To explain why the enthalpy of vaporization of vanadium (460 kJ/mol) is much larger than that of zinc (114 kJ/mol) Concept introduction: Molecular orbital theory is determining to the molecular structure in which electrons are not assigned to individual bonds between atoms, but are treated as moving under the influence of the nuclei in the whole molecule. The spatial and energetic properties of electrons within atoms are fixed by quantum mechanics to form orbitals that contain these electrons. While atomic orbital contain electrons ascribed to a single atom, molecular orbitals, which surround a number of atoms in a molecule, contain valence electrons between atoms. To explain: The enthalpy of vaporization of vanadium (460 kJ/mol) is much larger than that of zinc (114 kJ/mol)

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Chapter 21, Problem 21.132CP

Interpretation Introduction

Interpretation:

To explain why the enthalpy of vaporization of vanadium (460 kJ/mol) is much larger than that of zinc (114 kJ/mol)

Concept introduction:

Molecular orbital theory is determining to the molecular structure in which electrons are not assigned to individual bonds between atoms, but are treated as moving under the influence of the nuclei in the whole molecule. The spatial and energetic properties of electrons within atoms are fixed by quantum mechanics to form orbitals that contain these electrons. While atomic orbital contain electrons ascribed to a single atom, molecular orbitals, which surround a number of atoms in a molecule, contain valence electrons between atoms.

To explain:

The enthalpy of vaporization of vanadium (460 kJ/mol) is much larger than that of zinc (114 kJ/mol)

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