* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Fall Final Review Honors
Nuclear binding energy wikipedia , lookup
Jahn–Teller effect wikipedia , lookup
IUPAC nomenclature of inorganic chemistry 2005 wikipedia , lookup
Low-energy electron diffraction wikipedia , lookup
Photoelectric effect wikipedia , lookup
Chemistry: A Volatile History wikipedia , lookup
Photoredox catalysis wikipedia , lookup
Molecular Hamiltonian wikipedia , lookup
X-ray fluorescence wikipedia , lookup
Size-exclusion chromatography wikipedia , lookup
Elementary particle wikipedia , lookup
Biochemistry wikipedia , lookup
Chemical thermodynamics wikipedia , lookup
Marcus theory wikipedia , lookup
Bond valence method wikipedia , lookup
Molecular orbital wikipedia , lookup
Bent's rule wikipedia , lookup
Metastable inner-shell molecular state wikipedia , lookup
Hydrogen atom wikipedia , lookup
History of chemistry wikipedia , lookup
Light-dependent reactions wikipedia , lookup
Electronegativity wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Electron scattering wikipedia , lookup
Resonance (chemistry) wikipedia , lookup
Gas chromatography–mass spectrometry wikipedia , lookup
Atomic orbital wikipedia , lookup
Computational chemistry wikipedia , lookup
Rutherford backscattering spectrometry wikipedia , lookup
Physical organic chemistry wikipedia , lookup
Atomic nucleus wikipedia , lookup
Metallic bonding wikipedia , lookup
Molecular dynamics wikipedia , lookup
Photosynthetic reaction centre wikipedia , lookup
Molecular orbital diagram wikipedia , lookup
History of molecular theory wikipedia , lookup
Hypervalent molecule wikipedia , lookup
Electron configuration wikipedia , lookup
CHEMISTRY I HONORS – 1st SEMESTER EXAM REVIEW – Fall 2010 STRATEGY: Start by reading through your notes to refresh your memory on these topics. Then, use this review sheet as a starting point to identify the areas on which you need to spend more study time. For those areas, go back to homework assignments, quizzes, and reviews to practice more problems. I would also recommend going through all of your tests since these questions are only samples and do not include specific examples of how vocabulary and other conceptual information might appear in a multiple-choice or other format. Remember you can access notes and reviews on Mrs. J’s Chemistry page at: www.nisd.net/comartww/pages/chem/notes. FORMAT: Questions will include multiple-choice and matching. A formula bank will be provided in addition to any values that you might need (electronegativity, etc.), but you will NOT be given “formulas” for items listed in the VOCAB sections (average atomic mass, % error, etc.). Measurement – Ch. 1.3,1.5-1.8,5.1 1. In a lab, the average measured density for Pre-1982 pennies was 7.98 g/cm3. Given that the literature value for the density is 8.92 g/cm3, calculate the percent error. 2. How many sig figs are in the following numbers? a. 2.35 c. 89.70 b. 34,000 d. 0.0052 3. Convert the following numbers into or out of scientific notation. a. 548,000 c. 1.200 × 10-3 b. 0.0000770 d. 9.25 × 107 4. Osmium is the densest element with a density of 22.57 g/cm3. Find the mass of a 56.2 cm3 sample of osmium. Matter – Ch. 1.9 10. Classify the following substances as solid, liquid, gas, or plasma based on their properties. a. flexible volume, high KE, particles can disperse freely. b. flexible volume, very high KE, particles are charged. c. fixed volume, very low KE, orderly particles. d. fixed volume, low KE, particles can move past each other. 11. Compare and contrast a solution, colloid, and suspension. 12. Classify the following as element, compound, heterogeneous mixture, or solution. a. graphite (carbon) b. grape juice c. table salt (NaCl) d. pepper Atomic Structure – Ch. 2.3-2.6,7.2,7.4-7.9,7.11 15. Identify the scientists who made the following discoveries. a. Atoms contain negative particles called electrons. b. The mass of an electron is 9.11 10-28 g. c. Atoms contain neutral particles called neutrons. d. Atoms contain a dense, positive nucleus. e. Atoms are indivisible and resemble billiard balls. 