Why are metals solid at room temperature?

Metals are solid at room temperature primarily because they are held together by strong electrostatic forces between metal atoms. In metallic bonding, atoms in a metal lose some of their electrons, which become delocalized and create a 'sea of electrons' around positively charged metal ions. This arrangement allows for a strong attraction between the metal ions and the delocalized electrons, resulting in a stable structure that remains solid at room temperature.

The presence of these strong electrostatic forces provides the metal with structural integrity, preventing the atoms from moving freely and maintaining a solid state. This characteristic is a defining trait of metals, contributing to their physical properties such as malleability, ductility, and high melting points.

Other options do not accurately describe the properties of metals. Weak interatomic forces would not be sufficient to keep the metal solid. Strong covalent bonds are particular to certain non-metals and do not apply to the bonding characteristics of metals. The statement about metals forming gas at room temperature contradicts the well-known fact that most metals are solid at this temperature. Therefore, the role of strong electrostatic forces in maintaining the solid state of metals is essential for understanding their behavior at room temperature.