1. Low electrical and thermal conductivity: Nonmetals are poor conductors of electricity and heat.
2. High ionization energy: Nonmetals require a significant amount of energy to remove electrons, making them relatively stable in terms of electron configuration.
3. High electronegativity: Nonmetals have a strong tendency to attract electrons from other atoms, making them highly electronegative.
4. Brittle solid state: Nonmetals tend to be brittle in their solid state, meaning they break easily upon the application of force.
5. Molecular bonding: Nonmetals often form covalent bonds with other nonmetals, sharing electrons to achieve a stable configuration.
6. Variety of physical states: Nonmetals can exist in different states of matter at room temperature, such as gases (e.g., oxygen, nitrogen), liquids (e.g., bromine), or solids (e.g., carbon, sulfur).
Oxygen, specifically, is a highly reactive nonmetal that forms diatomic molecules (O2) in its elemental state. It is vital for various processes, including respiration in organisms and combustion of fuels. Oxygen is also widely used in industrial processes, such as steel production and manufacturing of plastics, due to its oxidizing properties.
