How are the molecules or ions in each pair related? Classify them as resonance structures, isomers, or neither. CH3 a. CH,-Ö-CH,CH, and C. and b. and CH3-C=C-CH3 d. CH;CH,CH3 CH,CH,ČH2 and нн
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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 CThe Structure of Hydrocarbons 1. Draw the four carbon bonding patterns commonly seen in hydrocarbons and all other organic compounds. Construct the Lewis structures of the following compounds by combining the carbon atoms with the appropriate bonding patterns and the required number of hydrogen atoms. 2. a. hexane: CH,CH,CH,CH,CH,CH, b. 3-hexene: CH,CH,CH=CHCH,CH, c. 2-hexyne: CH,C=CCH,CH,CH, 3. There are three distinct bond angles formed in the four bonding patterns of carbon. What are they and in which bonding pattern(s) is each seen?How are the molecules or ions in each pair related? Classify them as resonance structures, isomers, or neither. OH
- b. There is one additional resonance structure. NH₂ c. There is a total of five resonance structures (including the original structure). : OH4. The following are valid Lewis structures for CH3SOCH3. Label the formal charges and circle the best Lewis structure. H :ö: H H :0 H a) H-C=S-C-H b) Н—С—S— С-н H. H. H. H. Н :0: Н H :ö: H d) H-C=$-C-H c) Н—С—$—С-н H. H. H H2-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
- 8) Fill in the blanks with the appropriate structures. Na,Cr,0, NH,OH.HCI H,SO, NaOAc heat8. Use bond energies as found in Table 9.1 of Tro, Fridgen and Shaw and estimate the energy change A H (in kJ/mol) for the following reaction:lowing reaction: H-C= C-H +2 HI →CH3-CHI ₂ The C-I bond energy is 213 kJ/mol.Calculate the Enthalpy Change (ΔH) from average bond energies, which have been listed below in KJ/mol, for the following reaction and identify the nature of the reaction: CH3COOH + CH3OH → CH3COOCH3 + H2O [C‒H: 413; C‒C: 347; C=O: 745; C=C: 614; Cl‒Cl: 239, C‒O: 358; O‒H: 467]
- H 4 H. H:Y:H H The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group (red). | bond(s) In this representation, each Y atom needs with atoms of H. |electron(s) to complete its octet, and gains these electrons by forming unshared electron pair(s) and |bonding electron pair(s) in the product molecule. There are The bonds in the product are|Assign formal charges to each carbon atom in the given species. All lone pairs have been drawn in. нн a. CH2=CH b. н-с-н с. Н-с-н d. H-Ć-Č нн H e. f. N=N=N: g h. or -N=Q:37) Use bond energies to calculate the enthalpy changes for the formation of ethane (C;H6) from ethylene (C3Ha) and hydrogen (H2). Bond energies: H'(kJ/mol): (C-H): 413, (C-C): 614, (C-C): 348, (H-H): 446. Is the reaction endo or exothermic ? H H H-c-C-H C=c H-H H H a) - 114 b) + 114 c) - 230 d) +330