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Electron Configuration and Orbital Filling

Orbitals

Ethmoid Orbital Plate

Lecture 4 Orbital Vasculature

Molecular orbital theoryZ

4.3 The quantum mechanical theory and the orbital

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals

Part II. Multiple choice, continued (3 points each). Name:__________________ Please circle your answer. There is only one correct answer to each question. 43. The F-N-F bond angle in the NF3 molecule is slightly less than ___________. A) 90˚ B) 109.5 ˚ C) 120˚ D) 180˚ 44. The angles between sp2 orbitals are _____________. A) 90˚ B) 109.5˚ C) 120˚ D) 180˚ 45. The blending of one s atomic orbital and two p atomic orbitals produces __________. A) three sp hybrid orbitals B) three sp2 hybrid orbitals C) three sp3 hybrid orbitals D) two sp3 hybrid orbitals 46. The π bond in ethylene, CH2CH2, results from the overlap of ___________. A) sp3 hybrid orbitals B) s atomic orbitals C) sp2 hybrid orbitals D) p atomic orbitals 47. The amount of gas that occupies 60.82 L at 31˚ C and 367 mm Hg is _________ mol. A) 1.18 B) 0.850 C) 894 D) 11.6 48. The specific heat of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 ˚C to 37 ˚C? A) 7.8 B) 1.9 C) 19 D) 29 49. Which one of the following is a weak acid? A) HNO3 B) HI C) HF D) HClO4 50. Which combination will produce a precipitate? A) NH4OH (aq) and HCl (aq) B) AgNO3 (aq) and Ca(C2H3O2)2 (aq) C) NaCl(aq) and HC2H3O2 (aq) D) NaOH (aq) and Fe(NO3)2 (aq) 51. The density of chlorine (Cl2) gas at 25 ˚C and 450 torr is _______ g/L. A) 20 B) 4.9 C) 1.7 D) 0.86

Part II. Multiple choice, continued (3 points each). Name:__________________ Please circle your answer. There is only one correct answer to each question. 27. What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl? A) 13.1 B) 0.24 C) 14.3 D) 6.55 28. All of the orbitals in a given electron shell have the same value of the ___________ quantum number. A) principal B) azimuthal C) magnetic D) spin 29. The places where the value of Y2 is zero are called ___________. A) orbitals B) nodes C) orbits D) wave functions 30. Of the following elements, which has the largest first ionization energy? A) B B) N C) P D) Si 31. Which equation correctly represents the second ionization of phosphorous? A) P+(g) + e- à P2+(g) B) P(g) à P+(g) + e- C) P+(g) à P2+(g) + e- D) P-(g) + e- à P2-(g) 32. Which of the following does not have eight valence electrons? A) Rb+ B) Ca+ C) Xe D) Br- 33. Of the atoms below, ____________ is the least electronegative. A) Cl B) Si C) F D) Rb 34. Of the bonds below, __________ is the least polar. A) Na - S B) P - S C) Na - Cl D) Si - Cl 35. In the Lewis structure of ClF, the formal charge on Cl is ______ and the formal charge on F is ________. A) –1, -1 B) 0, -1 C) 0, 0 D) +1, -1

Part II. Multiple choice, continued (3 points each). Name:__________________ Please circle your answer. There is only one correct answer to each question. 14. Which of the following compounds would you expect to be ionic? A) SF6 B) H2O C) H2O2 D) CaO 15. Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) à 2NH3 (g) A 9.3-g sample of H2 requires ____________ g of N2 for a complete reaction. A) 43 B) 1.3 x 102 C) 3.9 x 102 D) 4.6 16. What is the frequency of light (s-1) that has a wavelength of 1.23 x 10-6 cm? A) 3.69 B) 2.44 x 1016 C) 4.10 x 10-17 D) 9.62 x 1012 17. Which sketch represents an orbital with the quantum numbers n = 3, l = 1, ml = 0? A) B) C) D) 18. What color of visible light has the longest wavelength? A) blue B) violet C) red D) yellow 19. According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the __________ of an electron. A) mass B) color C) momentum D) shape 20. The wavelength of a photon that has an energy of 5.25 x 10-19 J is ___________ m. A) 3.79 x 10-7 B) 2.64 x 106 C) 2.38 x 1023 D) 3.79 x 107 21. There are ___________ orbitals in the second shell. A) 2 B) 4 C) 9 D) 18

electron orbital energy levels

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Lecture 11 - Molecular Orbital Theory