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Midterm 2015 Regents Chemistry Part A January 29, 2015 8:00 am Ms. Spaman Mr. Meredith Mr. Schlesing Regents Chemistry Midterm Test Part A 1 - 50 Multiple Choice 1. Which substance can be decomposed by a chemical change? 1) calcium 3) copper 2) potassium 4) water 2. At STP, which substance has particles arranged in a regular geometric pattern, also known as a crystalline lattice structure? 1) Ne 3) Hg 2) Zn 4) He 3. What occurs when a substance melts? 1) It changes from solid to liquid, and heat is absorbed. 2) It changes from solid to liquid, and heat is released. 3) It changes from liquid to solid, and heat is absorbed. 4) It changes from liquid to solid, and heat is released. 5. Which statement is an identifying characteristic of a mixture? 1) A mixture can consist of a single element. 2) A mixture can be separated by physical means. 3) A mixture must have a definite composition by weight. 4) A mixture must be homogeneous. 6. Which atom in the ground state has a partially filled second electron shell? 1) hydrogen atom 3) potassium atom 2) lithium atom 4) sodium atom 7. Compared to the charge and mass of a proton, an electron has 1) the same charge and a smaller mass 2) the same charge and the same mass 3) an opposite charge and a smaller mass 4) an opposite charge and the same mass 8. An atom in the excited state can have an electron configuration of 1) 2 - 8 - 2 (ls22s22p63s2) 2) 2 - 7 - 2 (ls12s22p53s2) 3) 2 - 8 - 1 (ls22s22p63s1) 4) 2 - 7 (ls22s22p5) 4. Given the key: Which particle diagram represents a sample containing the compound CO(g)? 9. What is the total number of protons and neutrons in the nuclide 80 35Br? 1) 35 3) 80 2) 45 4) 115 10. Which electron-dot symbol represents an atom of chlorine in the ground state? 1) 3) 1) 2) 2) 4) Page 1 3) 4) Regents Chemistry Midterm Test Part A 1 - 50 Multiple Choice 11. An experiment in which alpha particles were used to bombard thin sheets of gold foil led to the conclusion that an atom is composed mostly of 1) empty space and has a small, negatively charged nucleus 2) empty space and has a small, positively charged nucleus 3) a large, dense, positively charged nucleus 4) a large, dense, negatively charged nucleus 12. Which Group 16 element undergoes natural radioactive disintegration? 1) Po 3) Se 2) S 4) Te 13. At STP, both diamond and graphite are solids composed of carbon atoms. These solids have 1) the same crystal structure and the same properties 2) the same crystal structure and different properties 3) different crystal structures and the same properties 4) different crystal structures and different properties 14. Given the balanced particle-diagram equation: Which statement describes the type of change and the chemical properties of the product and reactants? 1) The equation represents a physical change, with the product and reactants having different chemical properties. 2) The equation represents a physical change, with the product and reactants having identical chemical properties. 3) The equation represents a chemical change, with the product and reactants having different chemical properties. 4) The equation represents a chemical change, with the product and reactants having identical chemical properties. 15. Given the following ground state electron configuration, 2 - 8 - 18 - 6 (or ls22s22p63s23p63d104s24p4) What is the total number of electrons in the principal energy level that has the greatest amount of energy? 1) 4 3) 18 2) 8 4) 6 16. Which atom in the ground state requires the least amount of energy to remove its valence electron? 1) lithium atom 3) rubidium atom 2) potassium atom 4) sodium atom Page 2 Regents Chemistry Midterm Test 17. An element that is malleable and a good conductor of heat and electricity could have an atomic number of 1) 16 3) 29 2) 18 4) 35 18. The transfer of electrons from sodium atoms to chlorine atoms results in the formation of 1) metallic bonds 3) nonpolar bonds 2) polar covalent bonds 4) ionic bonds 19. The atomic mass unit (amu) is defined as exactly 1/12 the mass of an atom of 1) 12 3) 24 6 C 12Mg 14 2) 6 C 4) 26 12Mg 20. The bonds in all network solids are 1) covalent 3) metallic 2) ionic 4) nonpolar 21. Which element has a crystalline lattice composed of positive ions through which electrons flow freely? 