and __________ b. define the relationship between electrons in these two types of bonds c. a _______ bond is between a metal and a non-metal d. a ________ bond is between two non-metals 46. What are the main differences between the Bohr model of an atom, a Lewis dot structure and the modern model of the atom? 47. Draw the Lewis dot diagram for the following compounds: a. CCl4 b. O3 c. NF3 d. H2O e. Br2 f. SO2 g. COF2 48. Fill in the following information Orbital name Shape Max number of electrons sphere p 10 f You are not required to know this 49. Write the full AND noble gas electron configuration for the following a. sodium b. neon c. bromine d. calcium e. oxygen 50. How many more electrons do the following need to satisfy the octet rule? a. [Ne] 3s23p3 b. 1s2,2s2, 2p4