are given in a character table having the point group on top left and the symmetry operations in the first row. H2O‚ SO2 The z axis coincides with the principal symmetry axis (C2 above) and the molecule (H2O‚ SO2) lies in the yz plane (σv’ above). NH3‚ CH3Cl CHEM 331 – 2014 Dr. Roland Roesler 8-1 Symmetry: Character Tables BF3‚ CO32ˉ 2C3 stands for C31 and C32. C33 = E. The first column provides a list of symmetry labels corresponding to irreducible representations: A and B indicate non-degenerate
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Chapter 1 Carbon Compounds and Chemical Bonds. (Covered material: 1.1 - 1.8; 1.12 - 1.17) 1. Structural Theory – most fundamental theory of Organic Chemistry (developed independently by A. Kekule‚ A. Couper and A. Butlerov between 1858 and 1861). Organic Compounds – compounds of carbon and hydrogen. Other elements frequently found in organic compounds are: oxygen‚ nitrogen and halogens (F‚ Cl‚ Br‚ I); less frequently found are: sulfur and phosphorus. Review Periodic Table for determining valence
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Thermochemistry IB questions 1. Ammonium nitrate‚ NH4NO3‚ dissolves readily in water according to the equation: NH4NO3(s) NH4+(aq) + NO3-(aq) H = 28kJ mol-1 Which of the following contribute(s) to the occurrence of this process? I. The system moves to lower enthalpy. II. The system becomes more disordered. a. I only b. II only c. Both I and II d. Neither I nor II 2. Which substance has the largest lattice energy? a. NaF b. KCl c. MgO d. CaS 3. A certain reaction is spontaneous
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Are you turning to the answers too soon? When you get stuck on a question do everything you can to answer it EXCEPT looking at the answer 1. Use your textbooks 2. Use your notes 3. Use the presentations 4. Use drop in 5. Use websites Don’t ever simply copy down an answer without knowing how to get there. BUT finally do check all your answers carefully here. You can also read the examiner’s report for each question.
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recommended for this topic (a) Reaction classes Only three reaction classes occur in (organic) chemistry‚ defined as: (i) Heterolytic – here one partner donates or departs with both electrons while the other (partner) supplies a vacant orbital. The reaction-energy diagram (profile) tends to have at least one intermediate. These reactions involve a “two-electron push”: Examples: (ii) Homolytic – here each partner supplies one electron as a radical (a species with a single unpaired electron)
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Atomic Structure and Bonding Section 3.3 Electron Configurations and Periodic Trends (pg. 139-157) Feb. 11 For single electron system all orbitals with the same value of have the same energy Atoms with more than 1 electron with the same value of n have different energies (sublevels) Because of interactions between additional electrons All orbitals within a sublevel have the same energy The Fourth Quantum Number: A property of the electron (spin quantum number: ms) Describes property of
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Alkyl Halides Alkyl halides are a class of compounds where a halogen atom or atoms are bound to an sp3 orbital of an alkyl group. CHCl3 (Chloroform: organic solvent) CF2Cl2 (Freon-12: refrigerant CFC) CF3CHClBr (Halothane: anesthetic) Halogen atoms are more electronegative than carbon atoms‚ and so the C-Hal bond is polarized. H H μ C + C-l δ δ H The C-X bond is polarized in such a way that there is partial positive charge on the carbon and partial negative charge on the halogen. Dipole moment
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consequences: • Atoms with one‚ two‚ three‚ or four valence electrons form one‚ two‚ three‚ or four bonds‚ respectively‚ in neutral molecules (e.g.‚ BF3‚ CH4). • Atoms with five or more valence electrons form enough bonds to give an octet (e.g.‚ NH3). This results in the following equation: 3 Lewis Structures Lewis structures are electron dot representations for molecules. General rules for drawing Lewis structures: 1. Draw only the valence electrons. 2. Give every second-row element no more
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CHEMISTRY 101 FINAL EXAM SECTIONS 572-580 Dr. Joy Heising FORM 4N December 7‚ 2001 Directions: 1. Fill out your scantron sheet. a. Do not forget to include your SIGNATURE and ID number. b. Dept = CHEM‚ Course No. = 101 c. If you want your scores posted‚ mark A under the option column 2. Use a #1 or #2 pencil for marking the answer sheets. circles completely. 3. DO NOT write on the envelope. 4. Read each question carefully‚ then choose the best answer for each question. There is no penalty
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must be doubly bonded to one of those molecules. For a double bond to form p-orbitals must overlap over a sigma bond. The hybridization loses one p-orbital‚ leaving the carbon as sp2‚ allowing the formation of the other bond with the free p-orbital‚ forming a pi-bond. Back to our question‚ why are the aldehyde and a ketone more reactive than an alkane. When the pi-bond forms the electrons in this molecular orbital are more exposed‚ making them more vulnerable to reacting. Try to visualize the
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