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Review Study Guide for the Final Atomic Structure and Matter 1. Define an element. The simplest form of matter that has it a unique set of properties, it cannot be broken down into simpler substances by chemical means 2. Define a compound. A substance that contains two or more elements chemically combined in a fixed proportion 3. Define matter. 4. What is the atomic number? 5. What is the atomic mass number of an element? Number of protons plus neutrons 6. Where are electrons located? Outside the nucleus 7. Where are protons located? Inside the nucleus 8. Where are neutrons located? Inside the nucleus 9. What is it called when you have more electrons than protons? anion 10. What is it called when you have more protons than electrons? cation 11. Do all elements have neutrons? No, Hydrogen does not normally have a neutron 12. What are isotopes? Atoms of the same element that have the same atomic number but different masses due to a different number of neutrons Anything that has mass and occupies space The number of protons Periodic Table 13. What is Periodic Law? When elements are arrange in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. 14. Where are metals located at on the periodic table? Left of the stair-step line 15. Where are nonmetals located at on the periodic table? Right of the stair-step line 16. Where are semimetals located at on the periodic table? On the stair-step line 17. What is ionization energy? The amount of energy required to remove and electron from an atom 18. Elements in the same group have the same number of what? 19. What are valance electrons? 20. Where are the Alkali metals located? 21. Where are the Alkaline earth metals located? Valance electrons The outermost electrons used for bonding Column 1A Column 2A 22. Where are the Halogens located? Column 17A also known as the second to last column 23. Where are the Noble gases located? Column 18A also known as the last column Conservation of Mass and Stoichiometry 24. What is a mole? The amount of a substance that contains 6.02 x 1023 representative particle of that substance 25. What element is used to set the mass scale? 26. What is Avogadro’s number? 6.02 x 1023 Carbon-12 Chemical Bonds 27. Are electrons shared or transferred in an ionic bond? Transferred 28. Are electrons shared or transferred in a covalent bond? Shared Draw the Lewis Dot diagram for the following: Br .Br : : a. : 29. He c. Ar He : : b. : : Ar : 30. Combine the following ions a. Na+ CO32- Na2CO3 b. Sr2+ N3- Sr3N2 c. Al3+ Cl- AlCl3 d. Ca2+ OH- Ca(OH)2 e. Mg2+ PO43- Mg3(PO4)2 f. Mg2+ I- MgI2 31. Balance the following reactions: a. 4Al + 3O2 → b. 8Mg(s) + S8 → 8MgS c. 3Ca + N2 → 2Al2O3 Ca3N2 Solutions 32. Define the following terms A. Solution a homogeneous mixture involving two or more pure substances. B. Solute substance dissolved in the solution. C. Solvent the substance in which the solute is dissolved 33. What is the molarity of HCl when 18.00 g of HCl (g) is added to water yielding a total combined volume of 3.50L? 18.00g x 1 mole HCl = 0.4938 moles 36.45g 0.4938 moles 3.50 L 34. 0.141 M To what volume, in liters, must you dilute a solution containing 4 liters of 0.100 M of Ca(OH)2 to obtain a 0.00100 M solution as calcium hydroxide (Ca(OH)2)? (0.100M)(4L) = (0.00100M)(V2) V2 35. = = 400L How many grams of KMnO4 must be added to make 500 mL of 0.25M potassium permanganate solution? 500mL x 1L = 0.500L 1000mL 0.500L x 0.125 moles 0.25 moles L x 158.04g mole = 0.125 moles = 19.755g Reaction Rates and Equilibrium 36. What is a catalyst? the reaction. A catalyst works by lowering the activation energy, this then speeds up 37. Draw a reaction diagram for an endothermic reaction and for an exothermic reaction. Label the products and the reactants. Activation Energy Activation Energy Endothermic Exothermic Reactants Products Products 38. Reactants Predict how the following would change the direction of the given the following exothermic reaction at equilibrium. Briefly support your answer. Will it “shift to the left or shift to the right.” N2 + 3H2 Æ 2 NH3 + heat a) Increase in the concentration of N2. Shift to the right b) The equilibrium mixture is heated. Shift to the left c) Product NH3 is removed as it is produced. 39. Shift to the right Write the equilibrium expression for the following reaction CH4(s) + Cl2(g) Æ CH3Cl(g) + HCl(g) K = [HCl] [Cl2] 40. Write the equilibrium expression for the following reaction. CH4(s) + H2O(g) Æ CO(s) + 3H2(g) K = [H2]3 [H2O] 41. Solve the following [NO]= 2.0M and [N2]= 2.0M P4(s) + 6NO(g) Æ P4O6(s) + 3N2(g) K = [N2]3 [NO]6 (2.0)3 (2.0)6 K= 0.125 favors reactants Show your work mole and stoichiometry questions 42. Determine the number of grams that are in 0.688 mol of AgNO3. Ag = 107.87 g N = 14.01 g O = 16.00g x 3 169.88 g/ mole 0.688 mole x 169.88g mole = 116.87g How many moles of ethane (C2H6) contain 6.46 grams? 43. C = 2 x 12.01 g H = 6 x 1.01 g 30.08 g/ mole 6.46 g x 44. mole 30.08 g = 0.2147 moles Determine the number of grams that are in 3.48 mol of NaF Na = 22.99 g F = 19.00 g 41.99 g/ mole 3.48 moles x 45. 41.99g mole = 146.125 g For the equation below, if you have 3 moles of NH4NO3 how many moles of H2O can you produce? (1 step) NH4NO3 Æ N2O + 2 H2O 3 moles NH4NO3 46. x = 6 moles H2O You have 54 grams of C2H5 how many moles of H20 can you produce? (2-steps) 2 C2H5 + 5 O2 Æ 54g x 4 CO2 + 2 H2O 1 mole C2H5 29 g 1.86 C2H5 moles x 47. 2 mol H2O 1 mole NH4NO3 = 1.86 C2H5 moles 2 moles H2O 2 moles C2H5 = 1.86 H2O moles Use the equation given to determine how many grams of AlCl3 will be produced from 92 grams of Cl2 .(3-steps) 2 AlBr3 + 3 Cl2 Æ 3 Br2 + 2 AlCl3 92 g x 1 moles Cl2 70.9 g 1.2976 moles Cl2 x 2 moles AlCl3 3 moles Cl2 = 1.2976 moles Cl2 = 0.865 moles AlCl3 0.865 moles AlCl3 x 133.33 g 1 mole AlCl3 = 115.33 g 48. What is the percent yield if your actual yield is 8.65 g and your theoretical yield was 9.826 g? 8.65 g x 100 = 88.0% 9.826 g 49. What is the percent yield if your actual yield is 5.00g and your theoretical yield was 18.75 g? 5.00 g x 100 = 20.9% 18.75 g 50. If 35.0g of N2O4 reacts with 19.7g of N2H4, the products will be nitrogen, N2, and water, H2O. What mass of water, H2O, will be produced? N2O4 + 2N2H4 Æ 3N2 + 4H2O Solving from N2O4 35.0g x 1 mole N2O4 92.00g = 0.3804 moles N2O4 0.3804 moles N2O4 x 4 moles H2O 1 moles N2O4 = 1.5217 moles H2O 1.5217 moles H2O x 18.02g 1 mole H2O = 27.42g Solving from N2H4 19.7g x 1 mole N2H4 32g 0.6156 moles N2H4 x = 0.6156 moles N2H4 4 moles H2O 2 moles N2H4 = 1.231 moles H2O 1.231 moles H2O x 18.02g 1 mole H2O = 22.187g N2O4 is the excess reagent N2H4 is the limiting reagent