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Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 119

Many compounds of the transition-metal elements contain direct bonds between metal atoms. We will assume that the z-axis is defined as the metal–metal bond axis. (d) Sketch the energylevel diagram for the Sc2 molecule, assuming that only the 3d orbital from part (a) is important.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Transition Metals

Transition metals are elements found in the d-block of the periodic table, characterized by their ability to form variable oxidation states and complex ions. They have partially filled d-orbitals, which play a crucial role in bonding and the formation of compounds. Understanding their electronic configuration is essential for predicting their chemical behavior and the nature of metal-metal bonds.
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Energy Level Diagrams

Energy level diagrams visually represent the arrangement of electrons in an atom or molecule, showing the energy levels of different orbitals. In the context of transition metals, these diagrams help illustrate how d-orbitals are filled and how they interact during bond formation. For Sc2, focusing on the 3d orbital allows for a simplified view of the bonding interactions between the two scandium atoms.
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Metal-Metal Bonding

Metal-metal bonding occurs when two metal atoms share electrons, leading to the formation of a bond. In transition metal compounds, these bonds can involve d-orbitals, which contribute to the overall stability and properties of the molecule. Understanding the nature of these bonds is crucial for analyzing the electronic structure and reactivity of metal clusters like Sc2.
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Related Practice
Textbook Question

Sulfur tetrafluoride (SF4) reacts slowly with O2 to form sulfur tetrafluoride monoxide (OSF4) according to the following unbalanced reaction: SF4(g) + O2(g) → OSF4(g) The O atom and the four F atoms in OSF4 are bonded to a central S atom. (c) Use average bond enthalpies (Table 8.3) to estimate the enthalpy of the reaction. Is it endothermic or exothermic?

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Textbook Question

Sulfur tetrafluoride 1SF42 reacts slowly with O2 to form sulfur

tetrafluoride monoxide 1OSF42 according to the following

unbalanced reaction:

SF41g2 + O21g2¡OSF41g2

The O atom and the four F atoms in OSF4 are bonded to a

central S atom.

(e) For each of the molecules you drew in part (d), state how many

fluorines are equatorial and how many are axial.

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Textbook Question
The phosphorus trihalides 1PX32 show the following variation in the bond angle X¬P¬X: PF3, 96.3°; PCl3, 100.3°; PBr3, 101.0°; PI3, 102.0°. The trend is generally attributed to the change in the electronegativity of the halogen. (b) What is the general trend in the X¬P¬X angle as the halide electronegativity increases?
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Textbook Question
The organic molecules shown here are derivatives of benzene in which six-membered rings are 'fused' at the edges of the hexagons.

(e) Benzene, naphthalene, and anthracene are colorless, but tetracene is orange. What does this imply about the relative HOMO–LUMO energy gaps in these molecules? See the 'Chemistry Put to Work' box on orbitals and energy.
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Textbook Question

The organic molecules shown here are derivatives of benzene in which six-membered rings are 'fused' at the edges of the hexagons.

(b) Suppose you are given a sample of one of the compounds. Could combustion analysis be used to determine unambiguously which of the three it is?

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Textbook Question

Methyl isocyanate, CH3NCO, was made infamous in 1984 when an accidental leakage of this compound from a storage tank in Bhopal, India, resulted in the deaths of about 3800 people and severe and lasting injury to many thousands more. (a) Draw a Lewis structure for methyl isocyanate.

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