Edited Invalid date
8.3 Multiple Bonds
The nitrogen atoms are surrounded by four regions of electron density.
The nitrogen atoms are in urea.
There are three regions of electron density surrounding the carbon atom.
The carbon atom is in urea.
The molecule that gives vinegar its sour taste is acetic acid.
The geometry of single covalent bonds appears to be accounted for by the hybrid orbital model.
Multiple bonds consist of s and p bonds.
We can look at how we visualize these components and how they relate to hybrid orbitals.
The Lewis structure of ethene shows that each carbon atom is surrounded by one other carbon atom and two hydrogen atoms.
The bonding regions form a geometry.
There are five s bonds in the ethene molecule.
The p bond is above and below the s system.
The four hydrogen atoms and the two carbon atoms are all in the same plane.
The most stable bonding arrangement for the ethene molecule is the planar configuration.
The difference between s and p bonds is that the end-to-end overlap does not depend on the orientation of the orbitals on each atom in the bond.
The bonding electron density is symmetric about the axis, so rotation around it doesn't change the extent to which the s bonding orbitals overlap.
The off- axis overlap of the p bond is broken by the rotation of the internuclear axis.
A triple bond is given to the two carbon atoms of acetylene.
There are two C-C p bonds and one C-C s bond.
The line of the C-Cs bond leads to the two lobes of the p bonds.
Only s bonds, lone pairs of electrons, and single unpaired electrons are involved in hybridization.
The correct hybridization of the atoms is described by structures that account for these features.
Many structures have resonance forms.
There are various arrangements of p bonds that can cause resonance forms.
resonance does not affect the assignment of hybridization since the arrangement of p bonds only involves un hybridized orbitals.
There are two resonance forms for molecule benzene.
The resonance structure doesn't fully describe the electrons in the p bonds.
They aren't located in one position or the other, but they are delocalized throughout the ring.
Delocalization is not easily addressed by the valence bond theory.
Bonding in resonance forms is better described by the theory.
Review flashcards and saved quizzes
Getting your flashcards
Privacy & Terms