Question 17 +CI-C=C-H The Lewis Structure Of C2HCl Molecule Is Given Above

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Question 17 +CI-C=C-H The Lewis Structure Of C2HCl Molecule Is Given Above. Which Of The Following Statements Is False For This Molecule? Your Answer: There Are Three Sigma Bonds In The Molecule. It Has A Dipole Moment. O All Three Bonds Between Carbon Atoms Are Formed By The Side-To-Side Overlap Of Pure Atomic Orbitals. Each Carbon Atom Has Two Hybrid

The correct answer and explanation is:

Correct Answer:

All three bonds between carbon atoms are formed by the side-to-side overlap of pure atomic orbitals.

Explanation:

The molecule C2HCl\text{C}_2\text{HCl} has the following structure: H-C≡C-Cl. Here’s a detailed explanation of why this statement is false and other properties of the molecule:

  1. Bonding and Hybridization:
    • Each carbon atom in the molecule has a different hybridization state. The first carbon (connected to hydrogen) is sp-hybridized, and the second carbon (connected to chlorine) is also sp-hybridized.
    • The triple bond between the two carbon atoms consists of one sigma bond and two pi bonds. The sigma bond is formed by the head-on overlap of sp orbitals from the two carbon atoms. The two pi bonds arise from the side-to-side overlap of unhybridized pp-orbitals.
  2. Nature of the Bonds:
    • The statement “All three bonds between carbon atoms are formed by the side-to-side overlap of pure atomic orbitals” is false because only the pi bonds are formed by the side-to-side overlap of pp-orbitals. The sigma bond is not formed this way; it results from the head-on overlap of hybridized sp orbitals.
  3. Dipole Moment:
    • The molecule C2HCl\text{C}_2\text{HCl} has a dipole moment because of the electronegativity difference between the atoms. Chlorine is more electronegative than carbon, creating a dipole directed toward chlorine. Additionally, the linear geometry does not cancel the dipole.
  4. Sigma Bonds in the Molecule:
    • The molecule has three sigma bonds: one between the first carbon and hydrogen, one in the carbon-carbon triple bond, and one between the second carbon and chlorine.
  5. Hybrid Orbitals:
    • Each carbon atom in the molecule has two sp-hybridized orbitals, which are used to form sigma bonds and hold lone pairs (if present).

This clear breakdown demonstrates why the statement is incorrect.

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