Based on valence bond theory , which set of orbitals is used by a period 4 metal ion in forming a square planar complex has to be explained. Concept introduction: According to valence bond theory, complex ions have coordinate covalent bonds between Ligands (Lewis bases) and metal ions (Lewis acids). A coordinate covalent bond is a bond formed when both electrons came from one atom. Valence bond theory, which helps explain bonding and structure in main-group compounds (can also be used to describe bonding in complex ions. In the formation of a complex ion, the filled ligand orbital overlaps an empty metal-ion orbital: the ligand (Lewis base) donates an electron pair, and the metal ion (Lewis acid) accepts it to form a covalent bond in the complex ion (Lewis adduct). A bond in which one atom contributes both electrons is a coordinate covalent bond; once formed, it is identical to any covalent single bond. The VB concept of hybridization proposes mixing particular combinations of s , p , a n d d orbitals to obtain sets of hybrid orbitals, which have specific geometries. Let’s discuss orbital combinations that lead to octahedral, square planar, and tetrahedral geometries.

Question

Want to see the full answer?

Answer 1

Question

Chapter 23, Problem 23.71P

(a)

Interpretation Introduction

Interpretation:

Based on valence bond theory, which set of orbitals is used by a period 4 metal ion in forming a square planar complex has to be explained.

Concept introduction:

According to valence bond theory, complex ions have coordinate covalent bonds between

Ligands (Lewis bases) and metal ions (Lewis acids).

A coordinate covalent bond is a bond formed when both electrons came from one atom.

Valence bond theory, which helps explain bonding and structure in main-group compounds (can also be used to describe bonding in complex ions.

In the formation of a complex ion, the filled ligand orbital overlaps an empty metal-ion

orbital: the ligand (Lewis base) donates an electron pair, and the metal ion (Lewis acid)

accepts it to form a covalent bond in the complex ion (Lewis adduct).

A bond in which one atom contributes both electrons is a coordinate covalent bond; once

formed, it is identical to any covalent single bond.

The VB concept of hybridization proposes mixing particular combinations of s,p, and d orbitals to obtain sets of hybrid orbitals, which have specific geometries.

Let’s discuss orbital combinations that lead to octahedral, square planar, and tetrahedral geometries.

(b)

Interpretation Introduction

Interpretation:

Based on valence bond theory, which set of orbitals is used by a period 4 metal ion in forming a tetrahedral complex has to be explained.

Concept introduction:

According to valence bond theory, complex ions have coordinate covalent bonds between

Ligands (Lewis bases) and metal ions (Lewis acids).

A coordinate covalent bond is a bond formed when both electrons came from one atom.

Valence bond theory, which helps explain bonding and structure in main-group compounds (can also be used to describe bonding in complex ions.

In the formation of a complex ion, the filled ligand orbital overlaps an empty metal-ion

orbital: the ligand (Lewis base) donates an electron pair, and the metal ion (Lewis acid)

accepts it to form a covalent bond in the complex ion (Lewis adduct).

A bond in which one atom contributes both electrons is a coordinate covalent bond; once

formed, it is identical to any covalent single bond.

The VB concept of hybridization proposes mixing particular combinations of s,p, and d orbitals to obtain sets of hybrid orbitals, which have specific geometries.

Let’s discuss orbital combinations that lead to octahedral, square planar, and tetrahedral geometries.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Potential Energy (kJ) 1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. AH = -950 kJ AH = 575 kJ (i) Cl₂ (g) + Pt (s) 2C1 (g) + Pt (s) Ea = 1550 kJ (ii) Cl (g)+ CO (g) + Pt (s) → CICO (g) + Pt (s) (iii) Cl (g) + CICO (g) → Cl₂CO (g) Ea = 2240 kJ Ea = 2350 kJ AH = -825 kJ 2600 2400 2200 2000 1800 1600 1400 1200 1000 a. Draw the potential energy diagram for the reaction. Label the data points for clarity. The potential energy of the reactants is 600 kJ 800 600 400 200 0 -200- -400 -600- -800- Reaction Progress

Can u help me figure out the reaction mechanisms for these, idk where to even start

Hi, I need your help with the drawing, please. I have attached the question along with my lab instructions. Please use the reaction from the lab only, as we are not allowed to use outside sources. Thank you!