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(5 Points) State Which of the Following Sets of Quantum Numbers Would Be Possible and Which Would Not

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(5 Points) State Which of the Following Sets of Quantum Numbers Would Be Possible and Which Would Not 1. (5 points) State which of the following sets of quantum numbers would be possible and which would not. Using one sentence, explain what is wrong with the quantum numbers that are not possible. a) n = 4, l = 4, ml = 4, ms =1/2 b) n =4, l = 3, ml = 2, ms = 1/2 c) n = 4, l =5, ml = 0, ms = -1/2 d) n = 4, l = -2, ml = 0, ms = -1/2 e) n = 4, l = 3, ml = 5, ms = -1/2 Page 1 2. (8 points) )Which of electron configuration represents a violation of auf bau, Hund’s rule, and/or the Pauli principle? Explain briefly your choices. 1s 2s 2p a ↑↓ ↑↓ ↑ ↑ ↓ b ↑↓ ↑↓ ↑↓ ↑ c ↑↓ ↑↓ ↓ ↓ ↓ d ↑ ↑↓ ↑↓ ↑↓ e ↑↓ ↑↓ ↑ ↑ ↑ Give the set of quantum numbers for each of the electrons in the p orbitals in orbital diagram (a) 3. (2 points) How many angular nodes does an 12f orbital have? How many radial nodes does a 7p orbital have? Page 2 4. Name the element with the following electron configuration: [a] 1s22s22p63s23p2 [b] 1s22s22p63s23p63d 104s24p64d 105s25p5 [c] [Ar]4s13d 5 [d] [Xe]4f146s2 5. (4 points) Using the periodic table write the expected ground state electron configurations for a) The third element in Group-4A b) Element number 114 (yes even if it doesn't yet exist) c) The elements with two unpaired 3d electrons. d) The halogen with electrons in the 6p atomic orbitals. Page 3 6. (8 points) Determine which of the following statements are true and explain why or why not based on shielding effects, quantum shielding, and/or Zeff. a) Ionization energies increase down a group b) The ionization energy of an cation is larger than that of the parent atom. c) The sodium ion is smaller than the potassium ion d) The fluoride anion is smaller than the fluorine atom Page 4 7. Penetration is the process by which an outer electron moves through the region occupied by the core electrons to spend part of its time closer to the nucleus. Penetration and the resulting effects on shielding cause an energy level to spit into sublevels of differing energy. Use the penetration effect to explain the difference in relative orbital energies of a 2s and a 2p electron in the same atom. 8. The first ionization energy of the chlorine atom is 1251 kJ/mol. Which of the following values would be a more likely ionization energy for the iodine atom: 1000 kJ/mol or 1400 kJ/ mol. Explain your reasoning based on periodic trends AND Zeff. Page 5 9. Little is known about the properties of astatine, At because of its rarity and high radioactivity. Nevertheless, it is possible for us to make many predictions about its properties. Do you expect the element to a gas, a liquid or a solid at room temperature? Explain. What is the formula for the compound that forms when astatine reacts with sodium metal? 10. Answer the following questions clearly. Please explain your choice.: a) Of the elements S, Se, Cl, which one has the largest radius? b) Which is larger, the chlorine atom or the chlorine ion? c) Which has the largest ionization potential, N, P, or As? d) Which has the largest radius, O2–, N3–, F–? e) Which one of the following ions would you expect to have the smallest radius? Cr6+, P3-, Cl–, K+, or Ti4+ Page 6 11. (a) Explain the following trend in Lattice energy based on ion size and the definition of lattice energy: BeH2 3205 kJ/mol MgH2 2791 kJ/mol CaH2 2410 kJ/mol SrH2 2250 kJ/mol BaH2 2121 kJ/mol (b) The lattice energy of ZnH2 is 2870 kJ/mol. Based on the data given in part a, the radius of the zinc ion is expected to be closest to that of which group 2A element? Use a complete sentence to explain your choice. 12. Using electronegativity values, predict which bond in the following groups will be most polar. Show your work. a) C—H, Si—H, P—H b)Al—Br, Ga—Br, In—Br, Tl—Br Page 7 13. Determine which of the structures listed below would be the most plausible structure based on formal charges. • Show the calculations for formal charges • Explain your choice in one or two sentences based on formal charge, elecronegativity, size, etc. C N O N C O C O N 14. Write the resonance structures (using the best formal charge model) for – ClO2 , chlorite. Show all formal charges. Page 8 15. Draw the lewis structure for SeCl4. 