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FINAL REVIEW PACKET Nomenclature 1. Polyatomics 2. An ionic compound is made up of a __cation_______ and a _anion_______. The first element is ALWAYS the _cation______, which forms a _ion______ with a _positive______ charge. The second element is the __anion______, which forms an _ion_________ with a __negative________ charge. a. Give three examples (name and formula) MgO magnesium oxice FeCl3 iron (III) chloride AlBr3 aluminum bromide 3. A covalent compound is made up of ___neutral atoms usually two nonmetals__________________. a. Give three examples (name and formula) PO2 phosphorous dioxide N2Cl6 dinitrogen hexachloride CO2 carbon monoxide b. To name covalent molecular compound, use __prefixes to show _subscripts_______________________. 4. Differentiate between a binary and ternary compound a. Binary, two elements, ternary three of more elements b. Give three examples of ternary compounds (name and formula) KNO3 potassium nitrate NH4OH ammonium hydroxide MgSO3 magnesium sulfite 5. When is the Stock Naming system used. a. Why? To show the oxidation number a transition element used. b. Give three examples (name and formula) FeCl2 iron (II) chloride FeCl3 iron (III) chloride FeO iron(II) oxide 6. Name the following a. CaCr2O7 calcuim dichromate b. Pb(SO3)2 lead (IV) sulfite c. N3O6 trinitrogen hexoxide d. Na3N sodium nitride e. H3PO4 phosphoric acid f. HF hydrofluoric acid 7. Give formula for a. Hydroselenic acid H2Se b. Hydrocyanic acid HCN c. Perchloric acid HClO5 d. Sulfurous acid H2SO3 e. Hypomanganic acid H3MnO4 f. Barium chloride BaCl2 g. Vanadium (V) sulfide V2S5 h. Tetraphosphorous decaoxide P4O10 i. Nitrogen heptasulfide NS7 j. Aluminum phosphate AlPO4 k. Ammonia NH3 l. Hydrogen peroxide H2O2 m. Methane CH4 Chemical reactions 8. List five indicators of a chemical change a. Bubbling b. Temperature change c. Precipitate d. Color change e. Mass change 9. What is the only way to determine that a chemical reaction has taken place? Can not be undone 10. Give the general format for a chemical reaction. Reactants products 11. Identify the following symbol. a. yield b. Δ change in heat c. Mn On catalyst d. + and e. (s) solid f. (g) gas g. (aq) aqueous, in solution, dissolved in water h. (l) liquid 2 12. A) Predict products and B) Write a complete balanced chemical equation for the following equations. C) Indicate whether reaction will or will not occur. D) Indicate WHY. E) Indicate type of reaction. a. Ammonium hydroxide rapidly decomposes in the presence heat to form ammonia and water heat NH4OH NH3 + H2O decomposition, will occur due to increased entropy b. Carbon dioxide and water are formed as a result of the combustion of methane gas. CH4(g) + 2O2 CO2 + 2 H2O combustion, will occur c. A barium sulfate precipitate and aqueous sodium chloride are formed from the metathesis reaction between barium chloride and sodium sulfate solutions. BaCl2(aq) + Na2SO4(aq) BaSO4(s) + NaCl(aq) double replacement will occur forms a precipitate d. Zinc and dissolved copper II chloride react to form copper metal and zinc chloride. Zn + CuCl2(aq) ZnCl2 + Cu will occur, sincle replacement, zinc is more active than copper e. The dissolution of sulfur trioxide in water is a major source of acid rain through the formation of sulfuric acid. H2O + SO3 f. H2SO4 will occur synthesis reaction Propane burns in air C3H8 + 5O2 3CO2 + 4H2O combustion will occur 2 Final Review Packet_Honors/Academy Chemistry g. Magnesium reacts with nitrogen. 3Mg + N2 Mg3N2 synthesis will occur h. Calcium carbonate is heated heat CaCO3(s) CaO + O2(g) decomposition i. Zn metal is placed in a solution of Copper sulfate Zn(s) + CuSO4 ZnSO4 + Cu(s) will occur, single replacement, zinc is more reactive than copper j. Barium hydroxide and Lithium sulfate are mixed Ba(OH)2(aq) + Li2SO4(aq) BaSO4(s) + 2LiOH (aq) double replacement, will occur precipitate formed k. Sodium hydroxide and Phosphoric acid are mixed. 