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Types Of Bonding

Types of Bonding

Atoms form molecules because atoms want to have a full outer

valence shell. This means that they usually will have eight electrons

in their outer shells (s and p sublevels). If atoms gain or lose

electrons, then they will form ionic bonds. If atoms share electrons,

then they have covalent bonds.

Ionic bonds occur between metals and non-metals (high difference

between electronegative values). Metal loses electrons (cation) and

non-metals gain electrons (anion).

Covalent bonds occur when two atoms are sharing electrons. Each

atom counts the shared pair of electrons in its valence shell, thereby

fulfilling the octet rule. THE NUMBER OF COVALENT BONDS

THAT AN ATOM CAN FORM IS THE SAME AS THE NUMBER

OF ELECTRONS IN ITS VALENCE SHELL.

Metallic bonds are the third type of bond, ones that hold the atoms

together in a metallic solid. In this type of bond (and with atoms in

molecules) the positive nucleus of each atom in the metallic solid is

attracted to the electrons of the atoms that surround it. The attractions

(governed by Coulomb’s Law), combined with overlapping valence

shells orbitals of the atoms result in the formation of the metallic

bonds. These bonds allow the electrons to flow around the nuclei and

create a “sea of electrons” that are able flow around the metal. This is

the reason why metals conduct electricity very well.

The crystal lattice is a structure wherein

which each atom shares electrons with the

12 atoms that it touches and forms metallic

bonds with them.

The valence electrons are free to flow

between the atoms. This is known as

“delocalized” electrons – the electrons are not

“owned” by any one atom.

Types Of Bonding