Hybridization Flashcards
1
Q
Hybrid orbitals are used to form ___ bonds
A
Sigma bonds (σ) (overlap of atomic orbitals)
2
Q
Unhybridized orbitals are used to form ___ bonds
A
Pi (π)
3
Q
Every single bond contains one ___ bond
A
Sigma
4
Q
Describe the bonds in a double bond
A
Every double bond has at least one sigma and one pi bond
5
Q
Describe the bonds in a triple bond
A
1 sigma and 2 pi bonds
6
Q
Strength of sigma vs. pi bonds
A
Sigma bonds are stronger than pi bonds
7
Q
What is hybridization?
A
- A procedure in which standard atomic orbitals are combined to form new, hybrid orbitals
- Hybridization occurs when an atom’s atomic orbitals ‘mix’ with the other atom’s atomic orbitals to form new hybrid orbitals
- Types of hybridization = sp3, sp2, sp, dsp3, d2sp3
- Referred to as ‘localized electron model’
8
Q
sp3 hybridization
A
- Forms from one s-orbital and three p-orbitals
9
Q
Example of sp3 hybridization
A
10
Q
sp2 hybridization
A
- One s-orbital and two p-orbitals
11
Q
sp hybridization
A
- One s-orbital and one p-orbital
12
Q
How to determine hybridization in complex molecules
A
Number of hybrid orbitals = number of bonded atoms + number of lone pairs
2 hybrid orbitals: sp
3 hybrid orbitals: sp2
4 hybrid orbitals: sp3
Exception: do NOT hybridize terminal, single-bonded atoms
