CHM120H5 Lecture Notes - Lecture 37: Orbital Hybridisation, Molecular Geometry

35 views3 pages

blushrat11

26 Feb 2018

School

UTM

Department

Chemistry

Course

CHM120H5

Professor

Thottackad Radhakrishnan

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

# in the case of h2c=ch2 we have two such sp2 hybridized carbon atoms. # two of the hybridized orbitals on each c atom are used to form bond with h atoms. # the third orbital on each carbon atom will the over lap each other to form a carbon-carbon bond. # now the unhybridized p orbital on both c atoms are perfectly oriented so that they can overlap laterally to form a (cid:894)pi(cid:895) bond. # so the two c atoms are linked by a a(cid:374)d a bo(cid:374)d. # the bond angles hch, hcc are 1200. What are the differences between a and a bond. # when there is a sp3 hybridized carbon atom in a molecule it is connected to other atoms by single bonds- sp2- double bond and sp - triple bond. # carbon atom at the centre is linked to the other carbon atoms by double bonds.

Related Questions

Please answer the following

Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one ? bond with another carbon atom and one ? and one ? bond with another carbon atom. Each carbon atom also forms one ? bond with a hydrogen atom. Identify which types of orbitals overlap to form the bonds between the atoms in a benzene molecule. Drag the appropriate labels to their respective targets.

Attached is picture. Please explain/show work, will give 5 stars to correct answer, thank you very much! :)

Chemical bonds are formed by linear combinations of atomic orbital's. These atomic orbital's should have compatible energies. An axial overlap of these orbitals results in the formation of a sigma bond, whereas a lateral overlap results in the formation of a pi bond. When two atomic orbitai's on different atoms approach each other, two molecular orbital's are formed: one bonding molecular orbital and one antibonding molecular orbital. The bonding molecular orbital has a lower energy than the corresponding atomic orbital's: antibonding orbital's have higher energies than the corresponding atomic orbital's. An example using the hydrogen molecule is shown here. However, the same rule applies to systems with multiple atomic orbital's. For each atomic orbital that overlaps, one molecular orbital must form. In the diagram below. 1s orbitais from two hydrogen atoms combine to form one bonding sigma1 orbital and one antibonding orbital. The total number of bonding and antibonding orbital's is always equal to the number of orbital's that overlap. Similarly, molecular orbital's can also be formed by the overlapping of hybrid orbital's. The hybrid orbital's are formed by the linear combination of different atomic orbital's of nearly equal energy on the same atom. The atomic orbital's of nearly equal energy undergo a process of mixing and reorientation to form new orbital's of lower energy. This process is called hybridization For example, hybridization of one s and two p orbital's on an atom forms three sp2 hybrid orbital's. Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one sigma bond with another carbon atom and one sigma and one pi bond with another carbon atom. Each carbon atom also forms one sigma bond with a hydrogen atom. Identify which types of orbital's overlap to form the bonds between the atoms in a benzene molecule.

Answer True or false for the following questions.

1) There are eleven Ï bonds in this molecule?

2) There are three lone pairs of electrons in the complete Lewisstructure?

3) The C-N bond is formed from overlap of an sp3 hybrid orbitalfrom the carbon atom with an sp2 hybrid orbital from the nitrogenatom?

4) An sp2 hybrid orbital on C-1 overlaps with an sp3 hybrid orbitalon C-2 to form the sigma bond between C-1 and C-2?

5) There are four Ï bonds in this molecule?

6)The C-2 and C-3 atoms cannot rotate about the internuclear axisbetween the two atoms since the Ï bond would break?

7) The Ï bond between C-3 and O is formed by overlap ofunhybridized p atomic orbitals?

CHM120H5 Lecture Notes - Lecture 37: Orbital Hybridisation, Molecular Geometry

Document Summary

Get access

Related Documents

CHM120H5 Lecture Notes - Lecture 38: Orbital Hybridisation, Unpaired Electron, Pi Bond

CHM120H5 Study Guide - Midterm Guide: London Dispersion Force, Bond Order, Capillary Action

CHM120H5 Study Guide - Midterm Guide: Trigonal Planar Molecular Geometry, Octet Rule, Vsepr Theory

Related Questions