Unit 3 QMA - Test Review:

Transcription

1 Unit 3 QMA - Test Review: Give the Orbital Diagram for the following elements: 1. Chromium 2. Nitrogen Give the COMPLETE electron configuration for the following elements: 3. Argon 1s 2 2s 2 2p 6 3s 2 3p 6 4. Phosphorous 1s 2 2s 2 2p 6 3s 2 3p 3 Give the Noble Gas electron configuration for the following elements: 5. Plutonium Pu = [Rn] 7s 2 5f 5 6d 1 6. Mercury Hg = [Xe] 6s 2 4f 14 5d Complete the table. Element Total # of electrons Valence Configuration Gain or Lose e - How Many? Ion Symbol New Valence Configuration Total # of e - Phosphorous 15 3s 2 3p 3 G 3 P -3 3s 2 3p 6 18 Chlorine 17 3s 2 3p 5 G 1 Cl -1 3s 2 3p 6 18 Cesium 55 6s 1 L 1 Cs +1 5s 2 5p 6 54 Lithium 3 2s 1 L 1 Li +1 1s 2 2 Give the 4 quantum numbers for the last electron of the following elements: 8. Phosphorous n=3, l=1, ml=1, ms= +1/2 9. Manganese n= 3, l=2, ml=2, ms= +1/2 10. Silver n= 4, l=2, ml=1, ms= -1/2 11. Promethium n= 4, l=3, ml=0, ms= +1/2 12. Iodine n= 5, l=1, ml=0, ms= -1/2

2 Determine if the following sets of quantum numbers would be allowed in an atom. If not, explain why and if so, identify the corresponding atom n = 2, l = 1, ml = 0, ms = + Yes n = 4, l = 0, ml = 2, ms = No, because orbital 0 only has sub level n = 1, l = 1, ml = 0, ms = No, because l must be one less than n Give the element with the LARGER radius, ionization energy, electronegativity and reactivity. ELEMENTS ATOMIC RADIUS IONIZATION ENERGY ELECTRONEGATIVITY Sodium and Aluminum Na Al Al Chlorine and Iodine I Cl Cl Oxygen and Fluorine O F F Magnesium and Calcium Ca Mg Mg Circle the element / ion with the larger radius. 16. Mg or Mg S or S N 3- or F Sr 2+ or Br Cl - or Mg B or F For each of the following families, give their relative reactivity, the number of valence electrons, and at least one additional piece of information (such as how they are found in nature or what other group the generally react with). 22. Alkaline Earth Metals Very reactive, s 2, most in the earth s crust 23. Alkali Metals Very reactive, s 1, they will react in air and with water 24. Halogens Very reactive, s 2 p 5, they form salts 25. Noble Gases non reactive, s 2 p 6, they are gases at room temperature

3 Matching (1 point each): Match the description in Column B with the correct term in Column A. Write the letter in the blank provided. Each term matches with only one description, so be sure to choose the best description for each term. Not all descriptions will be used. Column A Column B A 26. Alkaline Earth Metal D 27. Transition Metal F 28. Alkali Metal A. located in the second column B. solid or liquid mixture of two or more metals C. horizontal row of elements I _ 29. Noble Gases D. located in columns 3-12 K 30. Halogen C 31. Period E 32. Ionization Energy H 33. Valence Electron E. energy required to remove an e- from an atom F. located in the first column G. ability of an atom to attract electrons G 34. Electronegativity I. located in column 18 J 35. Group H. an electron in the outermost shell of an atom J. vertical column of elements K. located in column 17 _D_ 36. Elements in a family or group in the periodic table often share similar properties because a. They look alike. b. They are found in the same place on Earth. c. They have the same physical state. d. Their atoms have the same number of electrons in their outer energy level. _B 37. Groups 3-12 are commonly referred to as a. Alkali metals. b. Transition metals. c. Lanthanides. d. Actinides. C_ 38. Which of the following elements has the highest electronegativity? a. Ca b. Cu c. Br d. As _B_ 39. An atom is neutral because the number of a. Electrons equals the number of neutrons. b. Electrons equals the number of protons. c. Protons equals the number of neutrons. d. None of the above.

