According to the Valence Bond Theory, sigma bonding involves the overlap of atomic orbitals. In the case of [Zn(H2O)6]2+, the metal involved is Zinc (Zn).

1. Identify the atomic orbitals of Zinc: Zinc is in the 4th period, d block, group 12 of the periodic table. Its electron configuration ends in 4s2 3d10. However, when Zinc loses two electrons to become Zn2+, the electron configuration becomes 4s0 3d10.

2. Identify the type of bonding: The Zn2+ ion is surrounded by six water molecules, forming a complex ion. The bonding in such complexes involves the donation of a lone pair of electrons from the oxygen atom in water to the empty 4s and 4p orbitals of the Zinc ion. This is a type of coordinate or dative bonding.

3. Identify the orbitals involved in bonding: The orbitals involved in this sigma bonding are the empty 4s and 4p orbitals of the Zinc ion and the filled orbitals of oxygen that contain the lone pair of electrons.

So, in [Zn(H2O)6]2+, the Zinc 4s and 4p orbitals would be involved in sigma bonding according to valence bond theory.

Question

According to the Valence Bond Theory, sigma bonding involves the overlap of atomic orbitals. In the case of [Zn(H2O)6]2+, the metal involved is Zinc (Zn).

1. Identify the atomic orbitals of Zinc: Zinc is in the 4th period, d block, group 12 of the periodic table. Its electron configuration ends in 4s2 3d10. However, when Zinc loses two electrons to become Zn2+, the electron configuration becomes 4s0 3d10.

2. Identify the type of bonding: The Zn2+ ion is surrounded by six water molecules, forming a complex ion. The bonding in such complexes involves the donation of a lone pair of electrons from the oxygen atom in water to the empty 4s and 4p orbitals of the Zinc ion. This is a type of coordinate or dative bonding.

3. Identify the orbitals involved in bonding: The orbitals involved in this sigma bonding are the empty 4s and 4p orbitals of the Zinc ion and the filled orbitals of oxygen that contain the lone pair of electrons.

So, in [Zn(H2O)6]2+, the Zinc 4s and 4p orbitals would be involved in sigma bonding according to valence bond theory.

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According to the Valence Bond Theory, sigma bonding involves the overlap of atomic orbitals. In the case of [Zn(H2O)6]2+, the metal involved is Zinc (Zn).

1. Identify the atomic orbitals of Zinc: Zinc is in the 4th period, d block, group 12 of the periodic table. Its electron configuration ends in 4s2 3d10. However, when Zinc loses two electrons to become Zn2+, the electron configuration becomes 4s0 3d10.

2. Identify the type of bonding: The Zn2+ ion is surrounded by six water molecules, forming a complex ion. The bonding in such complexes involves the donation of a lone pair of electrons from the oxygen atom in water to the empty 4s and 4p orbitals of the Zinc ion. This is a type of coordinate or dative bonding.

3. Identify the orbitals involved in bonding: The orbitals involved in this sigma bonding are the empty 4s and 4p orbitals of the Zinc ion and the filled orbitals of oxygen that contain the lone pair of electrons.

So, in [Zn(H2O)6]2+, the Zinc 4s and 4p orbitals would be involved in sigma bonding according to valence bond theory.

What metal orbitals would be involved in sigma bonding according to valence bond theory in[Zn(H2O)6]2+

Question

What metal orbitals would be involved in sigma bonding according to valence bond theory in `Zn(H2O)6^{2+}`?

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