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Chemistry ~ Fall Final Review Please Note: Final is comprehensive over the first semester. Half multiple choice. Half free response. Bring a calculator & something to write with. You may bring a 4x6 note card w/ notes on both sides (MUST be handwritten) You will be expected to show all work, use correct significant figures and include proper units. Topics covered: Measurement: significant figures, sci. notation, guess digits, density Properties of Matter: atoms/molecules, elements & compounds, chemical/physical changes History of the atom: models & scientists Wave calculations: properties of waves, energy, frequency, wavelength Electron configuration: orbital diagrams, electron configuration, shorthand notation Periodic Table: metal, nonmetal; valence number; ion formation Naming: covalent, ionic type I, ionic type II, polyatomic ions Dimensional analysis: conversion factor, converting units Mole conversions: mass mol particles; % composition, empirical/molecular formulas Balancing DISCLAIMER: These problems include some possibilities for the test. Therefore, the answer to the question, “If I know everything on this sheet, am I guaranteed an A on the final?” is NO. For comprehensive review, you must study old test and quizzes, homework sets, corresponding sections of the text and class notes. 1. How many significant figures are in the following numbers: a) 10 000 b) 10.0 c) 5 432 009 000 d) 0.0087 e) 3.801 x 109 10 ml 2. Identify the following measurements. Be sure to include the correct significant figures and units. 9 ml 8 cm 7 3. Perform the following calculations. Include units and the correct significant figures. a) 3.265 cm + 8.4 cm b) 2.780 m x 3.4 m c) 8.9x1012 m2/ 3.56x1014 m 4. The density of iron is 7.80 g/cm3. What is the mass of a 0.892 cm3 sample? 5. Define physical and chemical change. 6. Define element, atom, compound, molecule, mixture, solution. 7. Explain how to determine the # of protons, neutrons and electrons from given information about atomic mass, atomic number, and the charge on the atom (ion). 8. Describe the models of the atom: Democritus, Dalton, Thomson, Rutherford, Bohr, Electron Cloud. 9. Use a diagram to define wavelength and frequency. Write the equations that relate wavelength & frequency and frequency & energy. What is “c”? What is “h”? 10. A beam of light has an energy of 2.34 x 10-18 J. Calculate its frequency and wavelength. 11. Define Hund’s rule, Pauli’s exclusion principle, Aufbau principle. Draw an orbital diagram for nitrogen. Indicate where each rule applies. 12. For each of the following atoms/ions provide: (1) electron configuration, (2) shorthand electron configuration, (3) number of valence electrons, (4) number of core electrons. a) boron b) selenium c) calcium d) O2e) Mg2+ 13. Provide the name or formula for the following: a) calcium chloride b) magnesium oxide d) iron (II) sulfide e) Al2O3 g) CCl4 h) SnO2 c) dinitrogen tetrafluoride f) Pb2O3 i) Na3PO4 14. What is a mole? Why do chemists use the mole? 15. How many atoms are in 5.0 mol of Al? (Use dimensional analysis/units/sig figs) 16. How many mol are in 9.0 g of water? 17. What is the mass of 1.3 x 1023 molecules of calcium sulfate? 