Lewis Structure of HCl

Hydrochloric acid is a chemical that is inorganic. It has the chemical formula HCl and is a strong corrosive acid. It is also known as muriatic acid or hydrogen chloride.

HCl is formed when hydrogen chloride is dissolved in water. It is a simple diatomic molecule. A single covalent bond connects the hydrogen and chlorine atoms. Because the chlorine atom is more electronegative than the hydrogen atom, the bond between them is polar.

It has high acidity. It has no colour and is very viscous. It is highly corrosive and has a distinct pungent odour.

Table of Contents

• How to draw the Lewis Structure of HCl?
• Molecular Geometry of HCl
• Hybridization of HCl
• Polarity of HCl
• Frequently Asked Questions – FAQs

How to draw Lewis Structure of HCl?

When drawing a Lewis dot structure, we are always aiming for an electron count at which all of the atoms involved are stable and (usually) have full octets. We are also attempting to create a structure with the least amount of formal charge possible. The general rule is to isolate all of the elements involved and their valence electrons first, then start piecing them together in an attempt to reduce the formal charge and bring all elements involved to an octet.

Steps to draw Lewis structure of HCl

Step 1. Determine the total number of valence electrons in the molecule

In the periodic table, hydrogen is in the first group and chlorine is in the 17th.

As a result, the valence electron of-

Hydrogen = 1

Chlorine = 7

∴ Total available valence electrons = 1 + 7 = 8

Step 2: Determine the central atom

The central atom will be chlorine as it is more electronegative.

Step 3: Mark atoms with lone pairs

Step 4: If there are charges on atoms, mark them.

There are no charges in the molecule.

Step 5: To obtain the best Lewis structure convert the lonepairs to bonds.

As a halogen, chlorine requires one more electron to complete its octet. Similarly, hydrogen requires one more electron to achieve an octet because hydrogen’s outermost shell can only hold two electrons.

As a result, a single bond is formed between the two atoms, resulting in the formation of a covalent bond.

Step 6: Check the stability of the structure

It can be checked by using the formula-

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

Since the overall formal charge is zero, the above Lewis structure of HCl is most appropriate, reliable, and stable in nature.

Molecular Geometry of HCl

HCl has linear molecular geometry/shape and tetrahedral electron geometry, according to VSEPR theory. The bond angle is 180°.

Read more: Molecular Geometry and Electron Geometry

Hybridization of HCl

There is no optical hybridization in HCl because it is a linear diatomic molecule with an H and a Cl atom bonded covalently.

Chlorine’s 3s has too little energy to interact with hydrogen 1s atomic orbital, but chlorine’s 3p_Z can interact with hydrogen’s 1s atomic orbital just fine.

Polarity of HCl

Chlorine has a greater electronegative potential than hydrogen. A more electronegative atom attracts the electron bond pair slightly more. As a result, the chlorine atom acquires a relatively negative charge and becomes the negative pole, while the hydrogen atom acquires a relatively positive charge and becomes the positive pole.

Two poles (positive and negative) are generated across a molecule in this way. This makes the molecule polar in nature.

HCl has a dipole moment of 1.03 D.