1) bromine 3) carbon 2) calcium 4) sulfur 22. What is the chemical formula for copper (II) chlorate? 1) Cu2Cl 3) Cu2ClO3 2) CuCl2 4) Cu(ClO3)2 Part A 1 - 50 Multiple Choice 25. Given the reaction: H2 + Cl2 →2HCl Which statement best describes the energy change as bonds are formed and broken in this reaction? 1) The breaking of the Cl–Cl bond releases energy. 2) The breaking of the H–H bond releases energy. 3) The forming of the H–Cl bond absorbs energy. 4) The forming of the H–Cl bond releases energy. 26. Which is an empirical formula? 1) C2H2 3) H2O2 2) H2O 4) C6Hl2O6 27. Which symbol represents an atom in the ground state with the most stable valence electron configuration? 1) B 3) Li 2) O 4) Ne 28. Which type of bond is formed between the carbon and oxygen atoms in a CO2 molecule? 1) nonpolar covalent 3) ionic 2) polar covalent 4) metallic 29. Which electron-dot structure represents a non-polar molecule? 23. How does the size of an aluminum atom change when it becomes an ion with a charge of 3+? 1) It becomes smaller by losing 3 electrons. 2) It becomes smaller by gaining 3 electrons. 3) It becomes larger by losing 3 electrons. 4) It becomes larger by gaining 3 electrons. 1) 24. In the electron cloud model of the atom, an orbital is defined as the most probable 1) charge of an electron 2) conductivity of an electron 3) location of an electron 4) mass of an electron 2) 3) 4) 30. Which element has an atom with the greatest attraction for electrons in a chemical bond? 1) As 3) N 2) Bi 4) P 31. Which element is a nonmetallic liquid at room temperature? 1) hydrogen 3) mercury 2) oxygen 4) bromine Page 3 Regents Chemistry Midterm Test Part A 1 - 50 Multiple Choice 32. The properties of elements are periodic functions of their 1) mass numbers 3) atomic radii 2) atomic masses 4) atomic numbers 38. Atoms of different isotopes of the same element differ in their total number of 1) electrons 3) protons 2) neutrons 4) valence electrons 33. The elements in Period 3 all contain the same number of 1) protons 2) neutrons 3) valence electrons 4) occupied principal energy levels 39. As the elements in Group 15 are considered in order of increasing atomic number, which sequence in properties occurs? 1) nonmetal → metalloid → metal 2) metalloid → metal → nonmetal 3) metal → metalloid → nonmetal 4) metal → nonmetal → metalloid 34. Which is an example of a metalloid? 1) sodium 3) silicon 2) strontium 4) sulfur 35. Which atom forms an ion with the largest radius? 1) I 3) Cl 2) Br 4) F 36. The diagram below represents the nucleus of an atom. 40. Which element in Period 2 of the Periodic Table is the most reactive nonmetal? 1) carbon 3) oxygen 2) nitrogen 4) fluorine 41. Which element in Period 3 exists as diatomic molecules at STP? 1) argon 3) aluminum 2) chlorine 4) sodium 42. Which sample of water contains particles having the highest average kinetic energy? 1) 25 mL of water at 95°C 2) 45 mL of water at 75°C 3) 75 mL of water at 75°C 4) 95 mL of water at 25°C What are the atomic number and mass number of this atom? 1) The atomic number is 9 and the mass number is 19. 2) The atomic number is 9 and the mass number is 20. 3) The atomic number is 11 and the mass number is 19. 4) The atomic number is 11 and the mass number is 20. 37. Which element is in Group 2 and Period 7 of the Periodic Table? 1) magnesium 3) radium 2) manganese 4) radon 43. Which aqueous solution is colored? 1) CuSO4(aq) 3) KCl(aq) 2) BaCl(aq) 4) MgSO4(aq) 44. Which element can be brittle or soft in the solid phase and is a poor conductor of heat and electricity? 1) calcium 3) strontium 2) sulfur 4) copper 45. Magnesium and calcium have similar chemical properties because a magnesium atom and a calcium atom have the same 1) atomic number 2) mass number 3) total number of electron shells 4) total number of valence electrons Page 4 Regents Chemistry Midterm Test 46. Which element is an alkali metal? 1) Na 3) Al 2) Mg 4) Cl Part A 1 - 50 Multiple Choice 49. Which mass measurement contains a total of three significant figures? 