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- (b) The Murchison meteorite that landed in Australia in 1969 contained 92 different amino acids, including 21 found in Earth organism A skeleton structure (single bond only) of one of these extraterrestrial amino acids is shown below. Draw a Lewis structure, and identify any atoms having a nonzero formal charge. H3N. C ČH2 ČH3 (c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F, 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smaller going down the halogen group from HF to HI Describe these observationsWrite Lewis structures for the following:(a) SeF6(b) XeF4(c) SeCl3+(d) Cl2BBCl2 (contains a B–B bond)Please don't provide handwriting solution
- 65. Calculate the formal charge of each element in the following compounds and ions: (a) F2CO (b) NO– (c) BF4−BF4− (d) SnCl3−SnCl3− (e) H2CCH2 (f) ClF3 (g) SeF6 (h) PO43−what is the generic formula (format for example, AX3E) and formal charge of Chlorine trifluoride?Write Lewis structures for the following: (a) H2 (b) HBr (c) PCl3 (d) SF2 (e) H2CCH2 (f) HNHH (g) H2CNH (h) NO– (i) N2 (j) CO (k) CN–
- The structure of borazine, B3N3H6, is a six-membered ringof alternating B and N atoms. There is one H atom bondedto each B and to each N atom. The molecule is planar.(a) Write a Lewis structure for borazine in which the formalcharge on every atom is zero. (b) Write a Lewis structurefor borazine in which the octet rule is satisfied forevery atom. (c) What are the formal charges on the atomsin the Lewis structure from part (b)? Given the electronegativitiesof B and N, do the formal charges seem favorableor unfavorable? (d) Do either of the Lewis structuresin parts (a) and (b) have multiple resonance structures?(e) What are the hybridizations at the B and N atoms inthe Lewis structures from parts (a) and (b)? Would you expectthe molecule to be planar for both Lewis structures?(f) The six B¬N bonds in the borazine molecule are allidentical in length at 1.44 Å. Typical values for the bondlengths of B¬N single and double bonds are 1.51 Å and1.31 A°, respectively. Does the value of the B¬N…Write Lewis structures for the following:(a) H2(b) HBr(c) PCl3(d) SF2(e) H2CCH2(f) HNNH(g) H2CNH(h) NO–(i) N2(j) CO(k) CN–5) (a) Write the Lewis structure for HCO2 - ion. Include two resonance structures. (b) Assign formal charges to each of the atoms in these resonance structures and determine the molecular geometry of HCO2- ion? B(Ctrl)
- Determine the number of valence electrons in (CH₃C(O)CN) and then draw the corresponding Lewis structure.Rank the members of each set of compounds in order of increasing ionic character of their bonds. Use polar arrowsto in-dicate the bond polarity of each:(a) HBr, HCl, HI (b) H₂O, CH₄, HF (c) SCl₂, PCl₃, SiCl₄Draw all possible resonance structures for SO2, S0,, and SO. Use the resonance structures to solve the problems below. (a) Arrange these species in order of increasing S-O bond length (shortest bond first). O SO O SO O SO2 O SO2 O so;²- O SO O So3? O SO2 (b) Match each species with the number of covalent bonds predicted by Lewis structures to exist between an S atom and an O atom bonded to this S atom. (Hint: Average the number of bonds between S and an attached oxygen atom in a particular position using all of your resonance structures for the species that you are working on.) SO: -Select-v bonds between S and 0. -Select--- v bonds between S and O. SO2: Select-v bonds between S and O. (c) Match each species with the correct formal charge on the central S atom. SO: Select- charge on S. SO2: Select--v charge on S. SO32:-Select-vcharge on S. (d) Match each species with the average formal charge on an outside oxygen atom predicted by Lewis structures. so: -Select-vaverage charge on…