In order to draw the Lewis structure for LiCl, we need to know the number of valence electrons involved.

- Lithium (Li) belongs to Group 1 and has one valence electron in its outermost shell.

- Chlorine (Cl) belongs to Group 17 and has seven valence electrons in its outermost shell.

To form LiCl, the lithium atom will transfer its one valence electron to the chlorine atom. This results in a complete octet for chlorine, achieving a stable configuration.

In the Lewis structure, we represent the valence electrons as dots around the atomic symbols:

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:Cl-Li:

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Therefore, in the Lewis structure for LiCl, a total of 8 valence electrons need to be accommodated - one from lithium and seven from chlorine, to satisfy the octet rule.