1) 22.0 g 3) 220 g 2) 22.00 g 4) 2200 g 47. Given: (52.6 cm) × (1.214 cm) 50. Which laboratory glassware is shown in the diagram below? What is the product expressed to the correct number of significant figures? 1) 64 cm2 3) 63.86 cm2 2 2) 63.9 cm 4) 63.8564 cm2 48. The diagram below shows a portion of a graduated cylinder. 1) Beaker 2) Erlenmeyer Flask What is the meniscus reading in milliliters? 1) 17.60 3) 17.80 2) 17.70 4) 18.40 Page 5 3) Graduated Cylinder 4) Watch Glass Regents Chemistry Midterm Part B and Part C Regents Chemistry Midterm Test Mr. Schlesing Part B 51 - 75 Multiple Choice 51. How many kilojoules are equivalent to 10 joules? 1) 0.001 kJ 3) 1000 kJ 2) 0.01 kJ 4) 10,000 kJ 58. The normal boiling point of water is equal to 1) 173 K 3) 373 K 2) 273 K 4) 473 K 52. What is the total number of Joules of heat that must be absorbed to change the temperature of 100. grams of H2O from 25.0ºC to 30.0ºC? 1) 420. 3) 10500 2) 2100 4) 13000 59. The graph below represents changes of state for an unknown substance. 53. What is the total number of joules released when a 5.00-gram sample of water changes from liquid to solid at 0°C? 1) 334 J 3) 2260 J 2) 1670 J 4) 11 300 J 54. Solid A at 80ºC is immersed in liquid B at 60ºC. Which statement correctly describes the energy changes between A and B? 1) A releases heat and B absorbs heat. 2) A absorbs heat and B releases heat. 3) Both A and B absorb heat. 4) Both A and B release heat. 55. Which phase change is exothermic? 1) H2O(s) → H2O(…) 3) H2O(s) → H2O(g) 2) H2O(…) → H2O(s) 4) H2O(…) → H2O(g) 56. Which Kelvin temperature is equal to –73ºC? 1) 100 K 3) 200 K 2) 173 K 4) 346 K 57. A student investigated the physical and chemical properties of a sample of an unknown gas and then identified the gas. Which statement represents a conclusion rather than an experimental observation? 1) The gas is colorless. 2) The gas is carbon dioxide. 3) When the gas is bubbled into limewater, the liquid becomes cloudy. 4) When placed in the gas, a flaming splint stops burning. What is the boiling temperature of the substance? 1) 0ºC 3) 70ºC 2) 20ºC 4) 40ºC 60. Which equation is correctly balanced? 1) CaO + 2H2O → Ca(OH)2 2) NH3 + 2O2 → HNO3 + H2O 3) Ca(OH)2 + 2H3PO4 → Ca3(PO4)2 + 3H2O 4) Cu + H2SO4 → CuSO4 + H2O + SO2 61. Given the balanced equation representing a reaction: Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) Which type of reaction is represented by this equation? 1) decomposition 3) single replacement 2) double replacement 4) synthesis Page 7 Regents Chemistry Midterm Test Part B 51 - 75 Multiple Choice Mr. Schlesing 62. The graph below represents the uniform heating of a substance, starting with the substance as a solid below its melting point. Which line segment represents an increase in potential energy and no change in average kinetic energy? 1) AB 3) CD 2) BC 4) EF 63. Given the unbalanced equation: NaOH + H3PO4 → Na3PO4 + H2O When the equation is correctly balanced, the coefficient of H2O will be 1) 1 3) 3 2) 2 4) 4 64. What is the gram formula mass of Mg(ClO3)2? 1) 107 g 3) 174 g 2) 142 g 4) 191 g 66. The percent by mass of carbon in HC2H3O2 is equal to 1) 3) 2) 4) 67. What is the mass of 2.0 moles of NO2? 1) 92 grams 3) 46 grams 2) 60. grams 4) 30. grams 68. In the formula X2(SO4)3, the X represents a metal. This metal could be located on the Periodic Table in 1) Group1 3) Group 13 2) Group 2 4) Group 14 69. Which species represents a chemical compound? 1) N2 3) Na 2) NH4+ 4) NaHCO3 70. A real gas would behave most like an ideal gas under conditions of 1) low pressure and low temperature 2) low pressure and high temperature 3) high pressure and low temperature 4) high pressure and high temperature 65. What is the total number of atoms of oxygen in the formula Al(ClO3)3 • 6H2O? 1) 6 3) 10 2) 9 4) 15 Page 8 Regents Chemistry Midterm Test Mr. Schlesing 71. Which graph represents the relationship between pressure and volume for a sample of an ideal gas at constant temperature? 1) Part B 51 - 75 Multiple Choice 72. Based on Reference Table H, which substance has the weakest intermolecular forces? 