Question

Dimethylmercury, \(\mathrm{CH}_{3}-\mathrm{Hg}-\mathrm{CH}_{3}\), is a volatile compound of bp \(96^{\circ}\), whereas mercuric fluoride \(\mathrm{F}-\mathrm{Hg}-\mathrm{F}\) is a high-melting solid having mp \(570^{\circ} .\) Explain what differences in bonding in the two substances are expected that can account for the great differences in physical properties.

Short answer

Dimethylmercury's volatility is due to weak van der Waals forces, while mercuric fluoride's high melting point is from strong ionic bonds.

Step-by-step solution

Identify the Types of Compounds

Dimethylmercury is an organometallic compound containing carbon, hydrogen, and mercury. Mercuric fluoride is an inorganic compound composed of mercury and fluorine. The bonding types in these compounds will influence their physical properties.

Analyze Dimethylmercury's Bonding

In dimethylmercury (\(\mathrm{CH}_{3}-\mathrm{Hg}-\mathrm{CH}_{3}\)), the mercury is covalently bonded to two methyl groups. The carbon-hydrogen and carbon-mercury bonds are nonpolar or slightly polar covalent bonds, resulting in weak intermolecular forces such as van der Waals forces.

Analyze Mercuric Fluoride's Bonding

Mercuric fluoride (\(\mathrm{F}-\mathrm{Hg}-\mathrm{F}\)) consists of mercury ions (Hg) bonded ionically to fluoride ions (F). The ionic bonds formed due to the complete transfer of electrons between mercury and fluorine create a strong, stable lattice structure.

Compare Intermolecular Forces

In dimethylmercury, weak van der Waals forces dominate, which are typical in volatile, low boiling point compounds. Contrarily, the strong ionic bonds in mercuric fluoride result in a rigid lattice that requires considerable energy to melt, reflecting in its high melting point.

Conclusion on Physical Properties

The volatile nature and low boiling point of dimethylmercury are due to weak intermolecular interactions (van der Waals forces). In contrast, mercuric fluoride's high melting point is due to strong ionic bonds that form a stable lattice, requiring more heat to break apart.

Key concepts

Organometallic Compounds

Organometallic compounds are fascinating structures that form when carbon-based elements bond with metal atoms. Dimethylmercury, with the formula \(\mathrm{CH}_3-\mathrm{Hg}-\mathrm{CH}_3\), exemplifies this category. These compounds often exhibit unique properties due to their dual characteristic of possessing organic and metallic bonds.

• Carbon atoms typically form covalent bonds with metals, contributing to organometallic compounds' distinct nature.
• In dimethylmercury, mercury bonds with two methyl groups (\(\mathrm{CH}_3\) units).
• The methyl groups' bonds with mercury are usually weak, influencing the compound's low boiling point and volatility.

Organometallic compounds are crucial in chemistry, often serving as catalysis tools in industrial processes.

Inorganic Compounds

Unlike organometallic compounds, inorganic compounds do not primarily focus on carbon and metal bonding. Instead, they explore the interactions between metals and various other elements, such as fluorine in mercuric fluoride (\(\mathrm{F}-\mathrm{Hg}-\mathrm{F}\)).

• These compounds are characterized by forming crystalline structures with metals and non-metals.
• They often involve ionic or electrovalent bonds, offering physical stability and high melting points.
• Mercuric fluoride, for example, forms a structured lattice, contributing to its robustness and high melting point.

Understanding inorganic compounds aids in grasping the differences in stability and reactivity.

Intermolecular Forces

Intermolecular forces are the backbone of understanding physical properties of compounds, affecting phases and stability.

• Van der Waals forces are the weakest intermolecular forces, present in dimethylmercury, accounting for its volatility.
• These forces are more prominent in compounds with nonpolar covalent bonds, where temporary dipoles cause attraction.
• In contrast, ionic compounds like mercuric fluoride experience strong electrostatic forces between charged ions.

Recognizing the role of intermolecular forces helps explain why some substances are gases, while others are solid at room temperature.

Covalent Bonds

Covalent bonds form when two atoms share electrons, creating stability in their outer electron shells. This type of bonding is prevalent in organic and some organometallic compounds.

• In dimethylmercury, mercury forms covalent bonds with carbon in the methyl groups, although these bonds are relatively weak.
• Covalent bonds can be polar or nonpolar depending on the electronegativity difference between atoms involved.
• Weaker covalent bonds contribute to lower boiling points due to lesser energy needed to overcome these bonds.

Covalent bonding's understanding offers insights into molecular structures and reactions.

Ionic Bonds

Ionic bonds are formed through the complete transfer of electrons from one atom to another, resulting in positively and negatively charged ions. This bonding leads to the formation of strong, stable compounds, such as mercuric fluoride.

• In mercuric fluoride, mercury donates and fluorine accepts electrons, establishing a strong ionic bond.
• The resulting ionic lattice structure contributes to its hardness and high melting point.
• Such strong electrostatic forces require significant energy to break, explaining mercuric fluoride's solid state.

Ionic bonds are key in creating robust materials, used in multiple industrial and technological applications.