CHM151Y1 Lecture Notes - Bond Length, Covalent Bond

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Published on 3 Aug 2011
School
UTSG
Department
Chemistry
Course
CHM151Y1
Professor
Lecture 3- CHM151
covalent bonds results form the overlap of singly bound orbitals
sigma bonds- cylindrical cross-section [symmetry]
this is the feature of all sigma bonds,
why is it that these 2 hydrogens atoms form a bond? Why is it
favourable?
There is a positive and negative charge; however, there must be enough
energu, there is an optimal separation, they have to be a specific lengh
form one another. This length is known as bond length.
The SI unit used is pm ( picometre) 1pm=10^-12m, 1 Ancstrom = 10^-
10m
Another important feature of a bond, other than bond length, is the
amount of energy gained by bringing them together. For instance, by
brining together hydrogen bonds, you gain 436 kj/mol.
So if you want to disscoaite an H2 molecule to Hand H atoms, you have
to supply 436 jk/mol
HYBRID ORBITALS
- lower orbitals are further apart [more repulsion], and as you go higher, the
orbitals are closer tgether.
- the more bonds between the carbons, the stronger the bond.
- better overlap gives rise to greater bond strentgth
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Document Summary

Lecture 3- chm151 covalent bonds results form the overlap of singly bound orbitals sigma bonds- cylindrical cross-section [symmetry] this is the feature of all sigma bonds,  there is a positive and negative charge; however, there must be enough energu, there is an optimal separation, they have to be a specific lengh form one another.  the si unit used is pm ( picometre) 1pm=10^-12m, 1 ancstrom = 10^-  another important feature of a bond, other than bond length, is the amount of energy gained by bringing them together. For instance, by brining together hydrogen bonds, you gain 436 kj/mol.  so if you want to disscoaite an h2 molecule to hand h atoms, you have to supply 436 jk/mol. Lower orbitals are further apart [more repulsion], and as you go higher, the orbitals are closer tgether. The more bonds between the carbons, the stronger the bond.