Flexi Says: Metallic bonds are forces of attraction between positive metal ions and the valence electrons that are constantly moving around them. The valence electrons include their own and those of other nearby ions of the same metal. The valence electrons of metals move freely in this way because metals have relatively low electronegativity or attraction to electrons. The positive metal ions form a lattice-like structure held together by all the metallic bonds. The electrostatic forces that hold this structure together are relatively strong, so metals tend to have high melting points. This explains why most metals are solids at room temperature.