what is the hybrisation of C2H4
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1. In ethene C2H 4 , each carbon uses its 2s and two 2p orbitals for hybridization resulting three sp 2 hybrid orbitals. The third 2p orbital remains unhybridized.
The following figure demonstrates the bonding:
Step 1- Atomic orbitals of C-atom in ground state
Step 2- Atomic orbitals of C-atom in excited state
Step 3- sp 2 hybridization in C-atom with three sp 2 hybride orbitals and one p unhybrid orbital
Step 4- The three sp2 orbitals are shared by one C and two H atoms to give ethene molecule having C-C double bonds (one sigma and one pie)
2. C2H2 is hybridized in a sp orbital - triple bond between the carbon atoms.
The electronic configuration of carbon in the ground state (i.e. the lowest energy state) is 1s(2) 2s(2) 2p(2). If energy is supplied to raise one of the 2s electrons to a higher energy level to fill the vacant 2p orbital, the electronic configuration of carbon in the excited state, is 1s(2) 2s(1) 2p(3). More specifically, the electronic configuration of the excited carbon atom is 1s(2) 2s(1) 2px(1) 2py(1) 2pz(1). If we leave two of the 2p sub-orbitals (e.g. the 2py(1) and 2pz(1) sub-orbitals) to form the second and third bonds of the carbon to carbon triple bond, we can rearrange the other two sub-orbitals (i.e. 2s(1) and 2px(1)) to form two equivalent hybrid orbitals. When these new orbitals are arranged as far apart in space as possible, the new orbitals are arranged in a plane and are 180 degrees apart.
The particular hybridisation of the orbitals of carbon atoms in ethene, are called sp1 hybrids orbitals, (i.e. they arises from the hybridising of one sigma orbital and one pi orbitals). The bonds between the hydrogen atoms and carbons, and the first bond (of the double bond) between the carbon atoms of ethene are formed by the end-on overlap of these sp1 hybrids orbitals to form sigma bonds, and accounts for the 180 degree bond angles observed in this compound. The second and third bonds (of the triple bond) between the carbon atoms in ethyne is formed by the side-on overlap of the original atomic unhybridised orbitals (i.e. the 2py(1) and 2pz(1) orbitals) and these are pi bonds.
The following figure demonstrates the bonding:
Step 1- Atomic orbitals of C-atom in ground state
Step 2- Atomic orbitals of C-atom in excited state
Step 3- sp 2 hybridization in C-atom with three sp 2 hybride orbitals and one p unhybrid orbital
Step 4- The three sp2 orbitals are shared by one C and two H atoms to give ethene molecule having C-C double bonds (one sigma and one pie)
2. C2H2 is hybridized in a sp orbital - triple bond between the carbon atoms.
The electronic configuration of carbon in the ground state (i.e. the lowest energy state) is 1s(2) 2s(2) 2p(2). If energy is supplied to raise one of the 2s electrons to a higher energy level to fill the vacant 2p orbital, the electronic configuration of carbon in the excited state, is 1s(2) 2s(1) 2p(3). More specifically, the electronic configuration of the excited carbon atom is 1s(2) 2s(1) 2px(1) 2py(1) 2pz(1). If we leave two of the 2p sub-orbitals (e.g. the 2py(1) and 2pz(1) sub-orbitals) to form the second and third bonds of the carbon to carbon triple bond, we can rearrange the other two sub-orbitals (i.e. 2s(1) and 2px(1)) to form two equivalent hybrid orbitals. When these new orbitals are arranged as far apart in space as possible, the new orbitals are arranged in a plane and are 180 degrees apart.
The particular hybridisation of the orbitals of carbon atoms in ethene, are called sp1 hybrids orbitals, (i.e. they arises from the hybridising of one sigma orbital and one pi orbitals). The bonds between the hydrogen atoms and carbons, and the first bond (of the double bond) between the carbon atoms of ethene are formed by the end-on overlap of these sp1 hybrids orbitals to form sigma bonds, and accounts for the 180 degree bond angles observed in this compound. The second and third bonds (of the triple bond) between the carbon atoms in ethyne is formed by the side-on overlap of the original atomic unhybridised orbitals (i.e. the 2py(1) and 2pz(1) orbitals) and these are pi bonds.
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