Final answer:
Ionic bonds lead to crystal lattice formation in compounds such as sodium chloride, due to electrostatic attractions between ions. Covalent bonds are found in network solids like diamond, creating strong, directional bond networks. Metallic bonds in metals and intermolecular forces in molecular crystals also contribute to lattice structures.
Step-by-step explanation:
The type of bond that leads to crystal lattice formation within its compounds is primarily the ionic bond. Atoms in ionic crystals, such as sodium chloride, are held together by the electrostatic attraction between the positively charged cations and negatively charged anions. This strong electrostatic force results in a highly ordered ionic lattice structure.
Another type of bond that can lead to lattice formation is the covalent bond, found in covalent network solids like diamonds. Here, each carbon atom is linked to four others in a tetrahedral structure, forming an extensive network of strong, directional covalent bonds that contribute to the overall stability of the crystal lattice.
Metallic bonds are also responsible for crystal lattice formation, as seen in metals, where the positive metal ions are embedded in a sea of delocalized electrons. This allows for a metallic crystal lattice that is both strong and malleable.
Lastly, molecular crystals, which are held together by intermolecular forces such as hydrogen bonds, dipole-dipole interactions, and London dispersion forces, also form lattice arrangements but are generally weaker and possess lower melting and boiling points compared to ionic and covalent crystal lattices.