Draw the lewis dot structure showing what happens during the

reaction Lithium and Chlorine produce Lithium Chloride.

how do you draw this, please help .

Drawings are almost impossible on the boards. Here is about the best I can do.

Li. +
..
:Cl:
..
|
|
v
Li+ + :Cl:-1
then add two electrons to the top and two electrons to the bottom of the Cl.

I have one too many dots on the first Cl. Remove one of the dots to leave 7.

To draw the Lewis dot structure for Lithium and Chlorine reacting to form Lithium Chloride, follow these steps:

Step 1: Determine the number of valence electrons for each atom:
- Lithium (Li) is in Group 1, so it has 1 valence electron.
- Chlorine (Cl) is in Group 17, so it has 7 valence electrons.

Step 2: Determine the total number of valence electrons:
- In this case, we have 1 Lithium atom (1 valence electron) and 1 Chlorine atom (7 valence electrons).
- The total number of valence electrons is 1 + 7 = 8.

Step 3: Determine the central atom:
- In Lithium Chloride, Lithium is the metal and Chlorine is the non-metal. Lithium is less electronegative than Chlorine, so it will be the central atom.

Step 4: Connect the atoms:
- Place the Lithium atom in the center, and the Chlorine atom on one side.
- Connect them by a single bond (a line) representing a pair of shared electrons between them.

Step 5: Distribute electrons:
- Start by placing 2 electrons (1 pair) between the Lithium and Chlorine atoms to fulfill the Lithium atom's octet (2 valence electrons).
- The remaining 6 electrons will be placed around the Chlorine atom.

Step 6: Distribute electrons further and fulfill octets:
- Now, distribute the remaining 6 electrons around the Chlorine atom, giving a total of 8 electrons around it.
- Follow the octet rule, which states that atoms tend to gain or lose electrons to achieve a stable electron configuration with 8 electrons in the outermost shell (except for Hydrogen and Helium).

Step 7: Check for octet completion and formal charges:
- The Chlorine atom now has a complete octet (8 electrons), and no formal charges are present.
- The Lithium atom only has 2 electrons, which is less than the octet.
- To fulfill the Lithium atom's octet, borrow 1 pair of electrons from the Chlorine atom by converting one of the lone pairs on Chlorine into a bonding pair.

Step 8: Final structure:
- The Lewis dot structure for Lithium Chloride (LiCl) will have the Chlorine atom surrounded by 8 electrons (including the bonding pair with Lithium) and the Lithium atom having 2 electrons.

The final structure can be represented as:
Li
:
Cl-Li-Cl