I need help with number 1 part C. Of all the species that you looked at in this

Question

I need help with number 1 part C.

Of all the species that you looked at in this assignment, focus only on the following ten compounds/ions CH_4, CH_2 Cl_2, H_2 O, H_2 F^+, C_2 H_2 Cl_2 (all 3 isomers), CO_2, CO_3^2-, and O_3 in answering this question. If each of these compounds/ions were placed between two electrically charged plates (one positive and one negative) list all those species that would have a net attraction to the positive charge. list all those species that would have a net attraction to the negative charge. How is it possible that some species can be attracted to both positive and negative charges? Note the Lewis structure that you drew for H_2 F^+ (#6). Highly electronegative atoms often have a partial negative charge on them. Negative formal charges, on the other hand, are not necessarily found on highly electronegative atoms. Comment on the situation in this case. Is the formal charge of fluoronium ion on the least EN atom? Is this reasonable? Is there a choice? The three species N_2, CO, and CN^- (#11) are isoelectronic. As you did in the previous question comment on the location of any formal charges in these molecules/ion relative to the electronegativity of each of the atoms in the bond. Again, are all of the (non-zero) formal charges consistent with the relative EN's of the atoms? Are the structures reasonable?

Explanation / Answer

SOL: C) Some species are attracted by cathode and anode,depending on medium and potential.When the substance dissolved in medium to form cation by losing of an electrons and it is attracted by a cathode.When accept electrons from medium to form anion,attracted by a anode.

Ex: NH3 to form NH4+ and NH2-

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