Apply the trends in properties related to the blocks of the periodic table to identify the characteristic properties that belongs to the element with the following electron configuration (1 mark): 1s22s22p63s23p3 (A:1)

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The question asks us to apply periodic trends to identify the characteristic properties of the element with the given electron configuration: 1s22s22p63s23p3.
First, recognize the core noble-gas configuration (1s22s22p6) then add 3s23p3, which corresponds to phosphorus (P) in period 3 of the periodic table. This places the element squarely in the nonmetals region, specifically the pnictogens, rather than metals, metalloids, or transition metals.
Option a states: 'Metal, relatively higher boiling point than elements in higher periods.' This conflicts with the established fact that phosphorus is a nonmetal, and among nonmetals, boiling points are generally not characterized as 'relatively higher' than many elements in higher periods, especially metals that tend to have higher boiling points. Thus this choice misclassifies the element and its typical phase/behavior.
Option b states: 'Non metal, relatively lower boiling point than elements in higher periods.' Here the nonmetal classification is correct. The phrase 'relatively lower boiling point than elements in higher periods' aligns with the intuition that many heavier elements in higher periods (especially metals and some nonmetals with higher molecular structures, such as silicon and sulfur in higher periods) exhibit higher boiling points compared to lighter nonmetals like phosphorus in period 3. While there are nuances in boiling points across periods and groups, choosing a nonmetal with a comparatively lower boiling point relative to higher-period elements fits the trend for phosphorus when contrasted with many heavier elements that have higher melting/boiling points due to metallic bonding or network structures.
Option c claims: 'Transition metal with higher melting and boiling points than Alkaline metals.' This is inaccurate for phosphorus, which is not a transition metal at all; transition metals reside in the d-block, not in Group 15. The statement in c confuses the block and the characteristic melting/boiling relationships between categories of elements.
Option d asserts: 'Alkaline Metal, higher melting and boiling point than Alkali metals.' This is incorrect because the element is not an alkaline (alkaline earth) metal but a nonmetal in Group 15. Moreover, the comparison of melting/boiling points between alkaline earth metals and alkali metals is not applicable to phosphorus, which lies in a completely different category.
In summary, the electron configuration points to a nonmetal in period 3, and among the provided choices, option b is the only one that correctly identifies the nonmetallic character and conveys a relative trend about boiling points when compared to higher-period elements. The remaining options either misclassify the element or apply incorrect chemical category and trends.

Apply the trends in properties related to the blocks of the periodic table to identify the characteristic properties that belongs to the element with the following electron configuration (1 mark): 1s22s22p63s23p3 (A:1)

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