4 Unit 4 and 4B QMA Test Review Write the formula for the following compounds 1. Aluminum Bromide AlBr3 4. Dinitrogen Tetroxide N2O4 2. Ammonium Fluoride NH4F 5. Iron (II) Sulfate FeSO4 3. Copper (I) Chloride CuCl 6. Carbon Dioxide CO2 Name the following compounds 7. NaHCO 3 Sodium Bicarbonate 10. MgO Magnesium Oxide 8. H 2S HydroSulfic acid 11. N 2O 3. Dinitrogen Trioxide 9. Fe 2(SO 4) 2 Iron (II) Sulfate 12. CuCl 2 Copper (II) Chloride Name the following compounds: 13. HBr Hydrobromic acid 16. H 2CO 3 Carbonic acid 19. Pb(NO 4) 2 Lead (II) Pernitrate 22. H 2SO 3 Sulfurous acid 25 H 2SO 4 Sulfuric acid 28. HNO 3 Nitric acid 31. HNO 2 Nitrous acid 34. HNO 3 Nitric acid 14. BaSO 3 Barium Sulfite 17. HI Hydro iodic acid 20. Zn 3(PO 2) 2 Zinc Hypophosphite 23. HC 2H 3O 2 Acetic acid 26. Ra(C 2H 3O 2) 2 Radium acetate 29. H 3P Hydrophosphic acid 32. Fe(ClO 4) 3 Iron (III) perchlorate 35. SnO Tin (II) Oxide 15. Al 2(SO 4) 3 Aluminum Sulfate 18. Ca(SO 3) 2 Calcium Sulfite 21. Ca 3(PO 4) 2 Calcium Phosphate 24. K 2CrO 3 Potassium Chromite 27. NiClO Nickel Hypochlorite 30. H 3PO 4 Phosphoric acid 33. K 2O Potassium Oxide 36. H 2SO 3 Sulfurous acid 37. ZnSO 2 Zinc hyposulfite 38. Al(ClO) 3 Aluminum hypochlorite 40. Hg 2Cl Fe(OH) 2 Mercury (I) Chloride Iron (II) Hydroxide 43. Ba(ClO 2) Li 3PO 3 Barium Chlorite Lithium Phosphite 46. N 2O Cl 2S 7 Dinitrogen Tetraoxide Dichloride heptasulfide 49. Rb 2CO HClO Rubidium carbonate hypochlorous acid Write the chemical formula for the following compounds: 52 Hydrochloric Acid 53. Copper (II) Perchlorate HCl Cu(ClO4)2 55. Sodium Hypochlorite 56. Phosphoric Acid NaClO H3PO4 58. Sulfurous Acid 59. Tin(II) Fluoride 39. HI Hydro iodic acid 42. Fe 2(CrO 4) 3 Iron (III) chromate 45. KMnO 4 Potassium permanganate 48. PbO 2 Lead (IV) Oxide 51. Fe(OH) 3 Iron (III) hydroxide 54. Strontium Nitrate Sr(NO3)2 57. Lead(IV) Oxide PbO2 60. Potassium Permanganate H2SO3 SnF2 KMnO4 61. Aluminum Hyponitrite 62. Chromous Acid 63. Sodium Phosphate

5 Al(NO)3 H2CrO3 NaPO4 64. Mercury (II) Sulfide HgS 65. Sodium Sulfite Na2SO3 66. Ammonium Phosphate (NH4)3PO4 67. Tin(IV) Fluoride SnF4 68. Iron Nitrate Fe(NO3)2 69. Calcium Perchromate Ca(ClO5)2 70. Hyposulfurous Acid H2SO3 71. Copper(I) Sulfide Cu2S 72. Titanium (III) Chlorate Ti(ClO4)3 73. Calcium Hydroxide Ca(OH)2 74. Sodium Bicarbonate NaHCO3 75. Aluminum Hypophospite Al(PO2)3 76. Lithium Hyposulfite Li2SO2 77. Colbalt (III) Sulfite Co2(SO3)3 78. Tin(IV) Nitrite Sn(NO2)4 79. Calcium Fluoride CaF2 80. Lead(IV) Acetate Pb(C2H3O2)4 81. Ammonium Phosphite (NH4)3PO3 82. Iron(III) Oxide Fe2O3 83. Hydrosulfuric Acid H2S 84. Iron(II) Chromate FeCrO4 85. Potassium Cyanide KCN 86. Ammonium Sulfate (NH4)2SO4 87. Calcium Chloride CaCl2 88. Barium Hydroxide Ba(OH)2 89. Mercury(II) Sulfide HgS 90. Silver Chlorate Ag(ClO3)2 91. Lead (II) Sulfate PbSO4 92. Potassium Permanganate KMnO4 93. Silicon Dioxide SiO2 94. Draw the condensed structural diagram of the following types of compounds a. Alkane b. Alkene c. Alkyne d. Alcohol e. Carboxylic acid Draw the dot diagram for each of the IONIC compounds below CaO 6. Na2S 96. SrF2 10. KI

6 97. Complete the table below. Formula Electron Dot Diagram Shape Structural Formula Trigonal NCl3 Pyramidal CO2 Linear H2O Bent CH3F Tetrahedral VSPER Worksheet: 98. What is the main idea behind VSEPR theory? It is a set of rules whereby the chemist may predict the shape of an isolated molecule. It is based on the premise that groups of electrons surrounding a central atom repel each other, and that to minimize the overall energy of the molecule, these groups of electrons try to get as far apart as possible.