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Download Key To T2 Review For Final Study Guide File - District 196 e
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Key To T2 Final Review 2015 1. Determine the number of significant figures in the following numbers: a. .00356 g c. .5000 L b. 1.00 m d. 50 s 2. Write each measurement in scientific notation or in standard form. Record each measurement to 3 significant figures. a. 39980 kg 4.00 x 104 kg -3 b. 7.45583 x 10 mol .00746 mol 3. Using dimensional analysis, convert the following: a. 6.00 g to kg 6.00 x 10-3 kg 3 b. 1.86 x 10 mg to g 1.86 x 106 g c. 46 cm3 to quarts .049 qt 4. Define the law of conservation of mass and explain how this law is implemented when balancing equations. Mass cannot be created or destroyed in ordinary chemical reactions. This law is applied to balancing when coefficients are placed in front of elements or compounds to make the number of atoms on both sides of the equation equal. 5. Name the following compounds: a. P4O8 tetraphosphorous octaoxide b. NO nitrogen monoxide c. NH3 nitrogen trihydride (ammonia) d. (NH4)2S e. Pt(SO4)2 f. H3PO4 ammonium sulfide platinum (IV) sulfate phosphoric acid 6. Write the formulas for the following compounds: a. strontium phosphide Sr3P2 d. carbon tetrahydride CH4 b. zinc hydroxide Zn(OH)2 e. phosphorous monoxide PO c. hydrocyanic acid HCN f. iron (III) oxide Fe2O3 7. What are the 6 reaction types and their patterns? Provide an example of each type of reaction. Synthesis – A + B AB 2H2 + O2 2H2O Decomposition – AB A + B Single Replacement Cationic - A + BC B + AC Cu + 2AgNO3 2Ag + Cu(NO3)2 Single Replacement Anionic – A + BC C + BA F2 + KBr Br2 + KF Double Replacement - AB + CD AD + CB Na2SO4 + BaCl2 2NaCl + BaSO4 2NaCl 2Na + Cl2 Combustion – Hydrocarbon + Oxygen carbon dioxide + water CH4 + 2O2 CO2 + 2H2O 8. What is a limiting reactant? Why is this reactant so important? The limiting reactant is the reactant that runs out first in a chemical reaction, therefore determining the amount of product produced. 9. What is an excess reactant? The reactant that there is more than enough of to complete the limiting reactant. Some of this reactant will be left over when the reaction stops. Usually, this reactant is cheaper and easiest to isolate out of the possible reactants. 10. What does “theoretical” mean? Where/how are these results obtained? Theoretical results show what the value of a calculation should be under perfect conditions. These results can be obtained from a published source, teacher, or through stoichiometry. 11. What does “experimental” mean? Where/how are these results obtained? Experimental results show the value of a calculation that was obtained through lab results. Hopefully, the theoretical and experimental results should as close to the same as possible. 12. Using dimensional analysis, convert the following: a. 2.00 moles of oxygen gas to grams 64.0 g O2 b. 6.75 x 1022 molecules of oxygen gas to grams 3.59 g O2 c. 4.66 g iodine crystals to molecules 1.11 x 1022 molecules I2 d. 7.6 x 1023 formula units of salt to moles 1.3 mol NaCl 13. What is the difference between a coefficient and a subscript? Provide an example illustrating each. A coefficient is placed in front of elements and compounds to make the number of atoms on each side of the equation equal. 2H2O Subscripts are used in chemical equations to show the number of atoms bonded in a molecule or formula unit. 2H2O 14. What is the difference between a reactant and a product? Provide an example illustrating each. Reactants are found to the left of the arrow in a balanced chemical equation 2H2 + O2 2H2O Products are found to the right of the arrow in a balanced chemical equation. 2H2 + O2 2H2O 15. What is a catalyst? Provide 3 examples that we frequently use in the lab. A catalyst is a chemical or a process used to speed up a reaction. Examples include, heating, agitation/stirring, adding a chemical that will not become part of the products. 