Carbon Bonds

OBJECTIVE:
DESCRIBE THE BONDING OF ETHANE, ETHENE (ETHYLENE) AND ETHYNE(ACETYLENE) AND EXPLAIN THEIR GEOMETRY IN TERMS OF HYBRIDIZATION AND σ AND ¶ CARBON-CARBON BONDS.
Hybridization (or hybridization) is the concept of mixing (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electron to form chemical bond is valence bond theory.
An orbital of one atom can combine with that of another atom to form a sigma (σ) or pi (∏) bond.
A sigma bond is covalent bond resulting from the end-to-end overlap of orbitals.
A pi-bond results from the side-to-side overlap of p orbitals along a plane containing a line connecting the nuclei of the atoms

1. OBJECTIVE: DESCRIBE THE BONDING OF ETHANE , ETHENE (ETHYLENE) AND ETHYNE (ACETYLENE) AND EXPLAIN THEIR GEOMETRY IN TERMS OF HYBRIDIZATION AND σ AND ¶ CARBON-CARBON BONDS.

2. The electron configuration of carbon ( 1s 2 2s 2 2p 2 ) allows it to bind to itself to form chains and rings, and to bind covalently to other elements in different arrangements. Carbon has four valence electrons occupying the 2s and 2p orbitals. These orbitals can undergo hybridization into either sp 3 , sp 2 , or sp arrangements depending on the orientation of each orbitals on the hybrid.

3. What is hybridization? Hybridisation (or hybridization) is the concept of mixing (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electron to form chemical bond is valence bond theory.

4. An orbital of one atom can combine with that of another atom to form a sigma ( σ ) or pi (∏) bond. A sigma bond is covalent bond resulting from the end-to-end overlap of orbitals. A pi-bond results from the side-to-side overlap of p orbitals along a plane containing a line connecting the nuclei of the atoms.

5. Sigma bond forms from the end-to-end overlap of s-s , p-p , and s-p orbitals. s orbital s orbital s-s overlap + + p orbital p orbital p-p overlap

6. Sigma bond forms from the end-to-end overlap of s-s , p-p , and s-p orbitals. s orbital + p orbital s -p overlap

7. Pi bonds forms from side-to-side overlap of p-p orbitals + p orbital p orbital p-p overlap

8. Bond formation from hybridization Single bond - Sigma bond Double bond - Sigma bond + pi bond Triple bond - Sigma bond + pi bond + pi bond e nd-to-end s ide-to-side

9. The valence electrons of carbon can form both types of bonds, which results in the existence of a single, double, or triple covalent bonds.

10. In carbon atom, four sp 3 hybrid orbitals arise from a combination of one s orbital with three p orbital to form four single bonds with a tetrahedral geometry such as the case of ethane.

11. s p 3 C e thane

12. Another carbon hybridization can result in three sp 2 hybrid orbitals and one unhybridized 2 p orbital forming one double bond and two single bonds with a trigonal planar geometry. This is observed for the bonding in ethane.

13. sp 2 C ethene

14. The third hybridization scheme results in two sp hybrid orbitals and two unhybridization 2 p orbitals that can form one single bond and one triple bond with a linear geometry. This explains the triple covalent bond between the carbon atoms of ethyne .

15. sp C ethyne