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Example problems from previous quizzes and assignments. Matter Review Classify each of the following as a physical or a chemical property of matter. _____1. _____2. _____3. _____4. _____5. _____6. _____7. _____8. Iron and oxygen form rust Oil and water do not mix Aluminum has a silvery color Silver tarnishes Water boils at 1000 C Gold has a density of 19 g/ml Sodium ignites when dropped in water Magnesium burns brightly when ignited 9. Create a graphic organizer using the following words: Matter, Mixtures, elements, sugar, water, oxygen, pure substance, solution, homogeneous, gold, heterogeneous, compounds The Atom 1. Discuss Rutherford’s experiment. What was he testing for? What was his hypothesis? What did he discover? How did this change the theory of the atom? 2. Give the number of protons, neutrons and electrons in the following elements: a. C-12 b. Cu-63 c. Ni-58 d. U-235 3. Give the noble gas configuration of the following elements. Try not to use the atomic number while doing so. (HINT: use the s, p, d, and f blocks we discussed). a. Cl b. Co c. Al d. I 4. What element has the following electron configuration? a. [Kr] 5s2 4d5 b. [Ar] 4s2 3d10 4p4 c. [Xe] 6s2 4f14 5d4 5. Fill the following table out about quantum levels and sublevels Quantum level Sub levels Orbitals in sub Total electrons present level in sub level 1 2 3 4 Periodic Table 1. On the periodic table below, label the following items (use the letter given to label): a. two elements in the same group (A) b. two elements in the same period (B) c. a transition metal (C) d. A lanthanide (D) e. An alkali Earth Metal (E) f. A non-metal (F) g. A metalloid (G) 2. On the periodic table above, draw in the following trends, showing how the particular trend increases, both across and up/down (ex – if atomic radius increases across, draw an arrow from left to right and label it increasing, atomic radius). Explain WHY the trends are the way they are. a. Atomic radius, ionic radius, ionization energy, electronegativity 3. What is the difference between ionization energy and electronegativity? Ionic and Covalent Compounds 1. How does a cation form? An anion? 2. Using the following list of ions, create 10 ionic compounds AND name them. Au +1 Fe+2 Na+1 Ca+2 Al+3 NH4+1 BrO-1 Cl-1 OH-1 NO2-1 SO4-2 N-3 O-2 ClO4-1 BO3-3 C2H3O2-1 3. Describe the difference between ionic and covalent compounds. 4. Name the following covalent compounds: a. NO ________________________________________ b. NF3 ________________________________________ c. P2F4 _______________________________________ d. SeO3 _______________________________________ 4. Draw the following molecular structures for the covalent compounds. 5. a. SeBr2 b. PO3-3 c. CO3-2 Chemical Reactions Write out the correct, balanced chemical equation given the following word equations. Also, determine the type of reaction that is occurring. 1. Sodium sulfide and silver nitrate react to form sodium nitrate and silver sulfide. 2. Carbon monoxide and oxygen react to form carbon dioxide. 3. Potassium chlorate decomposes into potassium chloride and oxygen. 4. Iron (III) chloride reacts with sodium hydroxide producing solid iron (III) hydroxide and sodium chloride. 5. How can you determine whether a single replacement reaction will occur? Moles and Molar Conversions Convert the following numbers to either moles, grams or particles in the following elements or compounds. 1. X mol in 5.5 x 1026 atoms of Bi 2. X grams in 4.67 mol Li 3. X mol in 25 g Zn 4. X atoms 3.54 mol Hg 5. X mol of CO2 in 3.2 x 1020 molecules 6. X g of CaCO3 in 1.9 mol 7. X particles in 44.5 g H2O 8. X g KMnO4 in 2.54 X 1024 formula units Stoichiometry 1. One of the main ingredients of pearls is calcium carbonate. If pearls are put in an acidic solution, they dissolve. CaCO3 + HCl CaCl2 + H2O + CO2 How many moles of CaCO3 can be dissolved in .0250 mol HCl? 2. The fuel methanol (CH3OH) is made by the reaction of carbon monoxide and hydrogen. How many grams of hydrogen are needed to produce 45.0 g of methanol? 3. Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen and methane. NH3 + O2 + CH4 HCN + H2O If 5.0 X 103 kg of CH4 are used, what mass of HCN and H2O would be produced? **Density and isotope problems – very little on the final, look over previous tests and quizzes for example problems**