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Name: ___________________________ Chemistry Fall Semester Review Sheet Lab Safety & Equipment: 1. What should you do if you get acid on your hands? Rinse with lots of water 2. How should you smell a chemical if you are instructed to do so? waft 3. When are goggles required? When using chemicals, heat or glassware 4. What should you do with broken glass? Dispose of broken glass in the broken glass container Density, Kinetic Theory & States of Matter: 5. What are the three main states of matter? Solids, liquids & gases 6. Fill out the table below for the three states of matter State Compressibility Shape Volume Kinetic energy (high/low) (definite/indefinite) (definite/indefinite) (high/low) Solid LOW DEFINITE DEFINITE LOW Liquid LOW INDEFINITE DEFINITE MEDIUM Gas HIGH INDEFINITE INDEFINITE HIGH 7. Which phase is the most structured? The least? Solids are the most structured, Gases are the least 8. Label the following on the phase diagram on the right. Gas Liquid Solid Triple point Critical point Freezing Evaporation/boiling Sublimation Condensation Melting Deposition 9. What is the density of carbon dioxide gas if 0.196 g occupies a volume of 100 mL? D=m V D = 0.196 g 100 mL D = 0.00196 g/mL Directions: Use the data shown below to answer the following questions 10 and 11. Substance Density (g/mL) water 1.00 g/mL ethanol 0.78 g/mL benzene 0.88 g/mL 10. If you poured all 3 liquids together and they did not mix, which substance would be the top layer? Ethanol would be on the top layer 11. Identify the substance that has a mass of 8.1 grams and occupied a volume of 10.3 liters mL. D = m/V D = 8.1 / 10.3 D = 0.786 g/mL = ETHAHNOL Classification of Matter: 12. Identify each of the following as either an: element, compound, homogeneous mixture or heterogeneous mixture A. Pizza _____Heterogeneous_____ C. Salt (NaCl) _______Compound____ B. Vanilla Ice Cream _____Homogeneous_____ D. Carbon ______Element______ 13. Identify each of the following as either a: chemical or physical change A. Burning _______Chemical____ C. Boiling Water ______Physical______ B. Cutting paper _______Physical______ D. Iron Rusting ______Chemical_____ 14. A __compound__ can only be separated by chemical means. 15. List the 4 indicators of a chemical change: Bubbles, heat, light & precipitate 16. Define the Law of Conservation of Mass. Mass can’t be created or destroyed 17. Identify each of the following as either an: intensive or extensive property A. B. C. D. Mass Density Volume Texture _____extensive_____ _____intensive_____ _____extensive_____ _____intensive_____ Atomic Theory: 18. Complete the following chart. PARTICLE CHARGE MASS LOCATION proton Positive 1 amu nucleus neutron Neutral 1 amu nucleus electron Negative 0 amu Electron cloud 19. Define the law of multiple proportions. Elements form compounds in simple whole number ratios 20. What do isotopes of the same element have in common and what is different? Isotopes have the same number of protons, electrons and atomic number Isotopes have a different mass number and number of neutrons 21. Explain how Rutherford’s gold foil experiment worked and what it proved. Rutherford shot particles through gold foil. Most went through, but some bounced back. He concluded that atoms are mostly empty space and the particles bounced off the dense center called the nucleus. 22. What subatomic particle determines the identity of an atom? Protons 23. How do you find the following: A. Number of protons in an atom = __same as the atomic number__ B. Number of neutrons in an atom = __mass # - atomic #__ C. Number of electrons in an atom = __same as the atomic number__ Symbol Atomic Number Mass Number Number of Protons Number of Electrons Number of Neutrons Ag 47 109 47 47 62 Mg 12 24 12 12 12 Ga 31 72 31 31 41 The Periodic Table & Trends: 24. The horizontal rows found on the periodic table are called __periods__, while the vertical columns are called ___groups__ or ___families___. 25. The most reactive elements on the periodic table are in group __1A – Alkali Metals__. 26. Electronegativity ____decreases_____ (increases/decreases) going down groups and ______increases_____ (increases/decreases) going across periods from left to right. 27. Ionization Energy ______decreases_____ (increases/decreases) going down groups and ______increases_______ (increases/decreases) going across periods from left to right. 28. Atomic radius ________increases______ (increases/decreases) going down groups and _______decreases_______ (increases/decreases) going across periods from left to right. 29. The number of valence electrons ________increases______ as you go across a period, but will ______stay the same____ as you go down a group. 