Draw a single best Lewis structure for each molecule below. Assign non-zero formal charges to each atom. (a.) H2O2 (hydrogen peroxide) b) N2H4 (hydrazine) c) CH3SCN (methyl thiocyanate)
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Draw a single best Lewis structure for each molecule below. Assign non-zero formal charges to each atom.
(a.) H2O2 (hydrogen peroxide)
b) N2H4 (hydrazine)
c) CH3SCN (methyl thiocyanate)
d) CH2Cl2 (dichloromethane)
e) SF6 (sulfur hexafluoride)
f) PCl5 (phosphorus pentachloride)
g) HClO4 (perchloric acid)
h) BH3 (boron trihydride)
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- Carbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.Draw acceptable Lewis structures, including resonance contributors where appropriate with all non-bonding electrons and formal charges. N2O4 [HCO3]- [F2BrO]+ [H2PO3S]-
- Draw the lewis structure of SO2 ( best resonance) and 2nd best resonance showing the shape and bond angles of each one, the 3D structure with polar bonds or bonds dipole of each one and the molecular polarity. Here is an example of what I want the answer to be like:Draw three valid Lewis structures for the SiPSH (connected Si-P-S-H) that obey the octet rule and write any non-zero formal charges above the structures and circle the best structure.Calculate the formal charges on each oxygen atom in H2PO4-. show your work and explainanswer: In H2PO4-, two oxygen atoms (bonded to H) have a formal charge of zero, while the other two have a formal charge of -1/2.
- For the following molecules:I. Draw the best Lewis Dot Structures for each of the following molecules. The best structuretakes into consideration resonance structures, calculations of formal charge for each atom,and tries to minimize the overall formal charge for the structure. II. Draw the 3-D VSEPR structures for the following molecules. You may combine these twodrawings (for I and II) into 1 drawing if you wish. III. Label the bond angles. IV. State the electron geometry (basic VSEPR) and molecular shape (derivative VSEPR) foreach molecule. V. State the hybridization around each central atom in the molecule. VI. State whether the overall molecule is polar or nonpolar. VII. For any two of the following molecules, state the strongest intermolecular force betweenmultiple of the same molecule.a. IF2b. H2CO3c. CH3CH2COOHd. N2O4e. PO4^3-f. CH3COCNg. ClO3^-1h. C4H8Some of the figures below represent invalid sets of resonance structures for this molecule.Q1. Draw the Lewis structure of given compound;a) CH3NH2 (metil amine)b) HCOOH (formic acid)c) HCSNH2d) NH2CONH2Q2. Draw Lewis structure of the following species, indication formal charges andresonance where applicable;a) HOSO3-b) H2NCNc) FCO2-d) HCO3-e) FSO3-Q3. Use the VSEPR theory to predict the shape ofa) The molecule OSF2b) The ion ClO3-c) The ion of S2O32-d) Th ion of BrF4
- Q/ Three resonance structures of the highly unstable CSN – ion are shown below. a) Label any and all atomic formal charges that are present in each structure. b) Which of the structures is the major resonance structure? Why?Consider this “Dr. Yan’s imaginary” molecule below in line-angle formula. Note that you MAY NOT add or remove lone pairs. How many CH groups are there in the molecule? ____________ b) The formal charge of O is:__________; and the formal charge of N is: ____________________ c) The overall charge of the molecule: ___________What would be the formal charge on Se and S and both Os for the most stable resonance structures of SeSO22- (considering it's stabilized by minimizing formal charge) ? Group of answer choices Se(+1) , S(-), O(-), O(-) Se(-) , S(+1), O(-1), O(-) Se(-) , S(0), O(+), O(-) Se(0) , S(-), O(-), O(0) Se(0) , S(0), O(-), O(-)