The document explains the bonding and geometry of ethane, ethene, and ethyne in terms of hybridization and types of carbon-carbon bonds. It details how carbon's four valence electrons hybridize into sp3, sp2, or sp arrangements, leading to sigma and pi bonds, and describes the resulting geometries: tetrahedral for ethane, trigonal planar for ethene, and linear for ethyne. The document emphasizes the relationship between hybridization and bond formation, indicating that single, double, and triple bonds arise from different combinations of sigma and pi bonds.

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 (1s22s22p2)
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 sp3, sp2, 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
end-to-end
side-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 sp3 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.

12. sp3 C
ethane

13. Another carbon hybridization can
result in three sp2 hybrid orbitals and
one unhybridized 2p orbital forming
one double bond and two single
bonds with a trigonal planar
geometry. This is observed for the
bonding in ethane.

15. sp2 C
ethene

16. The third hybridization scheme results
in two sp hybrid orbitals and two
unhybridization 2p 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.

18. sp C
ethyne