Classify each of the following statements as true or false: (a) Although both molecular sol

step 1 So this question asks us to classify each of the following statements as true or false. The firs

Classify each of the following statements as true or false:...

Classify each of the following statements as true or false: $$ \begin{array}{l}{\text { (a) Although both molecular solids and covalent-network }} \\ {\text { solids have covalent bonds, the melting points of molec- }} \\ {\text { ular solids are much lower because their covalent bonds }} \\ {\text { are much weaker. }} \\ {\text { (b) Other factors being equal, highly symmetric molecules }} \\ {\text { tend to form solids with highly symmetric molecules }} \\ {\text { asymmetrically shaped molecules. }}\end{array} $$

Classify each of the following statements as true or false:

$$
\begin{array}{l}{\text { (a) Although both molecular solids and covalent-network }} \\ {\text { solids have covalent bonds, the melting points of molec- }} \\ {\text { ular solids are much lower because their covalent bonds }} \\ {\text { are much weaker. }} \\ {\text { (b) Other factors being equal, highly symmetric molecules }} \\ {\text { tend to form solids with highly symmetric molecules }} \\ {\text { asymmetrically shaped molecules. }}\end{array}
$$

Key Concepts

Molecular Solids Versus Covalent-Network Solids

This concept distinguishes two types of solids based on their bonding. Molecular solids are composed of individual molecules held together by relatively weak intermolecular forces (such as van der Waals or hydrogen bonds), whereas covalent?network solids have an extended lattice in which atoms are bonded by strong covalent bonds throughout. This difference in bonding is key when considering properties like melting point and hardness.

Intermolecular Forces Versus Intramolecular (Covalent) Bonds

Understanding the difference between the forces that hold atoms together within a molecule and the forces that hold the molecules together in a solid is essential. In molecular solids, the internal covalent bonds within the molecules are strong, but the overall melting point is low because the intermolecular forces linking separate molecules are weak. In contrast, covalent-network solids are characterized by strong covalent bonds throughout the structure, leading to much higher melting points.

Molecular Symmetry and Crystal Packing

This concept addresses how the shape and symmetry of a molecule influence the arrangement of molecules in a solid. Highly symmetric molecules tend to pack in an ordered, highly symmetric manner, which can lead to different crystallographic properties compared to the packing of asymmetrically shaped molecules. The efficiency of packing and the resulting crystal symmetry affect the macroscopic properties of the solid.

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