A simple method for writing

Several worked examples relevant to this procedure were given in previous posts please see the Sitemap - Table of Contents (Lewis Electron Dot Structures).

**Lewis Dot Structures**is given in a previous article entitled “Lewis Structures and the Octet Rule”.Several worked examples relevant to this procedure were given in previous posts please see the Sitemap - Table of Contents (Lewis Electron Dot Structures).

Let us consider
the case of chloryl (ClO

_{2}^{+})_{ }.__Step 1__: Connect the atoms with single bonds. The central atom is the chlorine atom.

Fig. 1 : Connect the atoms of the chloryl
(ClO_{2}^{+}) with single bonds._{} |

__Step 2__: Calculate the # of electrons in π bonds (multiple bonds) using

**formula (1)**:

Where n in this
case is 3 since ClO

_{2}^{+ }consists of three atoms.
Where V = (7 + 6
+ 6 ) – 1 = 18

Therefore, P = 6n
+ 2 – V = 6 * 3 + 2 – 18 = 2

**So, there are 2****π electrons in**_{ }**ClO**_{2}^{+ }**and the structure in Step 1 has 1 double bond.**
Electrons are
placed around each atom so that the octet rule is obeyed. Since Cl is a third row element can accommodate more than 8 electrons.

__Step 3 & 4__: The Lewis

**of**

__resonance structures__**ClO**

_{2}^{+ }_{ }are

**as follows:**

The most stable

**resonance structure**is #4 since it has the smallest charge separation and the positive charge is on the Cl atom which is less electronegative than O.
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