I am very confused about hybridization in general. Please give an explanation on how to do this.
Which of the following pairs of atomic orbitals of adjacent nuclei can overlap to form a sigma bond? a pi bond? or no bond at all?
a) 1s and 1s
b) 1s and 2px
c) 2px and 2py
d) 3py and 3py]
f) 1s and 2s
The following summarizes the bonding.
s + s = sigma bond
p + p = pi bond
s + p = sigma bond
a. see table.
b. see table.
c. no bond is formed BECAUSE the 2px and 2py are at right angles to each other and no interaction takes place.
d. pi bond. see table.
f. see table.
Look at the picture model of the first site shown here.
http://www.google.com/images?q=atomic+orbitals&oe=utf-8&rls=org.mozilla:en-US:official&client=firefox-a&um=1&ie=UTF-8&source=univ&ei=ocYoTeGeCoH7lwem-NTjAQ&sa=X&oi=image_result_group&ct=title&resnum=2&ved=0CDMQsAQwAQ&biw=800&bih=406
To understand hybridization, we first need to understand atomic orbitals. Atomic orbitals are regions of space around the nucleus where electrons are most likely to be found. They are denoted by letters and numbers, such as 1s, 2s, 2p, etc.
Hybridization occurs when atomic orbitals combine to form new hybrid orbitals. These new orbitals have properties that are intermediate between the original orbitals. Hybrid orbitals are used to explain the bonding in molecules.
To determine which pairs of atomic orbitals can overlap to form sigma, pi, or no bonds, we need to consider their shapes and orientations.
1. 1s and 1s: When two s orbitals (1s and 1s) overlap, they form a sigma bond. This type of bond is a single bond, where the electron density is concentrated along the internuclear axis.
2. 1s and 2px: When an s orbital (1s) and a p orbital (2px) overlap, they can form a sigma bond or no bond, depending on the orientation. If the two orbitals are aligned along the internuclear axis, they can form a sigma bond. However, if they are aligned in a side-by-side manner (parallel to the internuclear axis), they cannot form a sigma bond. In this case, no bond is formed.
3. 2px and 2py: When two p orbitals (2px and 2py) overlap, they can form a sigma bond, a pi bond, or no bond, depending on the orientation. If the two p orbitals overlap along the internuclear axis, they can form a sigma bond. If they overlap in a perpendicular manner (at right angles to the internuclear axis), they form a pi bond. However, if they are aligned in a side-by-side manner, they cannot form any bond.
4. 3py and 3py: When two p orbitals (3py and 3py) overlap, they can form a sigma bond, a pi bond, or no bond, depending on the orientation. If the two p orbitals overlap along the internuclear axis, they can form both a sigma bond and a pi bond. If they overlap in a perpendicular manner, they form only a pi bond. If they are aligned in a side-by-side manner, they cannot form any bond.
5. 1s and 2s: When an s orbital (1s) and a higher energy s orbital (2s) overlap, they can form a sigma bond. This type of bond is a single bond, similar to the sigma bond formed between two s orbitals.
In summary:
- 1s and 1s can form a sigma bond
- 1s and 2px can form a sigma bond or no bond
- 2px and 2py can form a sigma bond, a pi bond, or no bond
- 3py and 3py can form a sigma bond, a pi bond, or no bond
- 1s and 2s can form a sigma bond
Remember, the ability of atomic orbitals to overlap and form bonds depends on their shapes and orientations.