What is the hybridization of AlCl4-?
The Correct Answer and Explanation is :
The hybridization of the (\text{AlCl}_4^-) ion is sp³. Here’s a detailed explanation:
Explanation:
The (\text{AlCl}_4^-) ion consists of an aluminum (Al) atom bonded to four chlorine (Cl) atoms, and the overall charge on the molecule is negative (-1). Let’s break this down:
- Aluminum’s Electron Configuration:
Aluminum has an atomic number of 13, which means its electron configuration is ([Ne] 3s^2 3p^1). In its ground state, it has three valence electrons. - Bond Formation and Charge Distribution:
In the (\text{AlCl}_4^-) ion, the aluminum atom forms four bonds with four chlorine atoms. Chlorine atoms each provide one electron, and the negative charge on the ion indicates that an extra electron is present. So, the aluminum atom now has eight electrons in its valence shell, which it achieves by accepting one extra electron. - Electron Pairing and Hybridization:
The aluminum atom in the (\text{AlCl}_4^-) ion uses its four valence electrons (three from aluminum and one from the additional electron) to form four covalent bonds with four chlorine atoms. Since there are four bonding regions around the central aluminum atom and no lone pairs on aluminum, the aluminum atom undergoes sp³ hybridization. - Geometry:
The hybridization leads to a tetrahedral geometry around the aluminum atom. The four chlorine atoms are positioned at the corners of a tetrahedron with the aluminum atom at the center. This results in bond angles close to 109.5°, which is characteristic of a tetrahedral shape.
In summary, (\text{AlCl}_4^-) has sp³ hybridization due to the formation of four bonds and no lone pairs on the central aluminum atom, leading to a tetrahedral molecular geometry.
Now, I’ll generate an image to visualize this structure.
It looks like there was an issue generating the image. However, I can still describe the structure for you:
In the (\text{AlCl}_4^-) ion, the aluminum atom is surrounded symmetrically by four chlorine atoms. The molecule has a tetrahedral geometry, with bond angles of approximately 109.5°. This configuration ensures that the repulsion between the bonding electron pairs is minimized, which is why the molecule adopts a tetrahedral shape. The extra electron contributing to the negative charge is distributed evenly across the structure, making it stable.
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