1) ethanoic acid 3) propanone 2) ethanol 4) water 73. According to Reference Table H, what is the boiling point of ethanoic acid at 80 kPa? 1) 28°C 3) 111°C 2) 100°C 4) 125°C 2) 3) 74. A sample of a gas has a volume of 40. milliliters at 76.0 kPA. What will be the new volume of the gas if the pressure is increased to 80.0 kPa, temperature remaining constant? 1) 80 ml 3) 38 ml 2) 42 ml 4) 20 ml 75. A rigid cylinder with a movable piston contains a 2.0-liter sample of neon gas at STP. What is the volume of this sample when its temperature is increased to 30.°C while its pressure is decreased to 90. kilopascals? 1) 2.5 L 3) 1.6 L 2) 2.0 L 4) 0.22 L 4) Page 9 Part B - – Constructed Response Questions [5 pts total] Place all answers on the answer sheet Base your answers to questions 76 and 77 on the table below. Naturally Occurring Isotopes of Copper Isotope Notation Percent Natural Atomic Mass Abundance (%) (atomic mass units, u) Cu–63 69.17 62.930 Cu–65 30.83 64.928 76. What is the total number of neutrons in Cu–65? [1pt] 77. Show a correct numerical setup for calculating the atomic mass of copper. [1pt] Base your answers to questions 78 and 79 on the information below. A glass tube is filled with hydrogen gas at low pressure. An electric current is passed through the gas, causing it to emit light. This light is passed through a prism to separate the light into the bright, colored lines of hydrogen’s visible spectrum. Each colored line corresponds to a particular wavelength of light. One of hydrogen’s spectral lines is red light with a wavelength of 656 nanometers. Tubes filled with other gases produce different bright-line spectra that are characteristic of each kind of gas. These spectra have been observed and recorded. 78. Explain, in terms of electron energy states and energy changes, how hydrogen’s bright-line spectrum is produced. [1pt] 79. A student measured the wavelength of hydrogen’s visible red spectral line to be 647 nanometers. Show a correct, numerical setup for calculating the student’s percent error. [1pt] Base your answers to question 80 on the table below. Compound H2O H2S H2Se H2Te Boiling Point 100. °C -60.7 °C -41.5 °C -2.2 °C 80. Explain, in terms of intermolecular forces, why water has a higher boiling point than H2S, H2Se, and H2Te. [1pt] Part C – Constructed Response Questions [20 pts total] Midterm Exam Directions: Choose 4 of the 6 groups in this part of the examination. For the 4 groups that you choose to answer, make sure you answer all the questions within those groups. If you complete all 6 groups on your answer sheet, only the first 4 will be graded. Make sure that you answer the questions for each group in the correct location on the answer sheet. (20 points) Group 1) a) Given the information about the elements in the table below, fill in the missing information on the corresponding table on your answer sheet. [1pt] # of Protons Electron configuration Element Symbol of atom 12 2–8–2 11 Na 2–8 Ne 8 2–5 B ***Use only the elements from the above table (a) to answer questions b), c), d), & e) b) The element with the highest first ionization energy? [1pt] c) The element that will form a negative ion in a compound? [1pt] d) The element with the greatest number of unpaired electrons in its Lewis dot (electron dot) diagram? [1pt] e) The metal that would combine with oxygen in a one-to-one ion ratio? [1pt] Group 2) Answer the following questions (a,b,c,d) about a compound that is created by the elements of calcium and fluorine. a) c) d) Describe the type of chemical bond that would occur in a compound that consists of calcium and fluorine atoms. [1pt] Describe a specific chemical or physical property for a solid of this compound (Your property can’t be that it is a solid, that information is given in the problem.) [1pt] Give the correct chemical name for this compound of calcium and fluorine. [1pt] Draw the Lewis Structural Formula (Dot Diagrams) for this compound. [1pt] e) Write the correct name of Ni(NO3)2. [1pt] b) Group 3) For each of the following, give the symbol of the element described. a) b) c) d) e) an alkaline earth metal found in Period 4. [1pt] the