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Chapter 13: Problem 121

The linear structure is seen in (i) \(\mathrm{SnCl}_{2}\) (ii) \(\mathrm{NCO}^{-}\) (iii) \(\mathrm{NO}_{2}^{+}\) (iv) \(\mathrm{CS}_{2}\) (a) (i), (ii) and (iii) (b) (ii), (iii) and (iv) (c) (i), (iii) and (iv) (d) none of these

Short Answer

Expert verified
The linear structures are in (b) (ii), (iii) and (iv).

Step by step solution

01

Identify Linear Molecules

A linear molecule is one where the atoms are arranged in a straight line, often resulting in bond angles of 180 degrees. For example, molecules like carbon dioxide (CO2) are linear.
02

Examine SnCl鈧�

SnCl鈧� has a bent structure due to the presence of a lone pair on the central Sn atom, resulting in a bond angle of less than 180 degrees.
03

Examine NCO鈦� Ion

The NCO鈦� ion has a linear structure as the atoms are in a straight line due to sp hybridization, giving it a bond angle of 180 degrees.
04

Examine NO鈧傗伜 Ion

NO鈧傗伜 (nitronium ion) is also linear due to sp hybridization of the nitrogen atom, which leads to bond angles of 180 degrees.
05

Examine CS鈧�

CS鈧� is linear because the central carbon is sp hybridized, resulting in bond angles of 180 degrees.
06

Determine the Correct Answer

Based on the linear structures identified, NCO鈦�, NO鈧傗伜, and CS鈧� are linear. Therefore, the correct choice is those molecules listed under option (b) - (ii), (iii) and (iv).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Linear Molecules
Linear molecules are those in which atoms are arranged in a straight line. This geometric arrangement leads to a bond angle of exactly 180 degrees, producing a distinct straight-line appearance. Molecules achieve this structure when specific conditions like symmetrical charge distribution across the molecule are met.
Understanding linear molecules is crucial as they are one of the simplest molecular formations, often serving as a foundation for more complex molecular geometry learning. For instance:
  • In the NCO鈦� ion, the atoms are aligned linearly, forming a bond angle of 180 degrees, cementing its classification as a linear molecule.
  • The nitronium ion, NO鈧傗伜, also follows a linear structure due to the ideal bonding conditions produced by its electronic configuration.
  • In compounds like CS鈧�, the central carbon atom aligns with surrounding atoms in a linear arrangement.
Recognizing these traits will make it easier to identify other linear molecules in more complex chemistry problems.
sp Hybridization
sp hybridization is a fundamental concept explaining how atoms form linear molecules. It's a process where one s orbital and one p orbital combine to create two new equivalent orbitals known as sp hybrid orbitals. Each of these orbitals can form a bond, explaining the linear alignment of atoms.

For instance, in the NCO鈦� ion and CS鈧� molecule, the central atoms utilize sp hybridization:
  • This allows the orbitals to arrange themselves in a linear fashion, minimizing electron pair repulsions and leading to 180-degree bond angles.
  • sp hybridization is directly linked to creating the linear geometry, significantly impacting how these molecules interact and react with other substances.

Understanding how sp hybridization works is essential for predicting and explaining the behavior of linear molecules.
Bond Angles
Bond angles are the angles between adjacent lines representing bonds. They are significant as they dictate the molecule's spatial arrangement and directly influence the molecule's chemical properties.

In linear molecules such as NO鈧傗伜, NCO鈦�, and CS鈧�, the bond angles are crucial:
  • Each of these molecules has a bond angle of exactly 180 degrees鈥攁 hallmark feature of linear geometry.
  • Bond angles help distinguish between different molecular geometries, such as linear, bent, or trigonal planar, by providing insight into how atoms are spaced in a molecule.

A clear grasp of bond angles helps in understanding the steric and electronic considerations that lead to particular molecular forms, making them a vital aspect of molecular geometry.

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Most popular questions from this chapter

Among the following compounds, the one that is polar and has the central atom with sp \(^{2}\) hybridization is (a) \(\mathrm{SiF}_{4}\) (b) \(\mathrm{BF}_{3}\) (c) \(\mathrm{HClO}_{2}\) (d) \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Which one of the following statements is true? (a) The dipole moment of \(\mathrm{NF}_{3}\) is more than \(\mathrm{NH}_{3}\) (b) The dipole moment of \(\mathrm{NF}_{3}\) is less than \(\mathrm{NH}_{3}\) (c) The dipole moment of \(\mathrm{NH}_{3}\) is zero (d) The dipole moment of \(\mathrm{NF}_{3}\) is equal to \(\mathrm{NH}_{3}\)

Of the following sets which does not contain isoelectronic species? \([2005]\) (a) \(\mathrm{SO}_{3}^{2-}, \mathrm{CO}_{3}^{2-}, \mathrm{NO}_{3}^{-}\) (b) \(\mathrm{CN}^{-}, \mathrm{N}_{2}, \mathrm{C}_{2}^{2-}\) (c) \(\mathrm{BO}_{3}^{3}, \mathrm{CO}_{3}^{2-}, \mathrm{NO}_{3}^{-}\) (d) \(\mathrm{PO}_{4}^{3}, \mathrm{SO}_{4}^{2-}, \mathrm{ClO}_{4}^{-}\)

Lattice energy of an ionic compound depends upon [2005] (a) packing of ions only (b) size of the ion only (c) charge on the ion and size of the ion (d) charge on the ion only

The correct order of bond angles (smallest first) in \(\mathrm{H}_{2} \mathrm{~S}, \mathrm{NH}_{3}, \mathrm{BF}_{3}\) and \(\mathrm{SiH}_{4}\) is [2004] (a) \(\mathrm{H}_{2} \mathrm{~S}<\mathrm{SiH}_{4}<\mathrm{NH}_{3}<\mathrm{BF}_{3}\) (b) \(\mathrm{NH}_{3}<\mathrm{H}_{2} \mathrm{~S}<\mathrm{SiH}_{4}<\mathrm{BF}_{3}\) (c) \(\mathrm{H}_{2} \mathrm{~S}<\mathrm{NH}_{3}<\mathrm{SiH}_{4}<\mathrm{BF}_{3}\) (d) \(\mathrm{H}_{2} \mathrm{~S}<\mathrm{NH}_{3}<\mathrm{BF}_{3}<\mathrm{SiH}_{4}\)
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