NEET Chemistry: Bond length Practice Questions

Correct answer: D — Increase

As the size of the participating atomic orbitals increases, the spatial extent of the overlap between them increases, leading to a longer distance between the nuclei, thus increasing the bond length.

Correct answer: A — H₂O

In H₂O, oxygen forms two bonds (O-H), while in H₂S, sulfur forms two bonds (S-H). Sulfur is larger than oxygen. Generally, for a given bond type, the bond length in H₂O is slightly shorter than in H₂S due to differences in atomic size and orbital overlap characteristics, though the difference is subtle.

Correct answer: D — Triple bond

As the number of shared electron pairs increases (single < double < triple), the bond becomes stronger and shorter due to increased orbital overlap.

Correct answer: A — Larger atomic radii

Larger atomic radii mean the valence orbitals are more diffuse and extend further out. This increased distance between the nuclei leads to a longer bond length, assuming constant orbital overlap.

Correct answer: B — Bond length decreases

Increasing the bond order means sharing more electrons between the atoms. This increased attraction results in a stronger bond and a shorter equilibrium bond length.

Correct answer: C — Higher bond order leads to shorter bond length

Higher bond order implies more shared electrons and stronger attraction, resulting in a shorter internuclear distance (shorter bond length).

Correct answer: B — Formation of a triple bond

Formation of a triple bond (highest bond order) involves the maximum number of shared electrons, leading to the strongest attractive forces and the shortest possible bond length among the possible allotropes.

Correct answer: C — Triple bond

Bond order increases with the number of shared electron pairs. Thus, a triple bond (bond order 3) involves more shared electrons than a double bond (bond order 2) or a single bond (bond order 1), leading to a shorter bond length.

Correct answer: D — The distance between the nuclei of two bonded atoms

Bond length is defined as the average distance between the nuclei of the two atoms that are connected by a covalent bond.

Correct answer: C — sp² hybridization

sp² hybridization involves a greater overlap between atomic orbitals (and potentially involves fewer electron domains in the plane) compared to sp³ hybridization, often leading to shorter, stronger bonds, although the exact comparison depends heavily on the specific molecular context.

Correct answer: D — Bond length is inversely proportional to bond order.

Bond length is inversely proportional to bond order. As the bond order (the number of shared electron pairs) increases, the attraction between the nuclei increases, causing the bond to shorten, thus decreasing the bond length.

Correct answer: D — All bonds will have equal length

In general, increasing the bond order leads to a shorter bond length because the increased number of shared electron pairs results in a stronger attraction between the nuclei. Therefore, the triple bond (A–D) will have the shortest bond length.

Correct answer: C — The atomic size of the constituent atoms

Bond length is dictated by the extent of orbital overlap, which is strongly influenced by the size of the atomic orbitals involved, hence atomic size is a primary factor.

Correct answer: A — Triple bond

Bond length decreases as the number of shared electron pairs (bond order) increases. Triple bonds involve the sharing of three electron pairs, resulting in the shortest bond length compared to single or double bonds between the same pair of atoms.

Correct answer: A — Triple bond.

Multiple bonds (double and triple) involve the sharing of more electron pairs between the atoms, leading to a greater overall attraction and shorter internuclear distance (shorter bond length).