Covalent Bonding
1.0Master Covalent Bonding in Minutes
Discover how atoms collaborate by sharing rather than transferring. Learn the fundamentals of electron sharing, the structural types of covalent bonds, and their distinct molecular properties through clear chemical guidelines and exam-focused explanations.
2.0Learning Outcomes
After completing this lesson, you will be able to:
- Define covalent bonding and explain why atoms share electrons.
- Differentiate between single, double, and triple covalent bonds with textbook examples.
- Draw electron-dot (Lewis) structures for common molecules like Hydrogen, Oxygen, Nitrogen, and CH4.
- Explain the physical properties of covalent compounds (melting point, solubility, conductivity).
- Compare and contrast ionic bonding with covalent bonding to confidently ace board exam questions.
3.0Introduction
Chemistry explains how atoms combine with each other to form molecules and compounds. One of the most important concepts in Class 10 Science Chapter – Carbon and Its Compounds is Covalent Bonding. Covalent bonding helps explain how non-metal atoms combine by sharing electrons.
Many substances around us such as water, oxygen, methane, carbon dioxide, and hydrogen are formed through covalent bonding. Understanding covalent bonds is important because they are involved in many chemical and biological processes.
This article explains covalent bonding definition, covalent bonding examples, Class 10 notes, properties, formation, and important concepts in simple and easy-to-understand language.
4.0What is Covalent Bonding?
Covalent Bond is a type of chemical bond formed when two atoms share electrons with each other to achieve a stable electronic configuration. Unlike ionic bonding, where electrons are transferred, covalent bonding involves the sharing of electrons.
Covalent bonding usually occurs between:
- Non-metals
- Atoms with similar electronegativity
5.0Why Do Atoms Form Covalent Bonds?
Covalent bonds are formed when atoms share one or more pairs of electrons. Each shared pair of electrons forms one covalent bond.
Atoms form covalent bonds to achieve:
- Stable electronic configuration
- Octet completion
- Lower energy state
Most atoms try to attain the electronic configuration of noble gases.
6.0Types of Covalent Bonds
Depending upon the number of shared electron pairs, the covalent bond can be classified into:
- Single Covalent Bond
- Double Covalent Bond
- Triple Covalent Bond
Single Bonds
It occurs between two atoms that form a bond by sharing two pairs of electrons. It is represented as two dashes (=). Double covalent bonds are stronger than single ones but not as stable.
Double Bonds
There are double bonds when two pairs of electrons are being shared between the two bonded atoms. It is represented by two dashes (=). While double bonds are stronger than single bonds, double bonds are not as stable as triple bonds.
For example,
CO2 Molecule with Double Covalent Bond
O2 Molecule with a Double Covalent Bond
Double Bond in Ethylene Molecule
Triple Bond
When two atoms share three pairs of electrons, they produce a triple bond, which is represented by three dashes (≡). Triple covalent bonds are considered to be the least stable type of covalent bond.
Nitrogen Molecule with Triple Bond
Polar Covalent Bond
This type of covalent bond exists where the unequal sharing of electrons occurs due to the difference in the electronegativity of combining atoms. More electronegative atoms will have a stronger pull for electrons. The electronegative difference between the atoms is greater than zero and less than 2.0. As a result, the shared pair of electrons will be closer to that atom.
Nonpolar Covalent Bond
In this case, the two atoms will have a difference in electronegativity of zero (no difference). A bond will also form when two atoms with the same electron affinity are brought to combine (diatomic elements).
7.0Properties of Covalent Compounds
Covalent compounds have special properties because they are formed through electron sharing.
- Covalent bonding does not result in the formation of new electrons. The bond only pairs them.
- They are very powerful chemical bonds that exist between atoms.
- A covalent bond normally contains an energy of about ~80 kilocalories per mole (kcal/mol).
- Covalent bonds rarely break spontaneously after it is formed.
- Covalent bonds are directional, where the atoms that are bonded showcase specific orientations relative to one another.
- Most compounds having covalent bonds exhibit relatively low melting points and boiling points.
- Compounds with covalent bonds usually have lower enthalpies of vaporisation and fusion.
- Compounds formed by covalent bonding don’t conduct electricity due to the lack of free electrons.
- Covalent compounds are not soluble in water.
8.0Difference Between Ionic Bonding and Covalent Bonding
9.0Covalent Bonding Examples in Daily Life
Covalent compounds are present everywhere around us.
- Water (H₂O): Water is one of the most important covalent compounds necessary for life.
- Carbon Dioxide (CO₂): Carbon dioxide is used by plants during photosynthesis.
- Methane (CH₄): Methane is used as a fuel in homes and industries.
- Oxygen (O₂): Oxygen is essential for respiration.
10.0EUREKA by ALLEN – Premium Online Learning for Class 10
With EUREKA from the ALLEN, you will achieve the highest level of academic achievement through an innovative approach designed specifically for Class 10 students. EUREKA provides world-class education using top instructors, cutting-edge artificial intelligence, and a proven method for preparing for board examinations; thus creating a complete learning environment for success. Through personalized assistance, compelling content, and ongoing assessment of progress toward maximum achievement, students receive everything they need to realise their full academic capabilities.
11.0Supporting Study Materials
This study material, including CBSE Notes and NCERT Solutions for the Chapter "Carbon and Its Compounds" focusing on Covalent Bonding, is designed according to the latest CBSE Class 10 Science syllabus and NCERT guidelines. It features precise electronic configuration breakdowns, visual orbital overlap ideas, and key conceptual review tables to maximize your scores in competitive and school board assessments.
12.0Previous Year Questions (PYQs): Covalent Bonding
Q1. What is a covalent bond? Why do covalent compounds generally have low melting and boiling points and are poor conductors of electricity? (CBSE Board)
Answer: * Definition: A covalent bond is a chemical bond formed by the mutual sharing of one or more pairs of electrons between two atoms (usually non-metals) to achieve a stable noble gas configuration.
- Low Melting and Boiling Points: Covalent compounds exist as discrete molecules. Although the covalent bonds within the molecules are strong, the intermolecular forces of attraction between separate molecules (Van der Waals forces) are weak. Very little heat energy is required to break these weak intermolecular forces.
- Poor Electrical Conductivity: Covalent bonds involve the sharing of electrons; no transfer takes place. Consequently, there are no charged ions or free, mobile electrons present in covalent compounds to conduct an electric current.
13.030Second Quick Revision: Covalent Bonding
- Covalent bonds are formed by the sharing of electrons between atoms.
- Usually formed between non-metals.
- Atoms share electrons to achieve a stable electronic configuration.
- A single shared pair of electrons forms a single covalent bond.
- Two shared pairs form a double bond.
- Three shared pairs form a triple bond.
- Covalent compounds generally have low melting and boiling points.
- They are usually poor conductors of electricity.
- Examples: Hydrogen (H₂), Oxygen (O₂), Water (H₂O), Methane (CH₄), Carbon dioxide (CO₂).
- Covalent bonding helps atoms complete their valence shell and attain stability.
14.0Recommended Next Topics