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PAP Chemistry - Fall Final Review Chapter 1 (Matter) & 2 (Measurements) 1. Know the rules for significant figures (what’s significant and what’s not) 2. Be able to determine the number of significant figures present in a given number a. 0.00203 3 b. 123 3 c. 100 1 d. 100. 3 e. 100.050 6 Chapter 3 (Atoms) 3. Understand and apply the Law of Conservation of Mass 4. Understand the Law of Multiple Proportions 5. Define atom, nucleus, electron, neutron, proton (including relative size and charge of subatomic particles) 6. What did Rutherford discover from the Gold Foil Experiment – p.72 The nucleus and that the atom was mostly empty space 7. When is a bright-line spectrum produced by an atom? IE – How does an atom give off color (especially when burned)? The resting state or the ground state is when the electron is closest to the nucleus. It will jump to outer levels gaining energy and this is called the excited state. When the electron falls or drops back to the ground state, it will lose energy in the form of light. When burned, the heat is the energy lost or given off. 8. Use the mass number and atomic number to determine the element and its number of protons, electrons, and neutrons 9. Be able to determine the atomic number and mass number of an element when the number of protons, neutrons, and electrons is specified 10. How does mass number relate to number of protons when talking about isotopes? The number of protons does not change. An isotope is the different mass numbers for the same element. 11. What is Avogadro’s Number? 6.02 X 1023 12. How many atoms are in 1 mole of each element? 6.02 X 1023 Does this number change? No, since the equation is 1 mole = 6.02 X 1023 atoms 13. Be able to do mol-mass conversions 14. Determine the number of protons, electrons, and neutrons in the following isotopes: An isotope only deals with the different mass of the same element. The equation is mass = protons + neutrons. The number of protons will always equal the atomic number. If it is a neutral atom or an isotope, the number of protons and electrons are equal. The number of electrons changes if we are talking about an ion. a. sodium-23 protons = 11, neutrons = 12, electrons = 11 b. calcium-40 protons = 20, neutrons = 20, electrons = 20 c. Cu protons = 29, neutrons = 35, electrons = 29 d. Ag protons = 47, neutrons = 61, electrons = 47 15. Determine the mass in grams of the following: a. 2.00 mol N 2.00 mol N2 | 28.014 g N2 = 56.0 g N2 | 1 mol N2 b. 3.01 x 1023 atoms Cl 3.01 x 1023 atoms Cl2 | 1 mol Cl2 | 70.905 g Cl2 = 3.55 x 101 g Cl2 or 35.5 g 23 | 6.02 x 10 atoms Cl2 | 16. Determine the amount of moles of the following: a. 12.15 g Mg 12.15 g Mg | 1 mol Mg = .4999 mol Mg | 24.305 g Mg b. 1.50 x 1023 atoms F 1.50 x 1023 atoms F2 | 1 mol F2 | 37.996 g F2 = 9.47 g F2 | 6.02 x 1023 atoms F2 | 1 mol F2 17. Determine the number of atoms present in a 251.2 g sample of manganese. 251.2 g Mn | 6.02 x 1023 atoms Mn = 2.74 x 10 24 atoms Mn | 54.938 g Mn Chapters 4 (Electrons in Atoms) & 5 (Periodic Law) 19. How many electrons are held is each quantum sublevel (s = 2, p = 6, d = 10, f = 14) 20. Write electron configurations and orbital filling diagrams (including energy level, sublevels, and orbitals for any element) Example: chlorine Electron configuration: 1s2 2s2 2p6 3s2 3p5 Orbital notation: ↑↓ 1s ↑↓ 2s ↑↓ ↑↓ ↑↓ ↑↓ 3s ↑↓ ↑↓ ↑ . 2p 3p 21. Be able to locate the alkaline earth, alkali metals, noble gases, and halogens 22. Periodic Trends – know atomic radius and electronegatitivity and how they compare IE = increase across, decrease down ( , ) EA = increase across, decrease down ( , ) EN = increase across, decrease down ( , ) AR = decrease across, increase down ( , ) IR = decrease across, increase down ( , ) SHIELDING = remains constant across, increases down ( constant , ) 23. What is the octet rule? What orbitals must be filled for it to be satisified? There must be 8 electrons in the outermost shell, orbital. The “s” and “p” orbitals, 24. How is the periodic table organized (atomic number, atomic mass) By increasing atomic number. 25. Define periodic law and why is it important? 