How do metal atoms bond with one another?

In metallic bonds, the valence electrons from the s and p orbitals of the interacting metal atoms delocalize. That is to say, instead of orbiting their respective metal atoms, they form a “sea” of electrons that surrounds the positively charged atomic nuclei of the interacting metal ions. ... Metals are shiny.

Explanation:

i took it from google

Metallic bonds are mediated by strong attractive forces. This property contributes to the low volatility, high melting and boiling points, and high density of most metals. The group-XII metals zinc, cadmium, and mercury are exceptions to this rule.

Explanation:

Metallic bonds can occur between different elements, forming an alloy. Aluminum foil and copper wire are examples of metallic bonding in action .

Metals make up most of the elements in the periodic table (around 80%), and they are special. When metals bond with themselves, they bond in a different way than when they bond with other elements. It isn't ionic or molecular or covalent. It is its own metal bond.

When metals are together, the electrons float around the atoms; they roam around the whole metal complex. They float free as though floating through a sea of electrons, much like an individual water molecule floats free in the sea. This is why it is called the electron sea model.

Each metal atom allows its electrons to roam freely, so these atoms become positively charged cations. These cations are kind of like a positively charged island and are surrounded by a sea of negatively charged electrons. It looks a bit like positively charged cations surrounded by electrons .

Most metals have very few electrons in their outermost energy shells, and some have vacant outer electron orbitals. What this means for the metal is that its valence electrons are decentralized and free to move around. Remember that in ionic bonds, the electrons transfer from one atom to another atom. In covalent bonds, the electrons are shared between atoms. In metal bonds, the electrons wander around and aren't transferred or shared. It's more of a communal thing where they belong to all the metal atoms around them.

In metallic bonds, the valence electrons from the s and p orbitals of the interacting metal atoms delocalize. That is to say, instead of orbiting their respective metal atoms, they form a “sea” of electrons that surrounds the positively charged atomic nuclei of the interacting metal ions.

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