16. Explain how you know whether or not SR or DR reaction will occur. Provide an example for SR and DR that will occur. Provide an example for SR and DR that will not occur. (Use blue solubility sheet) A SR reaction will occur if the element that is by itself is more reactive (higher up) on the reactivity chart then the like element it is trying to replace in the compound. If not, then no reaction will occur. Ag + NaCl Na + AgCl NO RXN A DR reaction will occur if the partner swap due to mobile ions mingling will result in gas, water, or a precipitate will form. If not, only spectator ions are present and no reaction will occur. NaCl + KBr NaBr + KCl NO RXN 17. What is the % composition of each element in ammonium phosphate? (NH4)3PO4 % N = 28.19% % H = 8.128% % P = 20.77% % O = 42.92% 18. What is a hydrate? Anhydrate? A hydrate is a solid that contains water molecules. An anhydrate is the solid chemical that remains after the water has been removed from the hydrated form of the compound. 19. What is the % composition of water in MgCO3 10H20? % H2O = 68.123% 20. Compare empirical and molecular formulas. Provide an example of each. Empirical formulas show the lowest/simples whole number ratio of atoms in a compound. CH4 Molecular formulas show the actual or true number of atoms in a compound. C2H8 21. 11.0 g of a certain compound contains 2.82 g of magnesium and 8.18 g of chlorine. What is the empirical formula? MgCl2 22. A compound is tested and is found to be composed of 43.7% phosphorus and 56.3% oxygen. It has a molecular mass of 425.82 g/mol. Is the empirical and molecular formula the same? Provide formulas. No, the formulas are not the same. The empirical formula is P2O5. The molecular formula is 3 times as large in mass and atoms, P6O15. 23. A solution of magnesium chloride and silver nitrate are mixed: a. Write a balanced chemical equation with states for the reaction. MgCl2(aq) + 2AgNO3(aq) Mg(NO3)2(aq) + 2AgCl(s) b. What type of reaction is it? Double replacement c. Write a complete balanced equation (circle spectators). Mg+2(aq) + 2Cl-(aq) + 2Ag+(aq) + 2NO3-(aq) Mg+2(aq) + 2NO3-(aq) + 2AgCl(s) d. Write a net ionic equation. 2Cl-(aq) + 2Ag+(aq) 2AgCl(s) 24. What are spectator ions? Spectator ions are ions that watch throughout the entire chemical reaction. They are not involved in forming the precipitate. 25. Why is a net ionic equation so important? This equation is what shows what ions hook up in solution to form the precipitate that drives the chemical reaction. 26. For each set of reactants, identify the type of reaction, predict the product(s) in words and then write a balanced equation. a. Potassium + Oxygen Potassium Iodide 2K + O2 2KI Synthesis b. Fluorine + Lead (IV) Bromine Bromine + Lead (IV) Fluoride 2F2 + PbBr4 2Br2 + PbF4 Single Replacement Anionic c. Aluminum Oxide Aluminum + Oxygen 2Al2O3 4Al + 3O2 Decomposition d. Calcium + Gold (I) Oxalate Gold + Calcium Oxalate Ca + Au2C2O4 2Au + CaC2O4 Single Replacement Cationic e. Calcium Carbonate + Magnesium Phosphate Calcium Phosphate + Magnesium Carbonate 3CaCO3 + Mg3(PO4)2 Ca3(PO4)2 + 3MgCO3 Double Replacement f. Tricarbon Octahydride + oxygen Carbon Dioxide + Water C3H8 + 5O2 3CO2 + 4H2O Combustion 27. What is the difference between and ionic, covalent and metallic bond? Ionic metal + nonmetal (cation and anion) bonded through the transfer of electrons (loss and gain) Covalent 2 nonmetals bonded through sharing of electrons Metallic 2 metal cations surrounded by a sea of electrons 28. Why do things bond? To look like a noble gas and obtain a full valence shell 29. Draw the Lewis Dot Structure for each of the following ionic substances: a. LiCl b. MgBr2 c. Ca3P2 see additional key on Moodle 30. Draw the Lewis Dot Structure for each of the following covalent substances: a. Br2 b. O2 c. N2 d. CO2 see additional key on Moodle