30. The most electronegative element is ________Fluorine_____________. 31. The element with the largest atomic radius is _______Francium______. 32. Which of the following has a bigger atomic radius: Cesium or Calcium? (Circle one.) 33. Which of the following has a higher ionization energy: Potassium or Sulfur? (Circle one.) 34. Classify the following as either an: Alkali Metal, Alkaline Earth Metal, Halogen or Noble Gas A. Strontium __Alkaline Earth Metal____ C. B. Bromine ___Halogen___ D. Krypton Potassium __Alkali Metal___ __Noble Gas____ Electron Configurations & EMR Calculations: 36. Write the long-hand electron configurations AND noble gas notations for the following atoms: A. Calcium 1s22s22p63s23p64s2 [Ar]4s2 B. Iron 1s22s22p63s23p64s23d6 [Ar]4s23d6 37. What do the superscripts add up to in an electron configuration? ____the atomic number___ 38. What is the energy of a photon whose frequency is 6.9 x 1014 Hz? E=hxV E = 6.63 x 10-34 x 6.9 x 1014 E = 4.57 x 10-19 J E=hxv h = 6.63x10-34 J·s 39. What is the packet of light called that is released when an electron relaxes to the ground state? photon Bonding & Ionic Compounds: 40. Name the following compounds: A. BaCO3 _____barium carbonate____ B. NH4OH _____ammonium hydroxide_____ C. NiCl2 _____nickel (II) chloride_____ D. MnCl3 _____manganese (III) chloride____ 41. Write the formula for each of the following compounds: A. Aluminum phosphate ______AlPO4____ B. Copper (III) sulfide _____Cu2S3_____ C. Magnesium chloride _____MgCl2____ D. Potassium nitrate ______KNO3____ 42. Identify each of the following as either an: ionic or covalent bond A. electrons are shared __________covalent_______ B. electrons are transferred _________ionic_________ C. MgCl2 ________ionic_______ D. CO2 _________covalent__________ 43. Why are metals malleable and ductile? _________metals have a “sea of electrons”______ Covalent Compounds & VSEPR Theory: 44. Write the name for the following compounds: A. SF8 ____sulfur octafluoride___ B. SiH4 ____silicon tetrahydride____ C. F2O ___difluorine monoxide____ 45. Write the formula for the following: A. Diphosphorus pentoxide _____P2O5___ B. Dinitrogen tetrahydride ____N2H4____ C. Carbon monoxide ____CO_____ 46. Show the covalent bonding diagram and identify the shape and polarity for the following: CO2 CCl4 CH2O Shape: ____Linear____ Shape: ____Tetrahedral____ Shape: ___Trigonal Planar___ Polarity: ____Nonpolar____ Polarity: ____Nonpolar_ Polarity: ___Polar___ PH3 HCN H2S Shape: __Trigonal Pyramidal_ Shape: ___Linear____ Shape: ____Bent____ Polarity: ____Polar___ Polarity: _____Polar____ Polarity: ____Polar____ Dimensional Analysis & Significant Figures 47. Determine the number of significant figures in each of the following numbers. A. 8603 __4__ D. 52000 __2_ B. 11.00 ___4__ E. 40.5 ___3_ C. 0.701 __3__ F. 0.00390 ___3__ 48. Determine the answers to the following problems. Round your answer so that it has the correct number of decimal places or significant figures. A. 678 / 3.217 = 211 B. 16 + 5.18 = 21 C. 48.968 – 10.5 = 38.5 D. 0.0030 x 4560 = 14 49. Write the following numbers in scientific notation. A. 456,000 __4.56 x 105_ B. 0.000071 __7.1 x 10-5__ C. 500,000,000 __5 x 10 8__ 50. How many minutes are in 6.00 days? 6.00 days x 24 hours x 60 min = 8640 min 1 day 1 hour 51. How many inches are in 17.65 miles? (1 mile = 5280 ft) (1 ft = 12 inches) 17.65 miles x 5280 ft x 12 inches = 1.12 x 106 inches or 1,120,000 inches 1 mile 1 foot Mole Calculations 52. Calculate the molar mass for each of the following compounds. A) KCl ____74.551 g/mol___ D) H2O _____18.015 g/mol___ B) Mg3(PO4)2 ____262.855 g/mol__ E) AlS _____59.048 g/mol___ C) H2SO4 ____98.078 g/mol____ F) Ca(NO3)2 _____164.088 g/mol__ 53. How many moles of CO2 are in 56.3 Liters of CO2? 56.3 L x 1 mole = 2.51 moles 22.4 L 54. How many Liters are in 7.32 x 1024 molecules of O2? 7.32 x 1024 molecules x 1 mole x 22.4 L 6.02 x 1023 molecules 1 mole = 272 Liters 55. Convert the following: 2.8 g Na = __________________ atoms Na 2.8 g Na x 1 mole x 6.02 x 1023 atoms = 7.33 x 1022 atoms 22.990 g 1 mole 56. Which of the following contains the smallest number of moles (circle): 1 gram of carbon, 1 gram of copper or 1 gram of barium Percent Composition: 57. Define percent composition. The relative amount of an element in a compound 58. Calculate the percent composition of each element in CO2. %C = 12.011 x 100 = 27.3 %C %O = 31.998 x 100 = 72.7 %O 44.009 44.009 59. Calculate the percent by mass of hydrogen in water. % H = 2.016 x 100 = 11.2 %H 18.015 60. Calculate the percent by mass of oxygen in water. %O = 15.999 x 100 = 88.8 %O 18.015