copper and chlorine are likely to form a metallic bond, right?
Metallic bonding occurs between atoms with low electronegativities (low tendency to attract electrons from other atoms) and low ionization energies (little energy required to remove electrons from the atoms). The low tendency for the metallic atoms to keep their electrons allow their electrons to be shared between the atoms, which thus become cations. The cations tend to be very closely-packed; they are not repulsed by their similar positive charges, but attracted to the electrons flowing freely between the cations.
Metallic bonding therefore occurs between copper atoms, which have low electronegativity and ionization energy. Chlorine atoms have some of the highest electronegativity and ionization energy of all elements, and thus do not exhibit metallic bonding.So the answer would be No.
Copper and chlorine are not likely to form a metallic bond. Metallic bonds occur between metal atoms, where the valence electrons are delocalized and shared among all the atoms in the metallic lattice. Copper is a metal, but chlorine is a non-metal. Instead, copper and chlorine are more likely to form an ionic bond.
To determine the bonding between copper and chlorine, we can check the electronegativities of the elements. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Copper has an electronegativity value of around 1.9, while chlorine has an electronegativity value of approximately 3.0. The difference in electronegativity values between these elements suggests that there will be a transfer of electrons from copper to chlorine, resulting in an ionic bond.
In an ionic bond, copper will lose one or two electrons to achieve a stable electron configuration, becoming a copper ion with a positive charge (Cu+ or Cu2+). Chlorine will gain one or two electrons, becoming chloride ions with a negative charge (Cl- or Cl2-). These ions will then be attracted to each other due to their opposite charges, forming an ionic bond.