*[m課程名稱︰普通化學丙 課程性質︰必修 課程教師︰林英智 開課學院：工學院 開課系所︰機械系 考試日期（年月日）︰2011.03.31 考試時限（分鐘）：100 mins 是否需發放獎勵金：是 謝謝 *[1;33m（如未明確表示，則不予發放）*[m 試題 : 1. In a cubic closest packing (face-centered cubic) system of atom A, if all the octahedral holes are suitably filled with atom B, (1) what is the radius ratio (Ra:Rb) of the packing atom and the atom B.(4%) (2) What it the percentage of the total space filled by atoms A and B.(6%) 2. For a gas particle, the average velocity Uavg is given by (8RT/πM)^(1/2). The collision frequency between particles with a diameter of d is determined by the number of particles in the volume πd^2 x Uavg created by the movement of the particle. The factor of 2^(1/2) is also used to consider the relative velocity (collisions in various directions) between particles. Assume that the diameeter d of an O2 molecule is 300pm. (1) Write the equation for collision frequncy.(4%) (2)Calculate the collision frequency for an oxygen molecule in a sample of pure oxygen at 200K and 0.0001atm.(6%) 3. Non-ideal gas equation (van der Waal equation: [P+a(n/V)^2](V-nb) = nRT) could properly describe the behavior of CO2 with constants: a = 3.59 atmL^2/mol^2 ; b = 0.0427 L/mol. If a high pressure storage tank with a volume of 10L is filled with 50 moles of CO2 at 27°C, (1) what is the pressure calculated by the ideal gas law (5%) and (2) what is the pressure calculated by the van der Waal equation? (5%) 4. The electronic configuation for K is (1s)2 (2s,2p)8 (3s,3p)8 (4s)1. (1) Give the nuclear charge.(3%) (2) Considering the shielding effect of the internal electrons in 1s,2s,2p,3s,3p, calculate the effective nuclear charge for the electron at 4s orbital.(3%) (3) Also calculate the effective nuclear charge for the electron at 3p orbital.(4%) 5. Sodium chloride can be viewed as a cubic closest packing of chloride anion filled with sodium cation into all octahedral holes with the separation of one Na-Cl pair being d. The lattice energy of NaCl crystal can be calculated by considering the energy of attractive and repulsive force. The Madelung constant takes into account this concept of the attractive and repulsive forces. Give the first four terms for the Madelung constant.(10%) 6. Molecular orbital theory, where the molecular orbitals are made of linear combinations of atomic orbitals, is used to explain the paramagnetic property of O2. (1) Draw energy diagram of atomic and molecular orbitals of O2.(4%) (2) Draw shapes of three molecular orbitals (2π and one σ bonds) made of linear combinations of 2Px, 2Py and 2Pz.(3%) (3) Fill in electrons to explain the paramagnetic property of O2.(3%) 7. Using double quartet (two quartet makes an octet) to explain (1) the paramagnetic property of O2 (5%) (2) the equivalence of all six carbon-carbon bonds in benzene, each with a bond order of 1.5.(5%) Multiple choice: (2% / Question) 1. Consider three identical flasks filled with different gases. Flask A: CO at 760 torr and 0°C Flask B: N2 at 250 torr and 0°C Flask C: H2 at 100 torr and 0°C In which flask will the molecules have the greatest average kinetic energy? (A) Flask A (B) Flask B (C) Flask C (D) the same 2. We have three ways of describe a typical velocity for the particles in an ideal gas: the root mean square velocity (Urms), the most probable velocity to explain the paramagnetic property of O2.(3%) 7. Using double quartet (two quartet makes an octet) to explain (1) the paramagnetic property of O2 (5%) (2) the equivalence of all six carbon-carbon bonds in benzene, each with a bond order of 1.5.