3NaOH (aq) + H3PO4(aq) Na3PO4(aq) + 3H2O(l) double replacement, neutralization, will not occur, strong base, weak acid l. Calcium oxide in water. CaO + H2O Ca(OH)2 synthesis, will occur m. Sodium in water 2Na(s) + 2H2O(l) 2NaOH + H2(g) single replacement, sodium replaces hydrogen in water will occur ) 13. What is the activity series? Why is it useful? Identifies what elements will replace another in a compound, predicts if a reaction will occur a. Know how to use it to predict whether a reaction will occur. 14. Determine solubility of each of the following. a. Magnesium sulfate soluble b. Sodium carbonate soluble c. Calcium hydroxide soluble d. Calcium sulfate insoluble e. Silver nitrate soluble f. Silver iodide insoluble g. Lead (II) chloride insoluble h. Lead (IV) bromide insoluble i. Aluminum oxide insoluble j. 15. Know difference in solubility rules for reactants vs. products. 3 Final Review Packet_Honors/Academy Chemistry Mole Quantities 16. Define mole 6.02x1024 particles 17. Convert the following a. 4.58 mol to particles of Al = 2.76x1024 b. 4.58 mol to grams of Al = 124g c. 901.49 g to particles of Carbon dioxide = 1.23x 1025 d. 901.49 g to L of carbon dioxide = 458.9 18. Define molar mass. The mass of a mole of a substance, equal to the atomic mass in grams 19. Give molar mass of a. Vanadium = 50.94g b. Vanadium IV oxide =82.94 c. Glucose =180 20. Define percent composition the percent of the total mass that each component contributes. 21. Give percent composition of a. Aluminum carbonate = 23% Al 15% C 61% b. Potassium phosphate = 55% K 14.6% P 30% O 22. Distinguish between empirical and molecular formula empirical is the simplest ratio of atoms in a compound, the molecular is the actual number of atoms in a compound. 23. Solve the following a. What is the percent composition of Nickel (II) oxide , if a sample with a mass of 41.9 g contains 33.1 g Ni and 8.8 g O? = 79% Ni 21% O b. Calculate the molecular formulas of the compounds having the following empirical formulas and molar masses: i. C H , 58 g/mol; =C4H10 ii. CH, 78 g/mol; and =C6H6 iii. HgCl, 236.1 g/mol. = HgCl c. The percentage composition of acetic acid is found to be 39.9% C, 6.7% H, and 53.4% O. Determine the empirical formula of acetic acid. If the molar mass is 60 g/mol, determine the molecular formula for acetic acid. Empirical= CH2O molecular C2H6O2 24. STOICHIOMETRY (basic, Limiting Reactant, Excess Reactant, %Yield) a. How many moles of oxygen are consumed when 96.7 moles of hydrogen sulfide gas are burned, producing sulfur dioxide and water vapor in the process? =14.4 moles b. If 3.70 x 1023 molecules of oxygen react with excess benzene (C6H6), how many grams of water can be produced? =27g H2O c. 25.0 g Calcium reacts with 40.0 g Oxygen. Determine mass of product formed. = 35.0g CaO (find limiting reactant) d. 500.0 L of Nitrogen gas and 600.0 L of Hydrogen gas are available and react to form Ammonia. Determine mass of Ammonia that can be formed. How many Liters of Ammonia is produced? What is the identity and amount of excess reactant left over. =303.5g NH3 357g of N2 is left over 4 Final Review Packet_Honors/Academy Chemistry e. 30.0 grams of acetic acid reacts with excess methanol (CH3OH) to produce 30.0 grams of methyl acetate (CH3COOCH3) and water. Determine the percent yield of the reaction. 81% yield f. A chemist reacts 2.00 grams of vanadium (II) oxide with 5.75 grams of iron (III )oxide to produce vanadium (V) oxide and iron (II) oxide. The reaction goes to 67.0% completion. How many grams of the iron (II) oxide are produced? (balance oxidation reduction) Limiting reactant iron (III) oxide Theoretical yield 5.175g 67% of that is 3.47g produced. 5 Final Review Packet_Honors/Academy Chemistry