Question

according to the physical properties chart, what are the properties of this type of compound? ionic compounds: higher melting points and boiling points, hard, brittle solids, often high solubility in water, conduct electricity when dissolved in water, always solids, ex. nacl, mgo. covalent compounds - covalent network: high melting points, hard, solids, non - conducting, ex. diamond (carbon), sio2. molecular solids: low boiling points and melting points, do not conduct electricity, ex. nh3, wax. metallic compounds: electrical conductors (because of the “sea of electrons”), ductile, malleable, vary in melting points, ex. fe, mg

Explanation:

The chart lists physical - property differences among ionic, covalent (network and molecular), and metallic compounds. It details melting/boiling points, hardness, conductivity, and solubility characteristics for each type.

Answer:

Ionic Compounds: Higher melting and boiling points, hard - brittle solids, often high water solubility, conduct electricity when dissolved in water, always solids (e.g., NaCl, MgO).
Covalent Network Compounds: High melting points, hard, solids, non - conducting (e.g., diamond, SiO₂).
Covalent Molecular Solids: Low boiling and melting points, do not conduct electricity (e.g., NH₃, wax).
Metallic Compounds: Electrical conductors, ductile, malleable, vary in melting points (e.g., Fe, Mg).