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Q: (a) How does the structure of diborane (B2H6) differ fromthat of ethane (C2H6)? (b) Explain why…
A: (a) How does the structure of diborane (B2H6) differ from that of ethane (C2H6).
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- (a) How does the structure of diborane (B2H6) differ fromthat of ethane (C2H6)? (b) Explain why diborane adoptsthe geometry that it does. (c) What is the significance ofthe statement that the hydrogen atoms in diborane aredescribed as “hydridic”?Which of the following compounds are consistent with the Huckel rule?NB Assume the densities of all solutions are 1.0 g/mL and their specific heat capacities 4.184 J/g .K Molar Mass of KCl: 74.55 g/mol Help from calculating qr to average ethalpy.
- In CH2BrCl, are the hydrogen atoms equivalent (i.e., do they have identical environments with respect to the other atoms adjacent to themselves)?Can someone please explain and show work / calculations? Please use an outside bond dissociation energy sheetBriefly describe how the hydration energy of pentahydrated copper sulphate (CuSO4.5H2O) can be determined. State 2 conditions necessary for the formation of a dative or coordinate bond.
- There is some indication that other hydrogen ring compounds and ions in addition to H3 and D3 species may play a role in interstellar chemistry. According to J.S. Wright and G.A. DiLabio (J. Phys. Chem. 96, 10 793 (1992)), H5−, H6, and H7+ are particularly stable whereas H4 and H5+ are not. Confirm these statements by Hückel calculations.Explain why does it require an input of energy when an uncharged molecule moves from a concentration of 10-4 M to 10-2 M?Calculate the bond energy of C-F given that the heat of atominzation of CHFClBr is 1502 kj/mol, and that the bond energies of C--H, C--Br, and C-Cl are 413, 276 and 328 kj/mol, respectively. show the calculations