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Which of the following statement is false? (1) Octahedral molccular shape exists in sp \(^{3} \mathrm{~d}^{2}\) hybridisation. (2) \(\mathrm{XcF}_{2}\) involves \(\$ \mathrm{p}^{3} \mathrm{~d}\) hybridisation. (3) The repulsion among four hybrid orbitals is smallest if they point to the corners of a square. (4) IIybridisation can take place only between orbitals of roughly the same energy.

Short Answer

Expert verified
The false statement is (3).

Step by step solution

01

Analyze Each Statement

Review each statement one by one to determine its validity.
02

Check Octahedral Molecular Shape

Octahedral molecular shape is associated with \( \mathrm{sp}^{3} \mathrm{~d}^{2} \) hybridization. This statement is true.
03

Verify \( \mathrm{XeF}_{2} \) Hybridization

\( \mathrm{XeF}_{2} \) has a linear structure involving \( \mathrm{sp}^{3} \mathrm{~d} \) hybridization, which makes this statement true as well.
04

Analyze Repulsions Among Hybrid Orbitals

Among the four hybrid orbitals, the repulsion is smallest if they point to the corners of a tetrahedron, not a square. So, this statement is false.
05

Hybridization Energy Levels

Hybridization generally occurs among orbitals of similar energy levels. Therefore, this statement is true.

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Key Concepts

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

sp3d hybridization
Let's start with understanding the concept of sp3d hybridization. In chemical bonding, hybridization refers to the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are crucial for explaining the shape of molecules.
For sp3d hybridization, one s-orbital, three p-orbitals, and one d-orbital mix together to form five equivalent hybrid orbitals. These hybrid orbitals arrange themselves in a specific geometry to reduce electron repulsion. This typically results in a trigonal bipyramidal shape.
An example of sp3d hybridization can be seen in molecules like phosphorus pentachloride (PCl5). Here, the geometry results from the arrangement of three equatorial atoms making a triangle and two axial atoms located above and below the plane of the equatorial atoms. This helps in minimizing repulsion and stabilizing the molecule.
octahedral molecular shape
The octahedral molecular shape is linked to sp3d2 hybridization, which involves six hybrid orbitals. These orbitals are formed by the mixing of one s-orbital, three p-orbitals, and two d-orbitals. They arrange themselves in such a way as to minimize electron repulsion.
Picture an octahedron: a three-dimensional shape with eight faces. In an octahedral molecule, six atoms or groups are positioned symmetrically around a central atom, at the corners of an octahedron.
A common example of octahedral molecular shape is sulfur hexafluoride (SF6). Here, six fluorine atoms are symmetrically arranged around a central sulfur atom. This arrangement allows for minimal repulsion between the atoms, leading to a highly stable structure.
orbital repulsion
Orbital repulsion is a fundamental concept in chemistry. It refers to the repelling force between electron pairs within orbitals. As negative charges repel each other, electron pairs tend to arrange themselves as far apart as possible to reduce repulsion.
This concept is essential in determining the shape of molecules. For example, in the case of tetrahedral geometry, the four hybrid orbitals point to the corners of a tetrahedron to minimize repulsion. The statement mentioned that repulsion is smallest if the orbitals point to the corners of a square is inaccurate. In reality, a tetrahedral arrangement minimizes repulsion better than a square.
Understanding orbital repulsion helps us accurately predict molecular shapes using Valence Shell Electron Pair Repulsion (VSEPR) theory. By considering the repulsions between bonding and non-bonding electron pairs, chemists can determine the most stable structure for a molecule.

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Most popular questions from this chapter

Jodine monochloride molecule is formed by the overlap of (1) s-s orbitals (2) s-p orbitals (3) p-d orbitals (4) \(\mathrm{p}-\mathrm{p}\) orbitals

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.

\(\mathrm{NH}_{3}\) has a net dipole moment but boron trifluoride has zero dipole moment because (1) \(\mathrm{B}\) is less electronegative than \(\mathrm{N}\) (2) \(\mathrm{F}\) is more electronegative than \(\mathrm{H}\) (3) \(\mathrm{BF}_{3}\) is pyramidal while \(\mathrm{NH}_{3}\) is planar (4) \(\mathrm{BF}_{3}\) is trigonal planar while \(\mathrm{NII}_{3}\) is pyramidal

The correct statement about resonating structure is (1) They have no real existence. (2) These are hypothetical structures. (3) These structures can never be separated. (4) All are correct.

The false statement among the following is (1) Bond energy of covalent \(0-H\) bond in water is greater than bond energy of hydrogen bond. (2) The intermolecular attractive forces vary in the order: water \(>\) ether \(>\) alcohol. (3) The high heat of vapourisation of water is due to hydrogen bonding. (4) Acetic acid exists as a dimer in benzene due to hydrogen bonding.

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