Valence bond theory says that only unpaired electron of valence shell can participate in Bond formation the valence shell of carbon is 2P and in the 2P two electrons are filled and 2pz are are vacant why the electrons of 2s orbital of carbon excited and go to 2P orbital while 2s orbital is not not a valence shell of carbon

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State whether the following statement is true or false:

Tetra covalent nature of the element with following valence shell electronic configuration is :

1 s^{2}

{2 s}^{2}

{2 p}^{2}

explain on the basis of excitation of

2 s

-electrons to

2 p

-orbital.

Q. Why do only valence electrons involve in bond formation? Why not electron of inner shells? Explain.

Q. Ground state electronic configuration of valence shell electrons in nitrogen molecule

(N_{2})

is written as

(S_{2 s})^{2} (S *_{2 s})^{2} (P_{2 p})^{4} (S_{2 p})^{2}

Hence, the bond order of nitrogen molecule is:

According to orbital overlap concept, the formation of a covalent bond between two atoms results by pairing of electrons present in the valence shell having opposite spins.

Q. Assertion :Ionic bonds are directional in nature whereas covalent bonds are non-directional. Reason: According to orbital overlap concept, the formation of a covalent bond between two atoms results by pairing of electrons present in the valence shell having same spins.

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