1. Atomic Number: Nitrogen (N) has an atomic number of 7, meaning it has 7 protons in its nucleus. Beryllium (Be) has an atomic number of 4, with 4 protons. The higher number of protons in nitrogen's nucleus creates a stronger positive charge.
2. Electron Shielding: Electrons in inner shells shield the valence electrons from the full pull of the nucleus. Both nitrogen and beryllium have 2 electrons in their 1s shell. However, nitrogen has 2 electrons in its 2s shell and 3 electrons in its 2p shell, while beryllium has 2 electrons in its 2s shell.
3. Effective Nuclear Charge (Zeff): Zeff is the net positive charge experienced by an electron. The more shielding electrons there are, the lower the Zeff.
* Nitrogen: The 2 electrons in the 2s and 2p orbitals of nitrogen are shielded by the 2 core electrons (1s). The 5 protons in the nucleus exert a strong attractive force on the 5 valence electrons, resulting in a higher Zeff.
* Beryllium: The 2 valence electrons in beryllium are shielded by the 2 core electrons (1s). The 4 protons in the nucleus exert a weaker attractive force on the 2 valence electrons, resulting in a lower Zeff.
In Summary:
- Nitrogen has a larger nuclear charge due to more protons.
- Nitrogen has more shielding electrons in its inner shells compared to beryllium.
- This results in a greater effective nuclear charge experienced by the valence electrons of nitrogen, making them more tightly bound to the nucleus.
