What type of bond is typically found in metals due to electrons being freely shared?

The type of bond typically found in metals is a metallic bond, which is characterized by a unique structure where electrons are not bound to any specific atom but are instead delocalized and move freely throughout the metal lattice. This "sea of electrons" allows for the conduction of electricity and heat, as well as providing metals with their malleability and ductility.

In metallic bonding, metal atoms release some of their electrons to form a collective pool, which contributes to the strength of the bond and the properties that define metallic substances. The interaction between the positively charged metal ions and the negatively charged delocalized electrons creates a strong bond that holds the metal atoms together. This is in contrast to other types of bonds. For example, covalent bonds involve the sharing of pairs of electrons between specific atoms, while ionic bonds result from the electrostatic attraction between positively and negatively charged ions formed by the transfer of electrons. Polar covalent bonds involve unequal sharing of electrons between atoms with different electronegativities.

Thus, the definition and properties of metallic bonds directly explain why the correct answer is C, as it aptly describes the behavior of electrons in metals.