Question

The melting point of diamond is very high since the type of bonding in it is (1) ionic (2) Van der Waal's (3) polymeric network (4) coordinate

Short answer

Option (3) polymeric network

Step-by-step solution

- Identify the characteristic property of diamond

Diamonds have a very high melting point, which is a significant characteristic in determining the type of bonding.

- Recognize the type of bonding responsible for high melting points

High melting points are usually due to strong bonding forces within the structure. Identify which types of bonds generally have very strong interactions.

- Evaluate the given options

Consider the options provided: (1) ionic: involves electrostatic forces, quite strong(2) Van der Waal's: involves weak intermolecular forces(3) polymeric network: involves long chains of covalently bonded atoms, typically strong(4) coordinate: involves shared electron pairsEvaluate which option matches the strength observed in diamond.

- Determine the type of bonding in diamond

Diamond consists of carbon atoms each bonded to four other carbon atoms in a tetrahedral structure, forming a rigid three-dimensional network. This type of bonding is a covalent network, corresponding to option (3) polymeric network.

Key concepts

Diamond Melting Point

Diamonds are renowned for their extremely high melting point. This characteristic property is due to the intricate type of bonding within the diamond's structure. The melting point of diamond is about 4,027°C (7,280°F), which is extraordinarily high compared to many other materials. This is essential because the very high melting point indicates the presence of very strong bonds keeping the atoms in place.
Therefore, these bonds require an enormous amount of energy to break. The strength of these bonds provides a clue as to why diamonds are so resilient and maintain their structure even at high temperatures.

Covalent Network Bonding

Covalent network bonding plays a significant role in determining the properties of the diamond. In a diamond, each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral arrangement. This forms a continuous three-dimensional network of strong covalent bonds. These bonds are incredibly robust and require a lot of energy to break, contributing to the diamond's extraordinary hardness and high melting point.
The presence of this covalent network means that the atoms are held together very tightly, creating a solid that is both tough and durable. This type of bonding is different from simpler covalent bonding seen in molecules like water, where bonds are only between specific, limited pairs of atoms.

Strong Intermolecular Forces in Solids

In the context of solids like diamond, the forces that hold the atoms or molecules together are incredibly strong. Understanding these forces helps explain why some materials have high melting points and maintain their structure under extreme conditions.
The strong intermolecular forces in diamond are due to the covalent network bonding, where every carbon atom is bonded to its neighbors with very strong covalent bonds. These forces are much stronger than the van der Waals forces, which are weaker interactions found in other materials such as noble gases or organic molecules.
In summary, the strong intermolecular forces in diamond are a result of its covalent network structure. These strong forces ensure that a diamond remains solid and maintains its characteristic hardness and high melting point even under extreme conditions.