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Answer :
Final answer:
Group number correlates with the number of valence electrons, which influences the metallic and non-metallic character of elements. Metallic character increases down a group due to lower ionization energy and increased atomic radius, while non-metallic character increases from left to right across the periodic table because of a higher electronegativity.
Explanation:
The relationship between Group number, number of outer-shell (valency) electrons, and metallic/non-metallic character is foundational in understanding the periodic table and chemical reactivity. Group number generally indicates the number of valence electrons in an atom; for example, Group 1 (I) elements have one valence electron while Group 17 (VII) elements have seven valence electrons, excluding the transition metals (groups 3-12).
Metallic character refers to an element's tendency to lose electrons and form positive ions or cations. This character increases as you move down a group since the atomic radius increases, placing valence electrons farther from the nucleus, which decreases the ionization energy. Consequently, these atoms can more easily lose their outer electrons.
Conversely, non-metallic character relates to an element's tendency to accept electrons to form negative ions or anions. This character increases across the periodic table from left to right, as the atoms have a higher electronegativity and a greater desire to gain electrons to achieve a stable electron configuration like the noble gases.
The chemical reactivity of an element, whether metal or non-metal, largely depends on the ease with which it can gain or lose valence electrons.
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