The correct response regarding reactivity between Neon and Lithium is:
Lithium is more reactive because it is a group 1 element and does not have a full outer shell of electrons.
Here are the key points explaining this difference in reactivity:
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Group Classification: Lithium is in Group 1 (alkali metals) of the periodic table, which means it has one valence electron in its outer shell. This configuration makes Lithium highly reactive, as it readily loses that one electron to achieve a stable electron configuration (similar to the noble gases). In contrast, Neon is in Group 18 (noble gases), where elements have full outer electron shells, making them very stable.
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Stability of Electron Configuration: Neon has a complete outer shell of eight electrons (a stable octet), which makes it very nonreactive. Noble gases are known for their lack of reactivity because they do not tend to gain or lose electrons easily. Lithium, with its single valence electron, is actively seeking to lose that electron, which leads to its high reactivity.
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Chemical Behavior: The chemical behavior of elements is largely dictated by their tendency to either gain, lose, or share electrons to achieve stability. As a member of the alkali metals, Lithium will react vigorously with water and other substances to form compounds. In contrast, Neon typically does not form compounds under normal conditions due to its stable electronic configuration.
In summary, Lithium is the more reactive element between the two due to its single valence electron and its desire to attain a stable electron configuration, whereas Neon is very stable and unreactive because of its full outer shell of electrons.
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