16. Describe the evolution of the atomic model from the billiard ball model to the electron cloud model. 17. Write the isotope symbol, including atomic number & mass number, for the following isotopes. a. carbon-14 c. nickel-63 b. chromium-53 d. zirconium-92 18. Complete the table for the following isotopes. Symbol Zn Atomic # 20 Mass # 65 74 40 # of protons 34 # of neutrons 21 # of electrons 18 5. Perform the following SI prefix conversions. a. 65.2 mm = ? dm c. 65,000 L = ? mL b. 2.3 kg = ?g d. 0.502 km = ? cm 6. How many milliliters are in a 2.0 quart jug of milk? 7. Mrs. J. spent last weekend grading lab notebooks. If she spent 5.5 min on each notebook, how many hours did it take her to grade all 95 notebooks? 8. Calculate the density from the slope of a "Mass vs. Volume" graph. 9. Record the appropriate # of SigFigs when measuring. VOCAB: accuracy vs. precision 13. Classify the following as chemical or physical changes. a. cutting wire b. ripening tomato c. apple slices turning brown d. compressing a gas 14. Classify the following properties as physical or chemical. a. melts at 68.0C b. corrosive c. reacts violently with water d. decomposes in air e. magnetic VOCAB: kinetic molecular theory law of definite composition law of multiple proportions 19. Calculate the wavelength if the frequency is 2.5 x 105 Hz. 20. Find the energy of a photon if frequency is 7.31 x 1014 Hz. 21. Describe how Bohr’s model explains the bright lines (red, green, violet, violet) in the emission spectrum of hydrogen. 22. What is the primary difference between the modern model of the atom and Bohr’s model? 23. Draw orbital diagrams for the following elements. Symbol Atomic # Orbital Diagram F V 24. Explain why chromium’s electron configuration is [Ar] 4s13d5 instead of the expected configuration of [Ar] 4s23d4. 25. Give the shorthand electron configuration for the following. Symbol # eShorthand e- Configuration Pd At 26. Predict the ions that will form from the following atoms and give the shorthand configuration of the ion. Atom Ion Noble Gas Shorthand e- Configuration Rb Te 27. How did Mendeleev and Mosely arrange the elements in the periodic table? 28. Circle the atom with the LARGER radius. a. Ra N b. Ne Xe 29. Circle the particle with the LARGER radius. a. Cl Cl – b. Mg Mg2+ Nuclear Chemistry – Ch. 2.5,3.1,18.1-18.4,18.5 34. Calculate the average atomic mass of Br, if the nuclides are Br-158(25.34%), Br-160(50%), and Br-162(24.66%). 35. Calculate the relative abundance of sodium nuclides. If the average atomic mass is 22.99 and the nuclides are Na-23 (mass is 22.985amu) and Na-24 (mass is 23.789 amu). 36. Find the mass defect of Pu. If the average atomic mass of Pu is 244. (1 p= 1.007276 amu, 1 n = 1.008665 amu, 1 e= 0.0005486 amu) 37. __________ + 4He 243Bk + 1n 38. 238U + 12C ________ + 6 1n Chemical Bonding – Ch. 2.8, 4.8, 8.1-8.2,8.4-8.8 41. Based on their electronegativities (p353), are the bonds in the following substances IONIC, POLAR, or NONPOLAR? a. MgO c. LiCl b. H2O d. Br2 42. Are the following properties characteristics of ionic, covalent, or metallic bonding? a. These bonds are formed by delocalized electrons in an “electron sea.” b. These bonds involve a transfer of electrons. c. Substances containing these bonds are malleable and have very high melting points. d. Substances containing these bonds do not conduct electricity and have low melting points. e. Compounds containing these bonds have a crystal lattice structure. f. These bonds are formed by sharing electrons. 43. Use Lewis Diagrams to show the formation of MgO. 44. Use Lewis Diagrams to show the formation of H2O. 30. Circle the atom with the HIGHER first ionization energy. a. Li Cs b. Ba As 31. Circle the atom with the HIGHER melting point. a. Cl Si b. Cs W 32. Why are there small jumps in the 1st ionization energies of the elements as you move across a period? 