Concept explainers
(a)
Interpretation:
The aromatic cyclopolyenes with a single positive charge are to be predicted.
Concept introduction:
The movement of delocalized pi electrons leads to the corresponding resonance structures. The stability of a compound depends upon the number of resonating structures. The compounds which follow the
(b)
Interpretation:
The aromatic cyclopolyenes with double positive charge are to be predicted.
Concept introduction:
The movement of delocalized pi electrons leads to the corresponding resonance structures. The stability of a compound depends upon the number of resonating structures. The compounds which follow the Huckel rule of aromaticity are known as aromatic compound.
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
EBK PHYSICAL CHEMISTRY
- 16. Which of the following structures is the CORRECT resonance structure of the following. molecule: (A) (B) (C) (D) CH3- CH₂ CH3 -H CH₂CH3 CH₂CH-CH₂ CH3 CH3arrow_forward(e) The mean bond enthalpy for chlorine is +242 kJ mol·l and that for fluorine is +158 kJ mol-". The enthalpy of formation of CIF (g) is 56 kJ mol·l (ii) Calculate the enthalpy of formation of, gaseous Chlorine Trifluoride, CIF3 (g), using the bond enthalpy value you obtained in part (i). (iii) The bond enthalpy of CIF3 calculated in part (ii) is likely to be different than that determined from experiment. Explain.arrow_forwardTo satisfy the octet rule, fullerenes must have doublebonds. How many? Give a simple rule for one way ofplacing them in the structure shown in Figure 7.17a.arrow_forward
- Draw Lewis structures for each of the following compounds. In each case, specify the number of valence electrons surrounding the central atom. (Assign lone pairs and radical electrons where appropriate.) (Assume the central atom does not contain an expanded octet.) (a) bromine dioxide (BrO2) (b) beryllium bromide (BeBr2) (c) phosphorus pentafluoride (PF5)arrow_forwardIf the first, second and third bond dissociation enthalpies of methane are +420, +475, and +421 KJmol-l, respectively, calculate the fourth. How do you account for the fact that; ammonium nitrate is readily soluble in water even though the standard enthalpy of solution has a positive value? although the enthalpy of combustion of cane sugar is about -6000 KJmol-l cane sugar is not observed to oxidise in air at ordinary temperature?arrow_forwardConsider a chemical species (either a molecule or an ion) in which a carbon atom forms three single bonds to three hydrogen atoms and in which the carbon atom possesses an unshared electron pair. (a) What formal charge would the carbon atom have? Note: enter sign followed by number to answer this question (e.g. "+1"). Formal charge = (b) What total charge would the species have? Note: enter sign followed by number to answer this question (e.g. "+1"). Total charge = (c) What shape would you expect this species have? Shape= (d) What would you expect the hybridization of the carbon atom to be? Carbon hybridization = sp O sp³d² O sp³d O sp³ sp²arrow_forward
- Hello, may someone help me thankyou!! urgent!arrow_forwardThe partial Lewis structure that follows is for a hydrocarbonmolecule. In the full Lewis structure, each carbon atomsatisfies the octet rule, and there are no unshared electronpairs in the molecule. The carbon—carbon bondsare labeled 1, 2, and 3. (a) How many hydrogen atomsare in the molecule? (b) Rank the carbon–carbonbonds in order of increasing bond length. (c) Whichcarbon—carbon bond is the strongest one? [Sections 8.3and 8.8]arrow_forwardThe partial Lewis structure that follows is for a hydrocarbonmolecule. In the full Lewis structure, each carbon atomsatisfies the octet rule, and there are no unshared electronpairs in the molecule. The carbon—carbon bondsare labeled 1, 2, and 3. (a) How many hydrogen atomsare in the molecule? (b) Rank the carbon–carbonbonds in order of increasing bond length. (c) Whichcarbon—carbon bond is the strongest one?arrow_forward
- Which molecule is very unlikely to be isolated as a pure, stable molecule? (a) (b) (c) CH3O HOH (d) (b) (c) (d)arrow_forwardKeeping the same atomic connections and moving only electrons, write a more stable Lewis structure for each of the following. Be sure to specify formal charges, if any, in the new structure. (g) (h) (i)arrow_forwardDraw a structural formula for a hydrocarbon with the given molecular formula that undergoes hydroboration-oxidation to give the indicated product. (a) (b) • All hydrogen atoms are implied. Apply formal charges where appropriate. • Omit lone pairs and radical electrons from your answer. ● C₂H10 C₂H12 1. (sia) BH 2. H₂O₂, NaOH Il 1. BH₂ 2. H₂O2₂, NaOH H Sn [F ? ChemDoodle OHarrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning