/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 4 A square planar complex is forme... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 4

A square planar complex is formed by hybridizationof the following atomic orbitals: (a) s, \(\mathrm{p}_{\mathrm{x}}, \mathrm{p}_{\mathrm{y}}, \mathrm{p}_{\mathrm{z}}\) (b) s, \(p_{x}, p_{y}, p_{z}, d\) (c) \(\mathrm{d}_{\mathrm{x}}^{2-2}{\mathrm{y}}^{2-\mathrm{s}}, \mathrm{p}_{\mathrm{x}}, \mathrm{p}_{\mathrm{y}}\) (d) s, p \(_{x}, p_{y}, p_{z}, d_{z}^{2}\)

Short Answer

Expert verified
None of the options correspond to the correct square planar hybridization.

Step by step solution

01

Identify Hybridization in Square Planar

In a square planar complex, the central atom typically uses dsp^2 hybridization. This involves one s-orbital, two p-orbitals, and one d-orbital.
02

Evaluate Option (a)

The hybridization configuration s, p_x, p_y, p_z involves one s-orbital and three p-orbitals, which forms a tetrahedral or trigonal planar hybridization rather than square planar, since it lacks a d-orbital.
03

Evaluate Option (b)

The hybridization configuration s, p_x, p_y, p_z, d includes an extra orbital from the p-orbitals and an additional d-orbital, which is unnecessary for a square planar geometry, making it incompatible.
04

Evaluate Option (c)

The hybridization configuration d_{x^2-y^2}, p_x, p_y lacks an s-orbital and prefers a trigonal planar geometry, which does not match square planar hybridization.
05

Evaluate Option (d)

The hybridization configuration s, p_x, p_y, p_z, d_{z^2} includes an additional p-orbital leading to an incorrect geometry similar to dsp^3 for octahedral, unsuitable for square planar complexes.
06

Conclusion: Identify the Correct Option

None of the given options align correctly with the dsp^2 hybridization required for a square planar complex.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

dsp^2 hybridization
In coordination chemistry, one fascinating aspect is hybridization, which plays a crucial role in determining the shape of a molecule. For square planar complexes, the central atom undergoes \(dsp^2\) hybridization. This means it combines one s-orbital, two p-orbitals, and one d-orbital from its electron configuration.Let's break this down:
  • The s-orbital is spherical, contributing to the symmetry of the hybridized orbitals.
  • The two p-orbitals, p_xand p_y,are aligned to form a plane, benefitting molecular planarity.
  • The d-orbital involved is specifically {d_{x^2-y^2}}.This orbital is crucial as it extends along the axes, making it ideal for planar arrangements.
Together, these orbitals form four equivalent hybrid orbitals directed 90掳 apart, enabling bonding in a square planar shape. This specific hybridization is prominent in complexes containing metals like platinum or gold.
coordination chemistry
Coordination chemistry is the field of chemistry concerned with the study of coordination compounds. These are unique structures formed by a central metal atom bonded to surrounding ligands. Coordination complexes are defined by:
  • Central Atom: Often a metal, it acts as a focal point around which ligands arrange themselves.
  • Ligands: Molecules or ions that attach through their lone electron pairs to the metal center, creating a coordination bond.
  • Coordination Number: This is the number of ligand bonds to the central atom, significantly influencing the geometry and stability of the complex.
Understanding these key aspects helps in predicting and explaining the behavior and formation of complex ions, dyes, catalysts, and even biological molecules like hemoglobin.
molecular geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. This configuration directly influences the physical and chemical properties of the compound. For square planar complexes:
  • Geometry Shape: Atoms are organized in a flat square, with the metal atom at the center.
  • Planarity: All atoms lie on the same plane, which is critical for the complex's stability and reactivity.
  • Angles: The angles between bonds are 90掳, characteristic of square geometries.
The accessibility of the square planar shape makes it a preferred geometry in materials used in pharmaceuticals and electronic devices. It influences interactions with enzymes or other substrates, making these complexes crucial in drug design.
d-orbitals involvement
The involvement of d-orbitals is pivotal in forming square planar complexes. Unlike other geometries, square planar complexes specifically utilize the d_{x^2-y^2}d-orbital. Key points about this orbital:
  • Orientation:The d_{x^2-y^2}d-orbital is oriented along the x- and y-axis in a plane. It allows for strong bonding with surrounding ligands.
  • Energetic Preference: This orbital's spatial alignment contributes to minimizing electron repulsion, enabling stability in electron-rich environments.
  • Metallicity: The use of d-orbitals gives these complexes distinctive magnetic and electronic properties, making them essential in fields that range from catalysis to quantum computing.
The distinct role of d-orbitals highlights their importance in molecular bonding and geometry, shedding light on why certain metals form specific geometric patterns.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The acid having \(\mathrm{O}\) - \(\mathrm{O}\) bond is: (a) \(\mathrm{H}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) (b) \(\mathrm{H}_{2} \mathrm{~S}_{2} \mathrm{O}_{6}\) (c) \(\mathrm{H}_{2} \mathrm{~S}_{2} \mathrm{O}_{8}\) (d) \(\mathrm{H}_{2} \mathrm{~S}_{4} \mathrm{O}_{6}\)

Which of the following is a linear molecule? (a) \(\mathrm{SO}_{2}\) (b) \(\mathrm{CH}_{4}\) (c) \(\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{BeCl}_{2}\)

The paramagnetism of \(\mathrm{O}_{2}{ }^{+}\) is due to the presence of an odd electron in the MO (a) \(\sigma^{*} 2 \mathrm{~s}\) (b) \(\pi 2 \mathrm{py}\) (c) \(\sigma^{*} 2 \mathrm{px}\) (d) \(\pi^{*} 2 \mathrm{py}\)

Among the following compounds, the one that is polar and has the central atom with sp2 hybridization is: (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (b) \(\mathrm{SiF}_{4}\) (c) \(\mathrm{BF}_{3}\) (d) \(\mathrm{HClO}_{2}\)

Which one of the following molecules contains both ionic and covalent bonds? (a) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (b) \(\mathrm{K}_{2} \mathrm{SO}_{4}\) (c) \(\mathrm{BeCl}_{2}\) (d) \(\mathrm{SO}_{2}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.