Covalent Bonding in Carbon Compounds MCQs Quiz | Class 10
This quiz is specifically designed for Class X students for the Subject Science (Code 086), covering Unit I: Chemical Substances – Nature and Behaviour. The topic in focus is Covalent Bonding in Carbon Compounds, dealing with why carbon forms covalent bonds and the basic mechanisms of electron sharing. Attempt these 10 MCQs to test your knowledge, submit to see your score, and click Download Answer PDF to save your result for future revision.
Understanding Covalent Bonding in Carbon
Carbon is a versatile element found in all living organisms and many non-living things. Its unique chemical properties are defined by its atomic number, electronic configuration, and the way it bonds with other elements.
1. Why Carbon Forms Covalent Bonds
Carbon has an atomic number of 6, which means its electronic configuration is 2, 4. To achieve a stable noble gas configuration, it needs to either gain or lose 4 electrons. However, both options present significant difficulties:
- Gaining 4 electrons (C4- anion): It would be difficult for the nucleus with 6 protons to hold on to 10 electrons due to high inter-electronic repulsion.
- Losing 4 electrons (C4+ cation): It would require a very large amount of energy to remove 4 electrons from the outermost shell, leaving behind a carbon cation with 6 protons and only 2 electrons.
Therefore, carbon overcomes this problem by sharing its valence electrons with other atoms of carbon or with atoms of other elements. This mutual sharing of electrons forms a Covalent Bond.
2. Types of Covalent Bonds
Depending on the number of electron pairs shared between two atoms, covalent bonds are classified as:
| Bond Type | Electrons Shared | Example |
|---|---|---|
| Single Bond | 1 pair (2 electrons) | Hydrogen (H2), Methane (CH4) |
| Double Bond | 2 pairs (4 electrons) | Oxygen (O2), Carbon Dioxide (CO2) |
| Triple Bond | 3 pairs (6 electrons) | Nitrogen (N2) |
3. Properties of Covalent Compounds
- Low Melting and Boiling Points: The forces of attraction between the molecules are relatively weak.
- Poor Conductors of Electricity: Since no charged particles (ions) are formed during covalent bonding, these compounds generally do not conduct electricity.
Quick Revision Notes
- Carbon is tetravalent (valency = 4).
- Shared electrons belong to the outer shells of both atoms and lead to both attaining the noble gas configuration.
- Methane (CH4) is the simplest hydrocarbon formed by single covalent bonds between one carbon and four hydrogen atoms.
Extra Practice Questions
- Draw the electron dot structure for Ammonia (NH3).
- Explain why covalent compounds are generally volatile.
- What is the bond angle in a methane molecule?
- Differentiate between ionic and covalent bonds with examples.
- How many covalent bonds are present in Ethane (C2H6)?
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