Final Answer:
Nitrogen can exceed the octet rule in compounds like ammonia (NH₃), forming more than eight electrons around its outer shell. Therefore the correct option is A.
Step-by-step explanation:
Atoms can indeed exceed the limits of the octet rule in bonding, and nitrogen (N) is a prime example of this deviation. Nitrogen has five valence electrons, and in many of its compounds, it can form more than the typical octet of electrons in its outer shell. One prevalent example is in ammonia (NH₃), where nitrogen shares its electrons with three hydrogen atoms, forming a total of eight electrons around it, thus exceeding the octet rule. Nitrogen achieves this by utilizing its lone pair of electrons to form additional bonds beyond the usual octet, showcasing its ability to surpass the eight-electron configuration in bonding.
Nitrogen, in certain compounds like ammonia, demonstrates its capability to expand its valence shell beyond the typical octet, challenging the traditional understanding of the octet rule. This deviation is possible due to nitrogen's access to its d-orbitals, enabling it to accommodate more than eight electrons in its valence shell. In the case of ammonia, nitrogen forms four electron pairs, with three shared with hydrogen atoms and one as a lone pair, totaling eight electrons around nitrogen. This departure from the octet rule occurs because nitrogen can access its empty d-orbitals to accommodate the additional electrons, allowing for exceptions to the typical octet configuration.
This ability of certain atoms, such as nitrogen, to exceed the octet rule is crucial in understanding the diverse bonding patterns observed in various molecules, showcasing exceptions to the standard eight-electron configuration in certain compounds like ammonia (NH₃). Therefore the correct option is A.