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Group 15 includes nitrogen, phosphorus, arsenic, antimony, bismuth, and moscovium. As we move down the group, the elements transition from non-metallic to metallic characteristics, passing through a metalloid phase. Nitrogen and phosphorus are non-metals, arsenic and antimony are metalloids, while bismuth and moscovium are typical metals.
Helium, with an electronic configuration of
Ionization energy refers to the amount of energy required to remove an electron from the outermost orbit of an atom. It is influenced by how strongly the nucleus holds onto the electron. The closer an electron is to the nucleus, the stronger the attraction, and therefore, more energy is needed to remove it.
In Group 15 elements, as we move down the group from nitrogen to bismuth, the atomic radius increases, which results in a decrease in ionization energy. This is because the outer electrons are farther from the nucleus and experience a weaker attraction, making them easier to remove.
The ionization enthalpy of Group 15 elements is generally higher than that of Group 14 elements within the same period, owing to the extra stability provided by the half-filled p orbitals in Group 15. However, as you move down the group, the ionization enthalpy gradually decreases due to the increasing atomic size and the resulting decrease in nuclear attraction.
Electronegativity refers to the tendency of an atom to attract electrons towards itself in a chemical bond. In Group 15, electronegativity decreases as you move down the group. This is because the increasing atomic size reduces the attraction between the nucleus and the bonding electrons. However, the change in electronegativity is less pronounced among the heavier elements in the group.
In Group 15, all elements except bismuth exhibit allotropy, meaning they exist in different structural forms. For example, nitrogen exists in two allotropic forms: alpha nitrogen and beta nitrogen. Phosphorus has multiple allotropic forms, with red and white phosphorus being the most significant.
Arsenic also shows allotropy with three primary forms: black, grey, and yellow arsenic. Similarly, antimony exists in three forms: yellow, metallic, and explosive antimony. These allotropic variations result from differences in the arrangement of atoms within the element, which can lead to distinct physical and chemical properties.