element in Period 4 with the greatest attraction for an electron in a chemical bond. [1pt] the most metallic element found in Group 15. [1pt] a diatomic molecule that is stable due to a triple covalent bond in its molecule. [1pt] a diatomic molecule that is a liquid at room temperature. [1pt] Group 4) A student wished to perform a lab to calculate the percent composition by mass of water in a hydrated crystal. The student first obtained the mass of an empty, dry evaporating dish. The student then placed a small amount of the hydrated crystal in the evaporating dish and weighed it. The student’s data is shown below: Mass of empty evaporating 11.70 g dish Mass of evaporating dish + 14.90 g hydrated crystal a) Explain at least 2 additional lab procedures that this student will need to do in order to gather enough data to calculate the percentage of water in this hydrated crystal. [2pts] b) At the end of this lab, the student found the mass of the anhydrous crystal (dehydrated crystal) to be 2.83 grams. Calculate using significant figures, the mass of the water found in the hydrated crystal. (show your work on the answer sheet) [2pts] c) Calculate the percentage of water in the original hydrated crystal. (show your work on the answer sheet) [1pt] Group 5) The electron configuration for the phosphorus atom is 2–8–5 or 1s22s22p63s23p3. Indicate for this atom: a) b) c) d) e) the number of completely filled principal energy levels. [1pt] the type of bond that forms when its chemically combines with chlorine. [1pt] the number of protons in its nucleus. [1pt] the electron dot diagram (Lewis dot diagram) for an atom of this element. [1pt] the specific ion it will most likely form when bonding with a metal atom. [1pt] Group 6) Many periodic trends can be observed on the modern periodic table. Answer the following questions about periodic trends on your answer sheet. a) Graph the periodic trend in atomic radius for Period 3 on the appropriate graph on your answer sheet. [1pt] b) Explain the cause for the observed periodic trend in atomic radius for Period 3 elements. [1pt] c) Graph the group trend in atomic radius for Group 2 on the appropriate graph on your answer sheet. [1pt] d) Explain the cause for the observed group trend in atomic radius for Group 2 elements. e) Ions of Group 2 elements are found to have radii smaller than that of the individual atoms, explain the cause of this observed trend. [1pt] End of Exam Part A = ______ Name: ______________________________ Teacher: _________________ Class: ____________ Regents Chemistry Midterm Answer Sheet Total Score Part B = ______ Part C = ______ Part A – do all 50 questions. 1. _____ 11. _____ 21. _____ 31. _____ 41. _____ 2. _____ 12. _____ 22. _____ 32. _____ 42. _____ 3. _____ 13. _____ 23. _____ 33. _____ 43. _____ 4. _____ 14. _____ 24. _____ 34. _____ 44. _____ 5. _____ 15. _____ 25. _____ 35. _____ 45. _____ 6. _____ 16. _____ 26. _____ 36. _____ 46. _____ 7. _____ 17. _____ 27. _____ 37. _____ 47. _____ 8. _____ 18. _____ 28. _____ 38. _____ 48. _____ 9. _____ 19. _____ 29. _____ 39. _____ 49. _____ 10. _____ 20. _____ 30. _____ 40. _____ 50. _____ Part A Score = Part B – do all questions. 51. _____ 56. _____ 61. _____ 66. _____ 71. _____ 52. _____ 57. _____ 62. _____ 67. _____ 72. _____ 53. _____ 58. _____ 63. _____ 68. _____ 73. _____ 54. _____ 59. _____ 64. _____ 69. _____ 74. _____ 55. _____ 60. _____ 65. _____ 70. _____ 75. _____ 76. ___________ 77. 78. _________________________________________________________________________________ ______________________________________________________ ______________________________________________________ 79. 