name of woodward's reagent k

woodward's reagent k

formula | C_11H_11NO_4S name | woodward's reagent k IUPAC name | 3-(2-ethyl-5-isoxazol-2-iumyl)benzenesulfonate alternate names | 2-ethyl-5-phenylisoxazolium-3'-sulfonate | 2-ethyl-5-phenylisoxazolium-3'-sulphonate | 3-(2-ethyl-1, 2-oxazol-2-ium-5-yl)benzenesulfonate | 3-(2-ethylisoxazol-2-ium-5-yl)benzenesulfonate | NEPIS | N-ethyl-5-phenylisoxazolium-3'-sulfonate mass fractions | C (carbon) 52.2% | H (hydrogen) 4.38% | N (nitrogen) 5.53% | O (oxygen) 25.3% | S (sulfur) 12.7%

Draw the Lewis structure of woodward's reagent k. Start by drawing the overall structure of the molecule, ignoring potential double and triple bonds: Count the total valence electrons of the carbon (n_C, val = 4), hydrogen (n_H, val = 1), nitrogen (n_N, val = 5), oxygen (n_O, val = 6), and sulfur (n_S, val = 6) atoms: 11 n_C, val + 11 n_H, val + n_N, val + 4 n_O, val + n_S, val = 90 Calculate the number of electrons needed to completely fill the valence shells for carbon (n_C, full = 8), hydrogen (n_H, full = 2), nitrogen (n_N, full = 8), oxygen (n_O, full = 8), and sulfur (n_S, full = 8): 11 n_C, full + 11 n_H, full + n_N, full + 4 n_O, full + n_S, full = 158 Subtracting these two numbers shows that 158 - 90 = 68 bonding electrons are needed. Each bond has two electrons, so in addition to the 29 bonds already present in the diagram we expect to add 5 bonds. To minimize formal charge oxygen wants 2 bonds and carbon wants 4 bonds. Identify the atoms that want additional bonds and the number of electrons remaining on each atom: To fully fill its valence shell, nitrogen will donate one of its electrons, allowing it to form four bonds (the maximum number an element on period 2 can form). Add 5 bonds by pairing electrons between adjacent highlighted atoms. Additionally, atoms with large electronegativities can minimize their formal charge by forcing atoms with smaller electronegativities on period 3 or higher to expand their valence shells. The electronegativities of the atoms are 2.20 (hydrogen), 2.55 (carbon), 2.58 (sulfur), 3.04 (nitrogen), and 3.44 (oxygen). Because the electronegativity of sulfur is smaller than the electronegativity of oxygen, expand the valence shell of sulfur to 6 bonds (the maximum number of bonds it can accomodate). Therefore we add a total of 7 bonds to the diagram, noting the formal charges of the atoms. Double bonding sulfur to the other highlighted oxygen atom would result in an equivalent molecule. The six atom ring is aromatic, so that the single and double bonds may be rearranged: Answer: | |

3D structure

molar mass | 253.27 g/mol phase | solid (at STP) melting point | 220 °C

CAS number | 4156-16-5 Beilstein number | 4149224 PubChem CID number | 77804 PubChem SID number | 24894560 SMILES identifier | CC[N+]1=CC=C(O1)C2=CC(=CC=C2)S(=O)(=O)[O-] InChI identifier | InChI=1/C11H11NO4S/c1-2-12-7-6-11(16-12)9-4-3-5-10(8-9)17(13, 14)15/h3-8H, 2H2, 1H3 MDL number | MFCD00012128

NFPA label

NFPA health rating | 1 NFPA fire rating | 0 NFPA reactivity rating | 0