# Add lone pairs to the lewis structures of these polyhalide ions

problem! ## General guidance

Concepts and reason
The problem is based on the concept of Lewis structure.

Lewis structure is the electron dot structure and represents the electron distribution in the atom. Lewis structure generally follows the octet rule.

Fundamentals

The electron distribution in the atom is represented by Lewis structure. The electrons in the outer shell are known as valence electrons. To complete the octet of the atom, valence shell should have 8 electrons. For the Lewis structure, the total number of valence electrons and number of electrons needed to complete the octet of the atom are counted. In the molecule, the total number of bonds in the molecule is counted and the skeletal structure of the compound is drawn. The total electrons are counted in the bond and the remaining electrons are added to the atom such that the octet of each atom is complete. The electrons which are not bonded to the bond are the non-bonding electrons and are termed as the lone pairs.

## Step-by-step

### Step 1 of 3

Part 1

Count the total number of valence electrons in as follows: The total number of valence electrons in are 22 electrons.

Consider the skeletal structure of as follows: The skeletal structure has 4 electrons. 18 valence electrons are remaining. Give 6 electrons to each atom of and . Draw the Lewis structure of as follows: Part 1

The Lewis structure for with lone pairs is as follows: The compound has 22 electrons. Two bonds are present in the compound which counts as 4 electrons. The remaining 18 electrons are distributed to the Chlorine (Cl) and Fluorine (F) atoms such that each atom of and has 6 non- bonding electrons. The compound do not follow the octet rule.

### Step 2 of 3

Part 2

Count the total number of valence electrons in as follows: The total number of valence electrons in are 20 electrons.

Consider the skeletal structure of as follows: The skeletal structure has 4 electrons. 16 valence electrons are remaining. Give 6 electrons to each atom of and . Therefore, the octet of and is complete. Draw the Lewis structure of as follows: Part 2

The Lewis structure for with lone pairs is as follows: The compound has 20 electrons. Two bonds are present in the compound which counts as 4 electrons. The remaining 16 electrons are distributed to the Chlorine (Cl) and Fluorine (F) atoms such that each atom of has 6 non- bonding electrons and atom has 4 non- bonding electrons. The compound follow the octet rule.

### Step 3 of 3

Part 3

Count the total number of valence electrons in as follows: The total number of valence electrons in are 36 electrons.

Consider the skeletal structure of as follows: The skeletal structure has 8 electrons. 28 valence electrons are remaining. Give 4 electrons to and 6 electrons to each atom of . Draw the Lewis structure of as follows: Part 3

The Lewis structure of with lone pairs is as follows: The compound has 36 electrons. Four bonds are present in the compound which counts as 8 electrons. The remaining 28 electrons are distributed to the Chlorine (Cl) and Fluorine (F) atoms such that each atom of has 6 non- bonding electrons and atom has 46 non- bonding electrons. The compound do not follow the octet rule.

Part 1

The Lewis structure for with lone pairs is as follows: Part 2

The Lewis structure for with lone pairs is as follows: Part 3

The Lewis structure of with lone pairs is as follows: 