1. hybridisation
Some atoms form a different number of covalent bonds than the electron configurations of those atoms might suggest they should form.

2. hybridisation
In general, when we look at the electron configuration for an atom, we can infer they type of bonding that it will undergo. However, certain atoms like carbon, beryllium, and boron, react differently than is expected.

3. hybridisation
Carbon has an electron configuration of 1s22s22p2. That indicates that there are 4 electrons in its valence shell. The 2s orbital is full, and there are there are 2 half-filled p-orbitals.

4. hybridisation
The two half-filled p-orbitals would suggest that carbon would form two covalent bonds. However, scientific research proves otherwise.

5. hybridisation
It appears that carbon will “promote” one of the electrons from the 2s orbital to the 2p orbital, leaving it with 4 half-filled orbitals. This gives carbon the ability to form 4 covalent bonds.

6. hybridisation
Chemists describe this unusual behavior as hybridisation. Hybridisation is the rearrangement of electrons within the valence orbitals of atoms during a chemical reaction.

7. Hybridisation
In carbon, the four half-filled orbitals all have identical energies, and each is referred to as an sp3 hybrid orbital. There are a total of 4 sp3 hybrid orbitals, as is illustrated by adding the superscripts (a 1 is assumed for the s).

8. Hybridisation
Once hybridisation has taken place, any one of the four is equivalent to any other. All four orbitals have new bond characteristics that are different from the characteristics of the s and p orbitals.

9. hybridisation
hybridisation also occurs in compounds of beryllium. The electron configuration if Be is 1s22s2. It would appear to have no half-filled orbitals with which to form covalent bonds.

10. hybridisation
However, Be can form 2 covalent bonds by “promoting” one of the electrons in the 2s orbital into the 2p orbital, giving it 2 half-filled orbitals.

11. hybridisation
The new half-filled orbitals formed by Be are referred to as sp hybrid orbitals. There are 2 sp hybrid orbitals.

12. hybridisation
Boron also undergoes a type of hybridisation. The electron configuration of B is 1s22s22p1. Boron will promote one of the 2s electrons, giving it 3 half-filled orbitals in its valence shell, allowing it to form 3 covalent bonds.

13. hybridisation
This kind of hybridisation is referred to as sp2 hybridisation.

14. Metallic Bonding
Metallic atoms, which have few valence electrons and low ionization energies, cannot achieve the inert gas configuration by sharing electrons or donating them to other metallic atoms.

15. Metallic Bonding
Therefore, neither ionic nor covalent bonding is possible between metallic atoms. However, a relatively strong type of bonding, called metallic bonding, does occur in metals.

16. Metallic Bonding
Metals consist of a crystalline lattice in which positive ions are arranged in fixed patterns, and the valence electrons are free to move. These electrons do not belong to individual atoms, but rather to the crystal as a whole.

17. Metallic Bonding
The “sea of electrons” produces an attractive force that fixes the positions of the metallic ions. Because the electrons can move about freely, metals are good conductors of heat and electricity.