(5%) Multiple choice: (2% / Question) 1. Consider three identical flasks filled with different gases. Flask A: CO at 760 torr and 0°C Flask B: N2 at 250 torr and 0°C Flask C: H2 at 100 torr and 0°C In which flask will the molecules have the greatest average kinetic energy? (A) Flask A (B) Flask B (C) Flask C (D) the same 2. We have three ways of describe a typical velocity for the particles in an ideal gas: the root mean square velocity (Urms), the most probable velocity (Ump), and the average velocity (Uavg). In order of increasing velocity. (A) Urms < Ump < Uavg (B) Ump < Uavg < Urms (C) Urms < Uavg < Ump (D) the same 3. Consider separate 1.0-L gaseous samples of He, CH4, Ar all at STP. Rank the gases in order of increasing average velocity. (A) Ar < Ne < CH4 < He (B) Ar < He < CH4 < Ne (C) CH4 < Ar < Ne < He (D) He < CH4 < Ne < Ar 4. An electron is excited from the ground state to the n = 3 state in a hydrogen atom. Which of the following statement is true? (A) It takes more energy to ionize (remove) the electron from n = 3 than from ground state. (B) The electron if farther from the nucleus on average in the ground state than in the n = 3. (C) The wavelength of light emitted if the electron drops from n = 3 to n = 2 is shorter than the wavelength of light emitted if the electron falls from n = 3 to n = 1. (D) The wavelength of light emitted when the electron returns to the ground state from n = 3 is the same as the wavelength of light absorbed to go from n = 1 to n = 3. 5. Arrange the following groups of atoms and ions in order of decreasing size. Which of following groups are false? (A) Ca < Mg < Be (B) Te < I < Xe (C) F < N < As (D) S < Cl < F 6. For each of the following groups, place the atoms and ions in order of decreasing size. Which of following groups are false? (A) Cu > Cu + > Cu 2+ (B) Pt 2+ > Pd 2+ > Ni 2+ (C) O - > O 2- > O 7. Which bonds in the following groups is the most polar? (A) Al-Br (B) Ga-Br (C) In-Br (D) Tl-Br 8. To predict the order of electronegativity in each of following groups of elements. Which of following groups are false? (A) C < N < O (B) Cl < Se < S (C) Rb < K < Na (D) Tl < Ge < S 9. Give the expected hybridization of the central atom for the molecules or ions Which of following one is false? (A) NH4 +: N is sp2 hybridized (B) PH3: P is sp3 hybridized (C) HCN: C is sp hybridized (D) CHCl3: C is sp3 hybridized. 10. Give the numerical values of n and l corresponding to 5d, and what is the maximum number of electrons that can occupy of the 5d subshell? (A) n = 5, l = 1, e- = 6 (B) n = 2, l = 15, e- = 10 (C) n = 5, l = 2, e- = 10 (D) n = 5, l = 3, 2- = 14 11. If the core electrons were totally effective at shielding the valence electron from the full charge of the nucleus and the valence electrons provided no shielding for each other, what would be the values of S and Zeff for a 3p electron in a sulfer atom? [Zeff = Z - S] (A) 6 (B) 10 (C) 12 (D) 16 12. Draw the molecular geometries for each of the following molecules or ions and predict their molecular geometries. Which molecular geometries of following molecules of ions are false? (A) PF3, trigonal pyramidal (B) HCN, linear (C) SO3 2-, trigonal planar (D) SF4, seesaw 13. Give the electron configuration of these ions, which of following electron configuration is wrong? (A) Na+ 1s2 2s2 2p6 (B) O- 1s2 2s2 2p5 (C) Cl 1s2 2s2 2p6 3s1 3p6 (D) Ca 1s2 2s2 2p6 3s2 3p6 4s2 14. Which member of the following pairs of compounds has the highest boiling point? (A) HF (B) HBr (C) CH4 (D) H2Se 15. Which of these are correct Lewis structures? ‥ (A) ：Ｎ══Ｎ： (B) ┌　　　Ｈ　　　┐＋　(C) ┌ ‥　　‥　　‥ ┐－ 　　 　　 　　　　　　　　│　　　│　　　│ │：Ｏ──Ｎ══Ｏ：│ 　　 　　 　　　　　　　　│　　　│　　　│ └ ‥　　　　　　 ┘ │Ｈ──Ｎ──Ｈ│ │　　　│　　　│ 　　　 　　　　　　　　　│　　　│　　　│ 　　　 　　　　　　　　　└　　　Ｈ　　　┘ (D) ‥ ：Ｏ： │ ‥ │ ‥ ：CL──Ｃ──Cl： ‥ ‥ ‥ --

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