Final answer:
The correct Lewis structure for the linear cation [H-C-N-Xe-F]+, taking into consideration the valence electrons and chemical bond rules, is H-C≡N-Xe-F with carbon and nitrogen connected by a triple bond, and xenon forming double bonds with nitrogen and fluorine.
Step-by-step explanation:
The question is asking to draw the Lewis structure of the linear cation [H-C-N-Xe-F]+. This structure is unusual because it involves a noble gas, Xe, which normally does not form many compounds. Given the linearity of the molecule and the fact that xenon can expand its octet, we can start by placing xenon (Xe) in the center with its eight valence electrons. We then connect Xe to both nitrogen (N) and fluorine (F), which are also in the compound.
A correct Lewis structure must take into account that the molecules form chemical bonds whereby each carbon (C) forms four bonds, nitrogen (N) forms three, and hydrogen (H) one. Considering xenon's ability to form more than eight electrons around it, we can have two double bonds (as shown by the :: symbols) connecting it to nitrogen and fluorine.
The correct Lewis structure that respects these rules and shows a linear geometry is: H-C≡N-Xe-F. Carbon and nitrogen are connected by a triple bond (as indicated by the ≡ symbol), and xenon bonds once to the nitrogen and once to the fluorine atom, both with double bonds.