Assertion: The bonds found in a molecule of $N_{2}$ are nonpolar covalent.
Reason: There is an equal sharing of electrons between the nitrogen atoms.

Both Assertion and Reason is correct and Reason is the correct explanation of Assertion

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Both Assertion and Reason is true and Reason is NOT the correct explanation of Assertion

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Assertion is correct and Reason is incorrect

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Assertion is incorrect and Reason is correct

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Both Assertion and Reason are incorrect

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Solution

The correct option is A Both Assertion and Reason is correct and Reason is the correct explanation of Assertion
Assertion : Thr bonds found in a molecule of $N_{2}$ are non polar covalent
The nature of polarity in a bond is the unequal distribution of bonding electrons due to differences in electronegativity. In $N_{2}$ , since the bond exists between two of the same atom, then they wil pull electrons equally (have the same electronegativity) and share them equally (i.e. Covalent bonding), making it non-polar.
Reason: There is an equal sharing of electron between the nitrogen atoms
If we count the number of valence electrons in each nitrogen atom, we would see that both equal to 8. Calculation of the formal charge for the most ideal shape, would be 0 and so it is the ideal structure.

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Assertion: The bonds found in a molecule of N2 are nonpolar covalent. Reason: There is an equal sharing of electrons between the nitrogen atoms.

Assertion: The bonds found in a molecule of $N_{2}$ are nonpolar covalent.
Reason: There is an equal sharing of electrons between the nitrogen atoms.