JEE Main Chemistry: Hybridisation of carbon and σ and π-bonds Practice Questions
15 free multiple-choice questions on Hybridisation of carbon and σ and π-bonds (Basic Principles of Organic Chemistry) for JEE Main Chemistry, each with the correct answer and a step-by-step explanation. Attempt a question, then reveal the solution to check your reasoning.
Practice thousands more JEE Main questions in the app →Q1. The bond formed by the overlap of atomic orbitals along the internuclear axis is known as which type of bond?
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Correct answer: B — Sigma bond (σ bond)
Sigma (σ) bonds are formed by end-to-end (head-on) overlap of orbitals and are generally stronger than pi (π) bonds.
Q2. In a molecule where carbon atoms are sp² hybridized, what is the typical shape of the bond angle formed by these atoms?
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Correct answer: D — 120°
sp² hybridization leads to a trigonal planar geometry, and the ideal bond angle in this geometry is 120°.
Q3. Which of the following hybridization states corresponds to a planar geometry with 120° bond angles?
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Correct answer: C — sp²
sp² hybridization leads to a trigonal planar geometry with ideal bond angles of 120°.
Q4. Carbon atoms exhibiting sp² hybridization typically form bond angles close to:
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Correct answer: C — 120°
sp² hybridization involves three hybrid orbitals, leading to a trigonal planar geometry with ideal bond angles of 120°.
Q5. In an sp hybridized carbon, the geometry around the carbon atom is:
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Correct answer: A — Linear
sp hybridization results in a linear geometry (bond angle of 180°), characteristic of C≡ C triple bonds.
Q6. The formation of a π bond in organic molecules primarily results from the side-by-side overlap of which type of atomic orbitals?
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Correct answer: A — p orbitals
π bonds are formed by the lateral (side-by-side) overlap of unhybridized p orbitals.
Q7. How many σ bonds are present in the structure of a tetrahedral molecule like methane (CH₄)?
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Correct answer: B — 6
In tetrahedral geometry (sp³ hybridization), each central atom forms four equivalent σ bonds. Methane has four σ bonds.
Q8. The difference in bond energy between a single σ bond and a π bond formed by the same atoms is generally observed to be:
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Correct answer: C — larger
π bonds are generally weaker than σ bonds due to the poorer orbital overlap, thus the σ bond energy is larger.
Q9. How many sigma (σ) bonds are present in a fully saturated tetrahedral structure like methane (CH₄)?
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Correct answer: C — 5
In a tetrahedral arrangement (sp³ hybridization), the carbon atom forms four single bonds, all of which are sigma bonds.
Q10. In an ethene molecule, the carbon-carbon bond is characterized primarily by which type of bond?
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Correct answer: B — π bond
Ethene (C₂H₄) involves sp² hybridization where one sigma bond and one pi bond are formed between the carbon atoms.
Q11. The geometry adopted by a carbon atom exhibiting sp² hybridization is:
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Correct answer: C — Trigonal Planar
sp² hybridization leads to three sigma bonds and one unhybridized p-orbital, resulting in a trigonal planar geometry.
Q12. What is the hybridization of the carbon atom in methane (CH₄)?
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Correct answer: B — sp³
Methane has four sigma (σ) bonds and no lone pairs on the central carbon atom, resulting in sp³ hybridization, with bond angles of 109.5° (tetrahedral).
Q13. What is the characteristic geometry adopted by an sp² hybridized carbon atom, such as in ethene?
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Correct answer: B — Trigonal Planar
sp² hybridization involves three hybrid orbitals arranged in a plane, leading to a trigonal planar geometry with 120° bond angles.
Q14. Which hybridization state is associated with a bond angle of approximately 109.5° in organic molecules?
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Correct answer: A — sp³
The sp³ hybridization results in a tetrahedral geometry with bond angles of approximately 109.5° (e.g., in methane).
Q15. If a molecule is formed entirely by sp hybridized carbon atoms, what is the expected bond angle in its structure?
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Correct answer: C — 180°
sp hybridization corresponds to linear geometry, meaning the bond angle is 180°.
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