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The properties of simple molecular structures are primarily determined by covalent bonds, which are formed when atoms share electrons. In these structures, the atoms are held together by strong covalent bonds, resulting in distinct molecules that possess specific characteristics such as low melting and boiling points, and poor electrical conductivity in solid state.

Simple molecular structures consist of discrete molecules, often with specific shapes determined by the arrangement of atoms and the angles between the covalent bonds. The strength and nature of the covalent bonds within each molecule are fundamental in defining the chemical stability and reactivity of the substance. This strong bonding makes the individual molecules stable, but the intermolecular forces (which could include hydrogen bonds or van der Waals forces) determine the physical properties such as solubility and phase changes.

In this context, while other types of bonds like ionic, metallic, and hydrogen bonds do play critical roles in various types of structures, they do not primarily characterize simple molecular structures. Ionic bonds typically involve the electrostatic attraction between oppositely charged ions, leading to the formation of solid lattices, while metallic bonds involve a sea of delocalized electrons, which is characteristic of metals and alloys. Hydrogen bonds, on the other hand, are specific types of relatively weak interactions