Metallic bonds have only a superficial resemblance to ionic bonds.
One very simple model describes metals as positive ions in a sea of electrons and while this rationalises the electrical conductivity of metals it does not explain why the metals generally have high melting points.
The force that holds the lattice together is not a simple electrostatic force as in an ideal ionic lattice. In most metals some of the bonding derives from some covalent bonding between metal atoms allied with delocalised bonds occupied by free electrons.
Different models that are used are
Band theory - considering the metal lattice as a fixed lattice of positive charges and then applying a similar approach as used for the hydrogen atom - a single charged nucleus with 1 electron. This model predicts bands of "orbitals" of similar energy which are delocalised.
Molecular orbital theory / valence bond theory which employ the same techniques as used by chemists for molecues. This also predicts delocalised orbitals.
purpose to form more stable structure
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Alumin(i)um coheres by metallic bonding.
Ionic and covalent bonding involve electrons. Ionic bonding involves the loss and gain of electrons, form ions. Covalent bonding involves the sharing of electrons.
Metallic Bonding
These bonds tend to be ionic. However, all bonds are somewhere between purely ionic and purely covalent.
Ionic bonding forms compounds.
How can you compare covalent bonding and ionic bonding with soccer
It is ionic bonding because Na is sodium which is a metal and Cl is chlorine which is a nonmetal. Ionic Bonding happens between nonmetals and nonmetals.
All salts are ionic
Ionic bonding is based on electrostatic attraction between ions.
Covalent bonding involves the sharing of electrons. Ionic bonding involves the transfer of electrons.
ionic bonding
LiCl has ionic bonding. (There is no compound with a formula LiCL.)