18. Determine the % composition by mass of each element in glycerine C3H5(OH)3 19. Determine the molecular formula of a compound that is 87.5% nitrogen and 12.5% hydrogen by mass. The true molecular mass is 32.0 g/mol. 20. Balance the following chemical equations. a) ___ FeCl3(aq) + ___ KOH(aq) ___ Fe(OH)3(s) + ___ KCl(aq) b) ___ Pb(C2H3O2)2(aq) + ___ KI(aq) ___ PbI2(s) + ___ KC2H3O2(aq) c) ___ P4O10(s) + ___ H2O(l) ___ H3PO4(aq) d) ___ Li2O(s) + ___ H2O(l) ___ LiOH(aq) e) ___ MnO2(s) + ___ C(s) ___ Mn(s) + ___ CO2(g) f) ___ Sb(s) + ___ Cl2(g) ___ SbCl3(s) g) ___ CH4(g) + ___ H2O(g) ___ CO(g) + ___ H2(g) h) ___ FeS(s) + ___ HCl(aq) ___ FeCl2(aq) + ___ H2S(g) 1) a) 1 b) 3 2) a) 7.45 cm b) 9.20 ml 3) a) 11.7 cm b) 9.5 m2 4) 6.96 g c) 7 d) 2 e) 4 c) 0.025 m 5) physical change – alteration in the appearance, but not the identity of the substance chemical change – alteration of a substance into a new substance with new properties 6) atom – building blocks of matter element – simplest form of matter (made up of atoms) molecule – chemical combination of atoms compound – chemical comination of elements (made up of molecules) mixture – physical combination of 2 or more substances solution – homogeneous mixture where one substance is dissolved in another 7) atomic number EQUALS number of protons atomic mass – atomic number = number of neutrons atomic number – charge = number of electrons 8) defined the atom –“tiny” indivisible particle DEMOCRITUS ~ 400 B.C. Affirmed Democritus definition thru experimentation DALTON Early 1800’s Discovered electrons (e-) called them corpuscles THOMSON Late 1800’s - Plum Pudding Model / chocolate chip cookie model - Most of the mass of the atom is located in a small space, called the nucleus - The nucleus is positively charged - Atoms are mostly empty space - Electrons circle the nucleus RUTHERFORD 1910 Reformed Rutherford’s model; stated that the electrons followed fixed paths called orbitals, as they circled the nucleus BOHR 1913 Electrons can move b/w orbitals: gain energy move up level lose energy move down level (gives off light) Scientists who contributed to model: Plank, DeBroglie, Schrodinger, Einstein WAVE MODEL (electron cloud model) 1920’s – Today 9) f = 2 Hz E = h*f h = 6.626 x 10-34 c = *f 10) c = 3 x108 m/s 1 sec E = 2.34 x 10-18 J E = h*f f = E/h = 2.34 x 10-18 / 6.626 x 10-34 f = 3.53 x 1015 Hz c = *f 8.50 x 10-8 m c/f = 3 x108 / 3.53 x 1015 11) Hund’s rule – put one electron in each orbital per sub level before doubling up Pauli’s exclusion principle (simplified) – electrons have opposite spins Aufbau principle – fill lowest energy levels first N (Z=7) Hund 2p 2s Pauli Aufbau 1s 12) a) boron - 1s22s22p1; [He] 2s22p1; 3; 2 b) selenium - 1s22s22p63s23p64s23d104p4; [Ar] 4s23d104p4; 6; 28 c) calcium - 1s22s22p63s23p64s2; [Ar] 4s2; 2; 18 d) oxide - 1s22s22p6; [Ne]; 8; 2 e) magnesium - 1s22s22p6; [Ne]; 8; 2 13) a) CaCl2 b) MgO c) N2F4 d) FeS f) lead (III) oxide g) carbon tetrachloride i) sodium phosphate 14) mole = Avagadro’s number = 6.02 x 1023 e) aluminum oxide h) tin (IV) oxide This many atoms provides a useable amount in the lab. Also, allows chemists to measure the mass of elements in grams. 15) 5 mol Al * 6.02 x 1023 atoms Al = 3.0 x 1024 atoms Al 1 mol Al 16) 9.0 g H2O * 1 mol H2O = 0.5 mol H2O 18 g H2O 17) 1.3 x 1023 molecules CaSO4 * 1 mol CaSO4 6.02x1023 molecules CaSO4 * 136 g CaSO4 1 mol CaSO4 = 29 g CaSO4 18) C – 12 x 3 = 36 H–1x8 = 8 O = 16 x 3 = 48 + 92 C: 36 / 92 = 39% H: 8 / 92 = 9% O: 48 / 92 = 52% 19) N: 87.5% 87.5 g / 14 = 6.25 mol / 6.25 = 1 NH2 H: 12.5% 12.5 g / 1 = 12.5 mol / 6.25 = 2 32 / 14 = 2 20) MOLECULAR FORMULA N2H4 a) ___ FeCl3(aq) + 3 KOH(aq) ___ Fe(OH)3(s) + 3 KCl(aq) b) ___ Pb(C2H3O2)2(aq) + 2 KI(aq) ___ PbI2(s) + 2 KC2H3O2(aq) c) ___ P4O10(s) + 6 H2O(l) 4 H3PO4(aq) d) ___ Li2O(s) + ___ H2O(l) 2 LiOH(aq) e) ___ MnO2(s) + ___ C(s) ___ Mn(s) + ___ CO2(g) f) 2 Sb(s) + 3 Cl2(g) 2 SbCl3(s) g) ___ CH4(g) + ___ H2O(g) ___ CO(g) + 3 H2(g) h) ___ FeS(s) + 2 HCl(aq) ___ FeCl2(aq) + ___ H2S(g) BALANCED