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Chapter 4: Problem 117

In an anti-bonding MO the clectron density is minimum (1) around one atom of the molecule (2) between the nuclei (3) at a point away from nuclci of the molecule (4) at no place

Short Answer

Expert verified
The electron density is minimum between the nuclei (option 2).

Step by step solution

01

Understand Anti-Bonding Molecular Orbitals (MOs)

Anti-bonding molecular orbitals are formed when atomic orbitals combine with destructive interference, leading to a reduction in electron density between the nuclei of the atoms involved in the bond.
02

Analyze Electron Density in Anti-Bonding MOs

In anti-bonding MOs, electron density is typically lowest in the region between the nuclei of the bonding atoms. This is due to the destructive interference that creates a node with zero electron density.
03

Identify the Correct Option

Given the options, the correct choice reflects the concept that the electron density is minimum between the nuclei in an anti-bonding MO.

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Key Concepts

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

electron density
Electron density refers to the probability of finding an electron in a specific location around an atom or molecule. It is a key concept in understanding molecular structures and bonding. In a chemical bond, electron density is typically shared between the atoms involved, but its distribution varies based on the type of molecular orbital.
In anti-bonding molecular orbitals, electron density is significantly altered due to specific interactions we're about to explore.
molecular orbitals
Molecular orbitals are regions in a molecule where electrons are likely to be found. They are formed through the combination of atomic orbitals from bonded atoms. There are two main types of molecular orbitals: bonding and anti-bonding.
  • Bonding Molecular Orbitals: These are formed when atomic orbitals combine constructively. This means they overlap in a way that increases electron density between the nuclei, stabilizing the molecule.
  • Anti-Bonding Molecular Orbitals: Here, atomic orbitals combine through destructive interference. This leads to a node where electron density is zero, typically between the nuclei of the atoms. These orbitals can often destabilize the molecule as a result.
The behavior of electrons in these orbitals explains many chemical properties and reactions.
destructive interference
Destructive interference occurs when two waves combine in such a way that they cancel each other out. In the context of molecular orbitals, this happens when electron waves from atomic orbitals overlap destructively.
In anti-bonding molecular orbitals, destructive interference leads to a reduction in electron density between the nuclei. This is why electron density is lowest at the node in these orbitals.
Understanding this concept helps to explain why anti-bonding orbitals are higher in energy compared to bonding orbitals. This higher energy state is less stable, which is why electrons tend to preferentially fill bonding orbitals first.

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Most popular questions from this chapter

Regarding hybridisation which is incorrect? (1) \(\mathrm{BF}_{3}, \mathrm{C}_{2} \mathrm{H}_{4}, \mathrm{C}_{6} \mathrm{H}_{6}\) involves sp \(^{2}\) hybridisation. (2) \(\mathrm{BeF}_{2}, \mathrm{C}_{2} \mathrm{H}_{2}, \mathrm{CO}_{2}\) involves sp hybridisation. (3) \(\mathrm{NH}_{3}, \mathrm{H}_{2} \mathrm{O}, \mathrm{CCl}_{4}\) involves sp \(^{3}\) hybridisation. (4) \(\mathrm{CH}_{4}, \mathrm{C}_{2} \mathrm{H}_{4}, \mathrm{C}_{2} \mathrm{H}_{2}\) involves \(\mathrm{sp}^{2}\) hyoridisation.

Which of the following conditions is not correct for resonating structures? (1) The contributing structures must have the same number of unpaired electrons. (2) The contributing structures should have similar energies. (3) The contributing structures should be so written that unlike charges reside on atoms that are far apart. (4) The positive charge should be present on the electropositive clement and the negative charge on the electroncgative clement.

Which statement is wrong? (1) IIybridisation is the mixing of atomic orbitals prior to thcir combining into molecular orbitals. (2) sp \(^{2}\) hybrid orbitals are formed from two \(\mathrm{p}\) - and one s-atomic orbitals. (3) sp \(^{3} \mathrm{~d}\) hybrid orbitals are all at \(90^{\circ}\) to one another. (4) \(\mathrm{sp}^{3} \mathrm{~d}^{2}\) hybrid orbitals are directed towards the corners of the regular octahedron.

A covalent bond is formed between the atoms by the overlapping of orbitals containing (1) a single electron (2) paired electron (3) single electrons with parallel spin (4) single electron with opposite spin

\(\mathrm{PCH}_{5}\) exists but \(\mathrm{NCl}_{5}\) does not exist because (1) Nitrogen has no vacant \(2 \mathrm{~d}\) -orbitals. (2) NCls is unstable. (3) Nitrogen atom is much smaller than p. (4) Nitrogen is highly inert.
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