Lewis Dot Structure For Chlorine

Chlorine gas exists every bit a diatomic molecule with the chemical formula Cl_ii that belongs to the halogen group. It has a corrosive nature and is primarily used in the product of newspaper and vesture.

Chlorine atoms are covalently bonded to course a diatomic Cl_two molecule.

Cl₂ Lewis structure consists of ii chlorine atoms linked by a unmarried bail with three lone pairs on each chlorine.

Tabular array of Contents

How to draw Lewis Construction for Cl₂
Molecular Geometry of Cl₂
Hybridization of Cl_ii
Polarity of Cl_two
Oftentimes Asked Questions – FAQs

How to Describe Lewis Structure for Cl₂

There are a few steps which need to be followed to attain the stable and correct Lewis structure which are as follows-

i. Determine the total number of valence electrons in chlorine molecule.

The chlorine molecule contains ii chlorine atoms. In the periodic table, chlorine is a grouping VIIA element with seven electrons in its last vanquish.

Therefore, the total number of valence electrons= 7(2)= 14.

2. Full electron pairs exist in the form of alone pairs and bonds.

Total electron pairs are calculated by dividing the total valence electron count by 2. For the Cl_ii molecule, the full number of electron pairs in their valence shells is vii.

three. Determine the key atom

In that location are only ii atoms and they both vest to the same element, therefore, the fundamental cantlet volition exist chlorine just.

4. Mark atoms with lone pairs.

At that place are seven electron pairs in total.
The drawn structure already has ane bond. Equally a event, there are six more solitary pairs to mark on chlorine atoms.
Since there is no primal atom, we tin marker the remaining lonely pairs on both chlorine atoms.
3 lone pairs will be taken by each chlorine atom.
All valence electron pairs are now marked.

5. If there are charges on atoms, mark them.

There are no charges in the molecule of chlorine.

6. To obtain the all-time Lewis construction, minimise charges on atoms by converting lonely pairs to bonds.

Since there are no charges on atoms, there is no need to reduce charges every bit part of the procedure of drawing the best Lewis structure. We already accept the best Lewis structure for Cl₂.

seven. Cheque the stability of the structure

It can exist checked by using the formula-

Formal charge = Valence Electrons – Unbonded Electrons – ½ Bonded Electrons

Element

Chlorine

Formula Practical

Valence electrons = vii

Lone pair electrons = half-dozen

Shared pair electrons (1 single bail) = two

Formal Charge

(7 – 6 – 2/2) = 0

Since the overall formal charge is zilch, the above Lewis structure of Cl₂ is most advisable, reliable, and stable in nature.

Molecular Geometry of Cl_ii

Cl₂ has a linear electron geometry. This is due to the fact that all diatomic molecules or any molecule with only 2 atoms will have a linear geometry or shape as these molecules contain ii atoms that are continued with a single bond.

Hybridization in Cl₂

Each chlorine atom in the Cl₂ Lewis structure has an sp³ hybridization. Information technology has one s orbital and iii p orbitals. This results in four hybrid orbitals.

Polarity of Cl₂

In general, all diatomic molecules with the same atoms are non-polar in nature because they lack a dipole moment in add-on to the bond.

The dipole moment is only generated in a molecule when there is a charge separation or unequal charges distributed beyond atoms.

Therefore, Cl₂ is nonpolar.

Frequently Asked Questions on Lewis Construction of Chlorine Molecule

What is the number of sharing and non-sharing electrons in the Cl₂ Lewis structure?

1 bond exists between two chlorine atoms in the Cl₂ Lewis structure. Considering one bail contains 2 electrons, at that place are two electrons bachelor for sharing. Each chlorine cantlet has 3 lone pairs. So the total number of lonely pairs is half-dozen, resulting in 12 unshared electrons.

Explain the polarity of the Cl₂ molecule.

Cl_ii is non polar in nature because information technology lacks a dipole moment.

What type of bond is there in Cl₂?

There is a covalent bond in the Cl_two molecule because both atoms share and hold tightly onto each other'due south electrons.

Explain the formal charge of chlorine in the Cl₂ Lewis construction.

The formal charge of chlorine in the Cl_ii can be calculated by-

Formal charge = Valence Electrons – Unbonded Electrons – ½ Bonded Electrons

Valence electrons = 7, Lone pair electrons = 6, Shared pair electrons (ane single bond) = two

Therefore, Formal Accuse= (vii – 6 – 2/2) = 0

What is the bond angle of Cl₂?

Cl₂ has a bond angle of 180° because its molecular geometry is linear, indicating that atoms lie in a direct line.