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marin [14]
3 years ago
5

What orbitals are used to form the 10 sigma bonds in propane (ch3ch2ch3)? Label each atom with the appropriate hybridization. Dr

ag the appropriate labels to their respective targets. Note: not all labels will be used?

Chemistry
1 answer:
SVETLANKA909090 [29]3 years ago
3 0

Mixing of pure orbitals having nearly equal energy to form equal number of completely new orbitals is said to be hybridization.

For the compound, CH_3CH_2CH_3 the electronic configuration of the atoms, carbon and hydrogen are:

Carbon (atomic number=6): In ground state= 1s^{2}2s^{2}2p^{2}

In excited state: 1s^{2}2s^{1}2p^{3}

Hydrogen (atomic number=1): 1s^{1}

All the bonds in the compound is single bond(\sigma-bond) that is they are formed by head on collision of the orbitals.

The structure of the compound is shown in the image.

The Carbon-Hydrogen bond is formed by overlapping of s-orbital of hydrogen to p-orbital of carbon.

In order to complete the octet the required number of electrons for carbon is 4 and for hydrogen is 1. So, the electron in 1s^{1} of hydrogen will overlap to the 2p^{3}-orbital of carbon.

Thus, the hybridization of Hydrogen is s-hybridization and the hybridization of Carbon is sp^{3}-hybridization.

The hybridization of each atom is shown in the image.

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