26. What is the general electron configuration for a noble gas? (s, p, d, f) Example: noble gas configuration for strontium [ Kr ] 5s2 27. Write the electron configuration for the following a. carbon 1s2 2s2 2p2 b. neon 1s2 2s2 2p6 c. sulfur 1s2 2s2 2p6 3s2 3p4 d. potassium 1s2 2s2 2p6 3s2 3p6 4s1 e. vanadium 1s2 2s2 2p6 3s2 3p6 4s2 3d3 Chapter 7 (Formulas and Compounds) 39. Be able to name compounds a. Pb3(PO4)2 lead II phosphate b. NaF sodium fluoride c. C2O dicarbon monoxide d. H2SO4 sulfuric acid e. HF hydrofluoric acid 40. Be able to convert between gramsmolesatoms. a. How many grams of Al2S3 are in 2.00 moles of Al2S3? 2.00 mol Al2S3 | 150.162 g Al2S3 = 300. g Al2S3 | 1 mol Al2S3 b. How many atoms are found in 1.00 moles of Na? 1.00 mol Na | 6.02 x1023 atoms Na | 1 mol Na = 6.02 x 1023 atoms Na c. How many Na+ ions are found in 1.00 moles of NaF? OMIT 41. In a compound, the sum of all the oxidation number of the atoms must equal? zero 42. In an ion, the sum of all of the oxidation numbers of the atoms must equal? The charge on the ion. 43. What is the oxidation number of C in CO2? CO2 oxygen has a -2 charge so multiple it by its subscript . -4 = 0 What number does it take to add to -4 to get zero? +4 +4 -4 = 0 44. What is the oxidation number of P in PO43PO4-3 the -3 is the charge of the polyatomic ion so the whole formula must equal a -3 PO4 oxygen has a -2 charge so multiple it by its subscript . - 8 = -3 phosphorus need a +5 in order for the equation to +5 - 8 = -3 produce a -3 45. What is % composition? % composition = part x 100 whole 46. Determine the % composition of NaCl. % composition = Na wt x 100 Na wt + Cl wt = 22.990 x 100 22.990 + 35.453 47. Determine the % composition of magnesium hydroxide. % composition = Mg wt Mg wt + (O wt x 2) + (H wt x 2) = = % composition = = 24.305 24.305 + 31.998 + 2.016 x 100 x 100 41.676% Mg (O wt x 2) Mg wt + (O wt x 2) + (H wt x 2) 31.998 24.305 + 31.998 + 2.016 x 100 x 100 = % composition = = 54.867% O (H wt x 2) Mg wt + (O wt x 2) + (H wt x 2) 2.016 24.305 + 31.998 + 2.016 x 100 x 100 = 3.457% H 48. What is empirical and molecular formula? Empirical – a formula with the subscripts in the lowest terms Molecular – a formula that is a multiple of the empirical formula 49. Be able to determine the empirical formula. a. What is the empirical formula for a compound that is found to contain 63.52% iron and 36.48% sulfur? (If given the number as a percent, you divide the % number by the weight of the element. If the given number is in grams, you convert to moles) Step 1 : divide to get a number .6352 Fe = .01137 55.845 .3648 S = .01137 32.066 Step 2: divide each number above by the smallest number .01137 = 1 .01137 .01137 = 1 .01137 Step 3: these numbers are the subscripts for the elements. So, the empirical formula is: FeS 50. Given the empirical formula and a molar mass, be able to determine the molecular formula. a. The empirical formula is CH5. Its formula mass is 85.0 g/mol. What is the molecular formula? (Since you are already given the empirical formula, you just have to do the step to calculate the molecular formula. The equation you use is the “me” equation: molecular wt = a # that is the multiplier empirical wt 85.0 Wt of C + (5 x wt of H) 85.0 17.051 = = 4.98 = round this to 5 So, the take the 5 and multiply each subscript by it. The molecular formula is C5H25 Chapter 8 (Rxns) 51. What is a precipitate? A solid in a liquid solution 52. When is a chemical equation balanced? When it follows the Law of Conservation: the same number of each atom on both sides of the arrow. 53. What is a subscript? # of atoms What is a coefficient? # of mol Where are the products and reactants located in a chemical reaction? 54. Be able to balance chemical equations. a. Al4C3 + H2O CH4 + Al(OH)3 Al4C3 + 12H2O 3CH4 + 4Al(OH)3 55. Be able to recognize a synthesis reaction, a single replacement reaction, a double replacement reaction, and a decomposition reaction. 56. When a double replacement reaction produces a precipitate, what happened? It is insoluble. 57. What products are formed when Lithium metal reacts with water? Li(s) + H2O(L) → H2(g) + LiOH(aq) 58. What is the activity series of metals? What does it indicate about the loss or gain of electrons? It tells which elements can or cannot replace which in a single replacement reaction. Those elements that can lose few electrons are higher on the activity series so they Are stronger and can replace other easier. 59. Given solubility rules, be able to determine what products will form precipitates (see the lab that took forever)