What is the electron dot structure for PC{{l}_{3}}?

The electron dot structure, also known as the Lewis structure or Lewis dot structure, represents the arrangement of electrons in a molecule. To draw the electron dot structure for PCl3 (phosphorus trichloride), you need to consider the valence electrons of each atom.

Here's how you can construct the Lewis structure for PCl3:

Determine the total number of valence electrons for PCl3:

Phosphorus (P) is in Group 15 of the periodic table, so it has 5 valence electrons.
Chlorine (Cl) is in Group 17 of the periodic table, so each chlorine atom has 7 valence electrons. PCl3 has 3 chlorine atoms, so that's a total of 3 x 7 = 21 valence electrons.
Total valence electrons = 5 (from P) + 21 (from 3 Cl atoms) = 26 valence electrons.

Determine the central atom. In PCl3, phosphorus (P) is the central atom because it is less electronegative than chlorine.

Place the central atom (P) in the center and connect it to the surrounding atoms (Cl) using single bonds (represented by a pair of electrons). This uses up 2 valence electrons for each bond.

P-Cl
|
Cl

Distribute the remaining valence electrons around the outer atoms (Cl) to satisfy their octet (8 electrons) or duet (2 electrons) rule. In this case, each chlorine atom needs 8 electrons to fill its outer shell.

P-Cl
| |
Cl Cl

Place the remaining valence electrons on the central atom (P) to satisfy its octet rule. In this case, phosphorus needs 8 electrons in its outer shell.

P
| |
Cl Cl

Check if all atoms have satisfied the octet (or duet) rule. In this case, all atoms have an octet (or duet), and there are no remaining valence electrons.

So, the electron dot structure for PCl3 is:

P
| |
Cl Cl

Each bond represents a pair of electrons, and all atoms have a full outer shell of electrons.