33. Why is there a large increase in ionization energy when the 4th electron is removed from aluminum? VOCAB: ionization energy periodic law metals/nonmetals/metalloids shielding excited state/ground state quark wave-particle duality isotope valence/core ephoton Pauli Exculsion Principle Hund’s Rule Heisenberg Uncertainty Principle Aufbau Principle average atomic mass 39. Find the nuclear binding energy of Pu, using the information from question 36. 40. Na-24 has a half life of 14.8 hours. If you have 5.6g left of this substance after 7.4 days, how much of this substance did you have originally (in kg)? VOCAB: fission fusion alpha particles Beta particles isotope half life Chain reaction critical mass mass defect Gamma rays positron avg. atomic mass 45. Explain the relationship between potential energy and stability. 46. Write formulas for the following compounds (HINT: First determine ionic/acid/covalent). a. calcium bromide d. silicon dioxide b. iron(III) sulfate e. dinitrogen tetroxide c. hydrofluoric acid f. sulfurous acid 47. Write names for the following compounds (HINT: First determine ionic/acid/covalent). a. CrCl3 d. MgSO4 b. Cu2CO3 e. P4O6 c. AsCl5 f. HClO3 48. Explain the difference between nonpolar covalent, polar covalent, and ionic bonds in terms of sharing of electrons and electric charge. VOCAB: bond energy (bond length) electronegativity chemical bond potential energy dipole Molecular Structure – Ch. 8.9-8.13 49. Explain the main idea of the VSEPR Theory. 50. For each of the following molecules, draw the Lewis electron dot diagram, give the shape and bond angle(s), and state whether the molecule is polar or nonpolar. Show your work in the spaces provided for counting valence e - and e- pairs. Number of Lewis Diagram Counting Molecular Shape Molecular & Bond Angle(s) Polarity valence e e pairs SiO2 AsF5 51. Draw the dipole moments for each bond in the following molecules and circle whether the molecule is polar or nonpolar. TeCl2 bent BCl3 trigonal planar CH2Cl2 tetrahedral Te Cl Cl Cl Cl B C Cl polar nonpolar VOCAB: octet rule bond angle expanded octet dipole moment Cl polar nonpolar lone pairs bonding pairs Chemical Reactions – Ch. 3.6-3.7,4.5-4.6,4.8-4.10 52. Write a word equation for the following reaction (incl. how many? of what? what state?). BaCl2(s) + 3O2(g) Ba(ClO3)2(s) 53. Rewrite and balance the following word equation using chemical formulas, physical states, and energy. – When solid sodium chlorate absorbs energy, it produces solid sodium chloride and oxygen gas. Predict the products and balance (54-57). Write N.R. if no reaction will occur. Include physical states . 54. Cu(s) + MgSO4(aq) 55. C5H12(l) + O2(g) Chemical Composition – Ch. 3.2-3.5 62. How many magnesium sulfate molecules are in 25.0 g? 63. Find the molarity of a 750 mL solution containing 346 g of potassium nitrate. 64. Calculate the number of grams required to make a 50.0 mL solution of 6.0M NaOH. 65. Find the % composition of copper(II) chloride. H polar Cl H nonpolar 56. NH4Cl(aq) + Pb(NO3)2(aq) 57. Fe2O3(s) 58. For each of the reactions in #54-57, specify whether it is combustion, synthesis, decomposition, single replacement, or precipitate. State whether the following species are being oxidized or reduced 59. Cr2+ Cr3+ 60. Cr Cr2O72Solve this redox reaction using half reaction method(acid) 61. CH4(g) + O2(g) CO2(g) + H2O(g) 66. The percent composition of a compound is 40.0% C, 6.7% H, and 53.7% O. The molecular mass of the compound is 180.0 g/mol. Find its empirical and molecular formulas. VOCAB: Avogadro’s number empirical formula percent composition molecular formula molarity CHEMISTRY I HONORS – 1st SEMESTER EXAM REVIEW – Fall 2010 ANSWER KEY 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 10.5% a. 3, b. 2, c. 4, d. 2 a. 5.48 × 105, b. 7.70 × 10-5, c. 0.001200, d. 92,500,000 1270 g a. 0.652 dm, b. 2,300 kg, c. 65 mL, d. 50,200 cm 1900 mL 8.7 hours slope = (mass) (volume) = density always record one estimate digit a. gas, b. plasma, c. solid , d. liquid Solution and colloid do not settle. Colloid