80. ________________________________________________________________________________ ______________________________________________________ ______________________________________________________ Part B Score = Part C - complete 4 of the 6 groups only! Group 1 a) # of Protons 12 11 Electron configuration of atom 2–8–2 Element Symbol [1pt] Na Ne 2–8 8 2–5 B b) _______________________________ [1pt] c) _______________________________ [1pt] d) _______________________________ [1pt] e) _______________________________ [1pt] Group 2 a) ____________________________________________________________________ __________________________________________________________________[1pt] b) ___________________________________________________________________ ___________________________________________________________________[1pt] c) __________________________________ [1pt] d) [1pt] e) ___________________________________ [1pt] Total Points on this Page =_______ Part C – Continued Group 3 a) _____________ [1pt] b) _____________ [1pt] c) _____________ [1pt] d) _____________ [1pt] e) _____________ [1pt] Group 4 a) #1 Step______________________________________________________________ ______________________________________________________________________ #2 Step______________________________________________________________ _________________________________________________________________[2pts] b) Show work in the box below and circle your final answer. [2pts] c) Show work in the box below and circle your final answer. [1pt] Group 5 a) ________________ [1pt] b) ________________ [1pt] c) ________________ [1pt] d) ________________ [1pt] e) ________________ [1pt] Total Points on this Page = ______ Group 6 a.) Atomic Radii of Period 3 b.) ______________________________________ 190 __________________________________________ 180 170 160 __________________________________________ Atomic Radius (picometers) 150 140 __________________________________________ 130 120 __________________________________________ 110 100 __________________________________________ 90 80 70 60 50 40 30 20 10 0 Na Mg Al Si P S Cl Ar Period 3 Elements c.) Atomic Radii of Group 2 d.) _________________________________________ 240 __________________________________________ 230 220 210 __________________________________________ 200 Atomic Radius (picometers) 190 __________________________________________ 180 170 __________________________________________ 160 150 __________________________________________ 140 130 120 110 100 90 80 70 0 Be Mg Ca Sr Ba Ra Group 2 elements e.) ______________________________________________________________________________________ _________________________________________________________________________________________ _________________________________________________________________________________________ Total Points on this Page = _________ k>3 Name: ftn,. Teacher: *t V1 Midterm Answer Sheet Chemist Part A - 11. 2^ 3 _l_ I 44_ .1 6. 7. 8. 9. 10. A Part B Part C: = : do all50 questions. ,1- 7 2. I 3lL 6.3 ?.3 ^ 22. 4 26. a_ a_ a_ I 28. L 3L sI k 2e. L 30. 3 40. 42. ( 44. 2 4s L/ $I t L L 4r. 3 27.4 8q 3_ 4_ L 24. 3 2s. t/ sI 3A 21. n. 4.3 6 5. Part 46. Ll I 47. 2 48. I 4s. { 2 s0. Part A Score: Part B - do all questions. n. L 52. 7 n.2 j .2^ 6r. ) 57. 2- 62. z3 66. 67. ]- 72. 68. _(_ 69. T 74. 58. 54.-l- 59. ssL ,u. 1L 77. s6. 3 A- 60. 63. . A a< 65. , e1,17 x (2,rso .3o8r 1_ (E) 6c{,qLa (,9.5'{ 64. Gi) ( 7 3 70. 17 x 3o,89 n 67, 635q, 71. 1_l ( 3 n3 3 7s. ( { 62,1ao (^1 C -12{ z lcto &"4+ : /oo +^, CrcJ'e 78. 79. b ej-cor a.cc<-p *t 7"*-r= .6't7"n-6{( 6{C n' = ('37tL sroc) 4-"'z'd!\sL$cr ^J t*tJt; +t-, .*Xit O 80. h* .,t d*r*-"p ^It' /*- br[," Part B Score = Paft C Group - do 4 of the 6 groups only! I a) # of Protons Electron configuration of atom 2-8-2 t2 l1 7-8- (a 7 Na Ne o 2-5 t$ 2-3 N.- [1pt] lY\9. ( 2-8 'la 8 b) Element Symbol B [1pt] c) C- .* N trou [1pt] M^- uy Group 2 lrpq a) lptl G^,2 < - (;,! b) €^ c) d) Co\ci.,n^, ft.r.ci d.-- d-J"Lrl;'dNick \ trptl [1pt] [1pt] Total Points on this Page = - Continued C=-? Group 3 Paft C "l ol B. [1pt] [1pt] c) [1pt] l"L d) "y Group 4 6cr- grptl ll'o dI'-L {. a) #1 Step__: .4-q.\ -L/ #2 Step b) [1pt] .fr( q-,L= 2ptsl Show work in the box below and circle your final answer. [2pts] hy"l*F,, * cn:dLL nr"== rK itL y [ (,7ot b",U\L 11 72 c-r .%feo ((r nswer. [1pt] Show work in the box % Lro';ffi-,.n,o<> .3?> "/ #ru=6'o.ao oc 0-( +T Group 5 a) [1pt] b) ( c) d) e) .?' P-t^ _ tlptl [tpt] Total Points on this Page: Group 6 a.) c.) Atomic Radii of Period ul -{h- 3 A,,^ fl6r.r,>- Q,&i-> Atomic Radii of Group 2 Group 2 elements '; A'=- d."- f er."t* u (*( Total Points on this Page =