16. The space shuttle orbiter utilizes the oxidation of methyl hydrazine by dinitrogen tetroxide. Use bond energies to estimate the !H for the reaction below. 5N2O4(l) + 4 N2H3CH3(l) → 12 H2O(g) + 9 N2(g) + 4CO2(g) O O H H N N N N O O H CH3 dinitrogen tetroxide methyl hydrazine Page 9 17. Write the best (formal charges, octet rule etc) Lewis structure for SO2Cl2. What is the molecular and electron pair geometry? What type of hybridized orbitals are needed for this molecule? Will it have the same molecular and electron pair geometry as OCl2? Justify your answer by comparing Lewis structures. Is this a polar molecule? why? c) Show the complete hybridization process for the oxygen in oxygen dichloride. Clearly label what the electrons are used for (bonding, lone pair) in the hybridization scheme. You do not have to show chlorine in the scheme. Page 10 18. The structures below show the stick and ball drawing of three possible shapes of an AF4 molecule. A is the general symbol for the central atom. The terminal atoms are fluorine. The lone pairs are not shown. a) Identify the molecular geometry for each of the shapes. b) For each shape, give VSEPR (electron pair or electron domain) geometry on which the molecular geometry is based. c) For each shape, how many lone pairs are there on atom A? d) For each shape, what are approximate bond angles? A B C Page 11 19. When two or more compounds have the same composition but a different arrangement of atoms (or geometries), we call them isomers. Isomers are composed of the same collection of atoms, but they differ in one or more chemical or physical property. There are several types of isomers found in chemistry. In a geometric isomer, the bonds are the same, but the orientation or arrangement of the bonds is different. PF2Cl3 has three geometric isomers. One of these isomers has a dipole of zero; two do not. (a) Draw the geometric isomers of PF2Cl3 using VSEPR. Clearly show the three dimensionality of each molecule. (Please label your drawings) (b) State which of the three molecules in part (a) has no dipole. (c) Explain BRIEFLY why your choice has no dipole. Page 12 20. (5 points) Using the valence orbital diagram (box diagram), show how the — atomic orbitals of the central atom in IF4 leads to the appropriate hybrid orbitals. Fill the hybrids with the correct number of electrons please. Page 13 – 21. The azide, N3 molecule is linear with two N—N bonds of equal length, 1.16Å. a) Draw the best Lewis structure for the azide ion, showing formal charges. b) Using VBT, what hybridization scheme would you expect at each nitrogen in the azide molecule to have? (Describe theVSEPR geometry, show hybridized orbitals containing electrons, link these orbitals to make bonds and sketch the molecule showing the sigma bonds and " bonds for full points.) Page 14 22. What factor accounts for each of the following differences in bond length? a) I2 has a longer bond than F2. b) N—F is shorter than N—Br. c) N—N is longer than N≡N — 23. Consider the molecules H2 and He2 and the ion H2 . (a)Sketch the molecular orbitals of these two molecules. (b)How many electrons are there in each species? c)What is the bond order for each species? d)Now consider the ions HeH— and He+. Which one is more stable? Page 15 24. A chloride of antimony is a solid at room temperature, but vaporizes when heated. When 2.359 g of this compound are vaporized in an evaluated 1.00 L chamber at 581K, the pressure in the bulb is 376 mmHg. What is the molecular weight of this chloride of antimony, assuming the vapor is an ideal gas? 25. Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I2(s) + 5 F2(g) → 2 IF5(g). A 5.00 -L flask is charged with 10.0 g of F2(g) and 10.0 g of I2(s) . The reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. What is the partial pressure of the IF5 in the flask? What is the mole fraction of IF5 in the flask? Page 16 26. Assume that a single cylinder of an automobile engine has a volume of 600.0 cm 3. If the cylinder is full of air at 80°C and 0.980 atm, how many moles of O2 are present? The mole percent of oxygen in air is 20.95 %. How many grams of Octane (C8H18) could be combusted by this quantity of O2, assuming complete combustion with the formation of CO2 and H2O? 27. Two gases in adjoining vessels were brought into contact by opening a stopcock between them. The one vessel measured 0.250 L and contained NO at 800.0 torr and 220.00K. The other measure 0.100L and contained oxygen at 600.0 torr and 220.00K.
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