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- Formula Lewis Electron Molecular Bond Polar or Attractive Structure Pair Geometry Angle Force Non Polar Geometry Between Molecules CH4 Around First C Around First C C2H4 Around First C Around First C C,H2 Around First C Around First C CH;OH Around O Around O C2H;OH Around O Around O CH20 CH,OCH, Around O Around O CH;COOH Central C Central C НСООН Central C Central C CH;NH2 Around N Around N CH;COCH; Central C Central Cindicate the approximate values for the indicated bond angles in the following molecules. 1 (a) H 0-N=ö 2. Н 4 H. (b) H C-c=0 H H H (c) H-N-O–H . H. (d) H-C-C=N: H.The structural formulas for ethanol, CH3CH2OH, and propene, CH;CH=CH,2, are нн H Н—С—С—0—н H-C-C=C-H нн H H H Ethanol Propene (a) Complete the Lewis structure for each molecule showing all valence electrons. (b) Using the VSEPR model, predict all bond angles in each molecule.
- For each of the following covalent bonds: (a) use the symbols δ+ and δ- to indicate the direction of polarity (if any).(a) C-F; (b) N-Br; (c) B-C; (d) Si-H(b) Rank the following covalent bonds in order of increasing polarity. (i) C-H, O-H, N-H; (ii) C-N, C-O, B-O; (iii) C-P, C-S, C-NIdentify the set of covalent bonds that shows the correct trend of increasing bond polarity. (A) H―F < H―Cl < H―Br < H―I; (B) H―C < H―N < H―O < H―F; (C) H―O < H―S < H―Se < H―Te; (D) H―C < H―Si < H―Ge < H―Sn;Identify the set that shows the correct trend in increasing polarity of covalent bonds: (A) B―F < C―F < C―Cl < N―Cl (B) C―F < C―Cl < N―Cl < B―F; (C) N―Cl < C―Cl < C―F < B―F; (D) C―Cl < N―Cl < B―F < C―F;
- 10. The following Lewis structures for (a) HCN, (b) C3H;, (c) SnOz, (d) BF3, (e)HOF are incorrect. Explain what is wrong with each one and give a correct structure for the molecule. (Relative positions of atoms are shown correctly.) (a) H-ëN (b) HCC-H (c) 0-Sn-0 (d) :F B :F: (e) H-O-F:Use the following table of bond energies to calculate the enthalpy of combustion (in kJ) of acetylene (C¿H2) gas in oxygen, based on the following chemical equation: C2H2(g) + 2.502(g) → 2CO2(g) + H;O(g) Single Bond H с N H 432 C 411 346 N 386 305 167 459 358 201 142 C=C 602 C=O 799 C=C 835 C=O 1072 Multiple kJ 1 2 3 4 5 6 C 7 8 +/- x 100 Tap here or pull up for additional resources LO2-Butanol can be made by the reaction of 1-butene and water: H2 C=CH-CH,–CH3 (g) + H2O(g) → CH; CH(OH)CH2CH3 (g) a Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Bond AH (kJ/mol) H-O 463 C=C 610 H-C 413 C-C 346 358 Enthalpy change = kJ b Calculate the enthalpy change for this reaction from enthalpies of formation. Substance AƒH (kJ/mol) CH3 CH(OH)CH2 CH3 (g) -293.1 H2O(g) -241.83 H2C=CH-CH2–CH3 (g) -0.1300 Enthalpy change = kJ
- Which of the following organic molecule has the highest formal charge? :ö=ö-ö: CH3-N-CH3 CH3-0 • CH3-N=C:b) Which are polar molecules? ÇI Ö=c=Ö H CH, CH, CH; H,C CH2 CH2 :0. ÇI `H HEthylene, C₂H₄, and tetrafluoroethylene, C₂F₄, are used tomake the polymers polyethylene and polytetrafluoroethylene(Teflon), respectively.(a) Draw the Lewis structures for C₂H₄ and C₂F₄, and give theideal H-C-H and F-C-F bond angles.(b) The actual H-C-H and F-C-F bond angles are 117.4and 112.4, respectively. Explain these deviations.