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Answer :
Nitrogen has seven protons, whereas beryllium has four. Therefore, the effective nuclear charge of beryllium is somewhat larger than that of 2.
Explain about the Nitrogen?
The chemical element with the atomic number 7 and the letter N is known as nitrogen. The lightest element in group 15 of the periodic table, often known as the pnictogens, nitrogen is a nonmetal. It is a typical element in the cosmos, believed to be eighth in the Milky Way and the Solar System in terms of overall abundance.
Nitrogen is a typical diatomic non-metal gas that is typically colourless, odourless, and tasteless. It is trivalent in the majority of compounds because its outer shell contains five electrons.
An vital macronutrient for plants, nitrogen is also a crucial component of amino acids, which serve as the building blocks for enzymes and proteins in plants.
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Final answer:
The valence electrons in nitrogen experience a greater effective nuclear charge compared to those in beryllium because nitrogen has more protons, resulting in a stronger pull on the valence electrons. This greater charge leads to nitrogen's smaller atomic size compared to beryllium.
Explanation:
The valence electrons in nitrogen experience a greater effective nuclear charge than those in beryllium. This is because, as you move from left to right across the periodic table, the nuclear charge increases due to an increase in the number of protons, while the inner electron shells (like the 1s shell in both beryllium and nitrogen) remain the same. The inner electron shells provide electron shielding which mitigates the effect of the increased nuclear charge. In nitrogen, there are five protons exerting a pull on the valence electrons, compared to only four in beryllium. Additionally, electrons in the same principal shell do not shield each other very effectively.
Nitrogen, being further to the right on the periodic table than beryllium, has more protons in its nucleus, resulting in its valence electrons feeling a stronger pull from the nucleus. This increased pull, or effective nuclear charge, causes nitrogen's atomic size to be smaller compared to beryllium, despite both elements having electrons in the 2s and 2p orbitals.
