Sigma (σ) and pi (𝝅) bonds Flashcards
1
Q
Sigma bonds
A
- Head-to-head overlap of orbitals
- Can be formed by s,p,d or hybrid orbitals
- Cylindrical symmetry of electron density about internuclear axis
2
Q
𝝅 bonds
A
- Cannot occur with s or hybridised orbitals
- Side-to-side overlap of p or d orbitals
- Electron density above and below internuclear axis
3
Q
Why are σ bonds stronger than 𝝅 bonds?
A
σ bonds are stronger because the electrons are in the same place. Attractive force is more focused.
In 𝝅 bonds the attractive force is more spread out
4
Q
Hybridisation
A
The mixing of different types of orbitals to form new types of orbitals
5
Q
What hybridisation do molecules with tetrahedral electron geometry have?
A
sp3
6
Q
What hybridisation do trigonal planar molecules have?
A
sp2
7
Q
What hydridisation do linear molecules have?
A
sp
