Amorphous solids are isotropic, meaning their properties are the same in all directions, unlike crystalline solids.

Covalent network solids, such as diamond, have very high melting points due to the strong covalent bonds throughout the structure.

Iron (Fe) is an example of a metallic solid, characterized by its metallic bonding and properties.

Iodine (I2) is an example of a molecular solid, where molecules are held together by van der Waals forces.

FeO is an example of a non-stoichiometric solid because it can have varying ratios of iron and oxygen.

Crystalline solids exhibit anisotropy, meaning their properties vary with direction, while isotropy refers to uniform properties in all directions.

Ionic solids do not conduct electricity in the solid state; they conduct when melted or dissolved in water.

Brittleness is not a property of metals; they are typically malleable and ductile.

Quadratic is not a recognized type of crystal system; the correct systems include cubic, tetragonal, hexagonal, orthorhombic, and others.

Amorphous solids do not have a long-range order and are not classified as crystalline solids.

Covalent network solids are typically brittle due to the strong covalent bonds that do not allow for easy deformation.

Ionic solids are typically brittle due to the strong electrostatic forces between the ions, which cause them to shatter when force is applied.

Metallic solids are known for their high electrical conductivity due to the presence of free-moving electrons.

Covalent solids exhibit a high degree of anisotropy due to their directional bonding.

Metallic solids have high thermal conductivity due to the presence of free-moving electrons.

The face-centered cubic (FCC) structure has the highest packing efficiency of approximately 74%.

Covalent network solids, such as diamond, have the highest melting points due to the strong covalent bonds throughout the structure.

The cubic crystal system has the highest symmetry among all crystal systems.

Molecular solids are composed of molecules held together by van der Waals forces and have a definite melting point.

Crystalline solids have a definite melting point due to their ordered structure, unlike amorphous solids which melt over a range of temperatures.