Answer :
Final Answer
The effective nuclear charge felt by a 2p electron of a nitrogen atom is approximately +4.91. The effective nuclear charge felt by its 1s electron is approximately +7.28.
Explanation
In an atom, the effective nuclear charge experienced by an electron is the net positive charge felt by that electron due to the nucleus. It's important to note that the electrons in an atom don't only experience the full nuclear charge because of the shielding effect caused by other electrons.
For a 2p electron in a nitrogen atom, we can calculate the effective nuclear charge (Zeff) using Slater's rules. The effective nuclear charge (Zeff) for a 2p electron in nitrogen can be calculated as follows:
Zeff(2p) = Z - S(2s) - S(2p)
Here, Z is the atomic number (7 for nitrogen). S(2s) and S(2p) are the shielding constants for the 2s and 2p electrons, respectively. Using Slater's rules, the shielding constants are approximately 0.35 for 2s and 0.85 for 2p.
Zeff(2p) = 7 - 0.35 - 0.85 = 4.8
Similarly, for the 1s electron, the effective nuclear charge can be calculated:
Zeff(1s) = Z - S(1s) = 7 - 0.30 = 6.7
So, the effective nuclear charge felt by a 2p electron of a nitrogen atom is approximately +4.8, and the effective nuclear charge felt by its 1s electron is approximately +6.7.
The effective nuclear charge determines the attraction between the nucleus and the electrons, which ultimately affects the atomic properties and behavior of elements.
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