and suspension are heterogeneous mixtures and scatter light. a. element, b. solution, c. compound, d. heterogeneous mixture a. physical, b. chemical, c. chemical, d. physical a. physical, b. chemical, c. chemical, d. chemical, e. physical a. Thomson, b. Millikan, c. Chadwick, d. Rutherford, e. Dalton Dalton’s billiard ball model-sphere of uniform density. Thomson’s plum pudding model-negative electrons dispersed in positive atom. Rutherford’s nuclear model-dense, positive nucleus surrounded by negative electrons. Bohr’s planetary model-electrons move in circular orbits in specific energy levels. Schrödinger’s electron cloud model-electrons move within orbitals not in specific orbits. (Chadwick then added neutrons to the nucleus.) 14 53 63 92 6 C, 24 Cr , 28 Ni, 40 Zr Zn Symbol Ca Se Ar 20 Atomic # 30 34 18 65 74 40 Mass # 41 34 # of protons 30 20 18 21 # of neutrons 35 40 22 18 # of electrons 30 20 34 1200 m 4.84 10-19 J Hydrogen atoms have specific energy levels. Therefore, the atoms can only gain or lose certain amounts of energy. When atoms lose energy, they emit photons which correspond to the lines in the emission spectrum. The more energy lost, the more energy the photon has. Bohr’s model stated that electrons circled the nucleus in fixed, circular paths called orbits. The modern model states that electrons move around the nucleus in orbitals where there is a probability of finding an electron. 23. F 9 V 23 24. In order to achieve greater stability, Cr moves one electron from the 4s-sublevel to the 3d-sublevel to make it half-full. 25. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. Pd At 46 85 [Kr] 5s24d8 [Xe] 6s24f145d106p5 26. Rb Te Rb+ Te2- Kr Xe [Ar] 4s23d104p6 [Kr] 5s24d105p6 Mendeleev arranged the elements in order of increasing atomic mass. Mosely arranged them by increasing atomic number. a. Ra, b. Xe a. Cl , b. Mg a. Li, b. As a. Si, b. W There are small jumps in 1st ionization energy when there is an element with increased stability (full or half-full sublevel). Removing the 4th electron from aluminum represents removing a core electron. 159.99 amu Na-24 = 0.62% and Na-23 = 99.38% -2.03525 amu 240Am 244Cf -3.04x10-10 J 22.93 kg a. ionic, b. polar, c. ionic, d. nonpolar a. metallic, b. ionic, c. metallic, d. covalent, e. ionic, f. covalent 44. 45. The lower the potential energy, the greater the stability. 46. a. CaBr2, b. Fe2(SO4)3, c. HF, d. SiO2, e. N2O4, f. H2SO3 47. a. chromium(III) chloride, b. copper(I) carbonate, c. arsenic pentachloride, d. magnesium sulfate, e. tetraphosphorous hexoxide, f. chloric acid. 48. nonpolar covalent – e- are shared equally, symmetrical orbital overlap, no separation of charge polar covalent – e- are shared unequally, lopsided overlap, partial charges ionic – e- are not shared, no overlap, complete charges 49. Electron pairs move as far apart from each other as possible in order to minimize repulsion. The number & type of electron pairs determines the bond angles and overall shape of the molecule. 50. 51. Number of valence e Lewis Diagram Counting e pairs Molecular Shape & Bond Angle(s) Molecular Polarity SiO2 1(4)+2(6)=16 2B, 0L linear, 180 nonpolar AsF5 1(5)+5(7)=40 5B, 0L trigonal bipyramidal, 120/90 nonpolar TeCl2 bent Te BCl3 Cl Cl Cl trigonal planar CH2Cl2 Cl C B Cl Cl H tetrahedral Cl H polar nonpolar polar nonpolar polar nonpolar 52. One unit of solid barium chlorate when heated produces one unit of solid barium chloride and three molecules of oxygen gas. 53. 54. 55. 56. 57. 58. 59. 60. 61. 62. 63. 64. 65. 66. 2NaCl(s) + 3O2(g) 2NaClO3(s) Cu(s) + MgSO4(aq) N.R. C5H12(l) + 8O2(g) 5CO2(g) + 6H2O(g) 2NH4Cl(aq) + Pb(NO3)2(aq) 2NH4NO3(aq) + PbCl2(s) 2Fe2O3(s) 4Fe(s) + 3O2(g) single replacement, combustion, double replacement, decomposition oxidized oxidized CH4(g) + 2O2(g) CO2(g) + 2H2O(g) 1.25 1023 molecules MgSO4 4.6M KNO3 12 g NaOH 47.27% Cu, 52.73% Cl empirical formula – CH2O, molecular formula – C6H12O6 I’m so proud of you! You survived a hard semester of Chem. Honors! See you next year!