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Chapter 1: Problem 196

Which is not corrcerly matched? Molecule \(\quad\) Shape (a) \(\mathrm{Sb}(\mathrm{Ph})_{3}\) Square pyramidal (b) \(\mathrm{T}_{\mathrm{C}} \mathrm{Cl}_{\mathrm{c}}^{2}\) Octaheriral (c) \(\mathrm{PCl}_{\text {. }}\) Octahedral (d) \(\mathrm{InCl}_{4}^{2-}\) Square planar

Short Answer

Expert verified
The incorrect match is (a) \(\mathrm{Sb}( ext{Ph})_{3}\) - Square pyramidal.

Step by step solution

01

Understand the problem

We are tasked with identifying which molecule-shape pair is incorrectly matched. We need to examine each given molecule and determine if its listed geometric shape is correct.
02

Analyze Sb(Ph)_3

The molecule \( ext{Sb(Ph)}_3\) is antimony triphenyl. Antimony typically forms a molecular geometry of trigonal pyramidal. Therefore, the given shape, square pyramidal, is incorrect for \( ext{Sb(Ph)}_3\).
03

Check TcCl_6^{2-}

The ion \(\text{TcCl}_6^{2-}\) is a complex with technetium at the center surrounded by six chloride ions. This configuration indeed corresponds to an octahedral shape, which matches the listed geometry.
04

Review PCl_6^鈭�

The ion \(\text{PCl}_6^-\) is phosphorus surrounded by six chlorine atoms. This arrangement forms an octahedral geometry, and thus the listed shape is correct.
05

Examine InCl_4^{2-}

The ion \(\text{InCl}_4^{2-}\) is indium with four chloride ions. This ion has a square planar geometry, which matches the shape provided in the question.
06

Final Step: Identify the incorrectly matched pair

Based on the analysis, the molecule \(\text{Sb(Ph)}_3\) does not match the provided shape (square pyramidal). The correct geometry for \(\text{Sb(Ph)}_3\) is trigonal pyramidal.

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Key Concepts

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

Antimony Triphenyl Geometry
Antimony triphenyl, denoted as \( \text{Sb(Ph)}_3 \), presents an intriguing example of molecular geometry. Here, 'Ph' stands for the phenyl group (\( \text{-C}_6\text{H}_5 \)). The geometry is determined by the number of bonds and lone pairs surrounding the central atom鈥攁ntimony (Sb) in this case.
Antimony commonly displays a trigonal pyramidal geometry.
  • This happens due to the three phenyl groups bonded to the antimony atom.
  • The presence of one lone pair on antimony also affects the shape.
The lone pair occupies one position, and the three phenyl groups take the other positions in a way that minimizes repulsion, leading to the trigonal pyramidal geometry. This is in contrast to the square pyramidal geometry, which actually represents a five-coordinate arrangement鈥攐ften involving different species.
Technetium Chloride Complex
The technetium chloride complex \( \text{TcCl}_6^{2-} \) is an example of an octahedral molecular geometry. This type of structure arises when six ligands (chloride ions in this case) surround a central atom, which here is technetium (Tc).
  • In an octahedral structure, all positions are equivalent, forming a symmetrical arrangement.
  • It maximizes separation between the electron pairs as per VSEPR theory, reducing repulsion.
This geometry is quite common in complexes involving transition metals with empty d-orbitals, as these orbitals can accommodate additional bonding with surrounding ligands. The symmetry leads to various interesting chemical properties and characteristics often utilized in catalysis and material sciences.
Phosphorus Chloride Ion
The phosphorus chloride ion, denoted as \( \text{PCl}_6^- \), typically adopts an octahedral geometry. With six chlorine atoms surrounding the central phosphorus atom, the structure forms a perfectly symmetrical shape.
  • This is due to the phosphorus atom using its d-orbitals to bond with six chloride ions.
  • Each chlorine occupies a vertex of the octahedron, minimizing repulsion between the electron clouds.
The presence of six identical bonds makes this structure quite stable and energetically favorable. This type of geometry is typical of hexacoordinate compounds, often found in complex ions and some molecular compounds.
Indium Chloride Ion
The indium chloride ion \( \text{InCl}_4^{2-} \) exhibits a square planar geometry. This geometric arrangement is common in ions or molecules where the central atom has a coordination number of four but sits within the same plane as the ligands.
  • In a square planar configuration, the four chloride ions are positioned at the corners of a square, with the indium atom at the center.
  • This formation minimizes electron pair repulsion, considering both bond regions and lone pairs present in some cases.
Such geometry is frequently observed in transition metal complexes that have a d8 configuration or in compounds where there's significant electronic delocalization, adding stability to the structure.

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Most popular questions from this chapter

Which of rhe following starcmenrs is ruc? (a) 'The dipole momenr of \(\mathrm{N} 1 \mathrm{t}_{3}\) is acro. (b) 1he dipole momenc of \(\mathrm{NT}_{3}\) is ecjual ro \(\mathrm{NH}_{s^{\circ}}\) (c) 'The dipole moment of \(\mathrm{NT}_{3}\) is zero. (d) "lhe dipole moment of \(\mathrm{NF}_{3}\) is less than \(\mathrm{NH}_{3}\).

The lincar strucrure is/arc assumed by (a) \(\mathrm{SnCl}_{2}\) (b) \(\mathrm{NCO}^{-}\) (c) \(\mathrm{NO}_{2}^{+}\) (d) \(\mathrm{CS}_{2}\)

\(\Lambda\) square plarar complex is formed by hybridization of the following atomic orbitals (a) \(\mathrm{s}, \mathrm{P}_{\mathrm{x}}, \mathrm{P}_{y} \mathrm{P}_{x}\) (b) \(s, p_{x}, p, p_{z}, d\) (c) \(\mathrm{dx}^{2}-y^{2}, \mathrm{~s}, \mathrm{p}, \mathrm{p}\) (d) \(\mathrm{s}, \mathrm{P}, \mathrm{p}, \mathrm{p}, \mathrm{d} z^{2}\)

'The hybrid state of central itocline atom is \(\mathrm{I}_{3}^{+}\) and \(\mathrm{I}_{3}^{-}\) are, respectively (a) \(\mathrm{sp}^{3}, \mathrm{sp}^{3} \mathrm{~d}\) (b) \(s p^{3} d, s p^{3}\) (c) \(s p^{3} d, s p^{5} d\) (d) \(\mathrm{sp}^{2}, \mathrm{sp}^{3} \mathrm{~d}\)

Which of the following is/are correct statement \((\mathrm{s}) ?\) (a) \(\mathrm{In}\left(\mathrm{CH}_{3}, \mathrm{~N}, \mathrm{C}-\mathrm{N}-C\right.\) bond angle is appraximately \(107^{\circ}\) whereas in \(\left(\mathrm{SiH}_{3}\right)_{3} \mathrm{~N}\) \(\mathrm{Si}-\mathrm{N}-\mathrm{Si}\) bond angle is appraximately \(120^{\circ}\) (b) In dilure solurion of \(\mathrm{H}_{2} \mathrm{CO}_{3}\) some \(\mathrm{C}-\mathrm{O}\) bond lengrhs arc cqual bur in \(11_{2} \mathrm{CO}_{3}(\mathrm{l}) \mathrm{all}\) \(\mathrm{C}-\mathrm{O}\) bond Icngths arc uncqual. (c) \(\mathrm{CO}_{2}\) is a monomer while \(\mathrm{SiO}_{2}\) is a rhrec dimensional gianr molecule. (d) Diamond is rhe conductor of clcctricity.
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