To understand the reactivity of neon compared to sodium, we can analyze their positions on the periodic table and their electronic configurations.
Sodium (Na):
- Atomic number: 11
- Period: 3
- Group: 1 (alkali metals)
Sodium has the electronic configuration of \(1s^2 2s^2 2p^6 3s^1\). As an alkali metal in group 1, sodium has one electron in its outermost shell (the 3s subshell). This single valence electron is relatively easy for sodium to lose, making it highly reactive, particularly with nonmetals like halogens and in reactions with water, where it can form sodium ions (Na⁺) and hydroxide ions (OH⁻).
Neon (Ne):
- Atomic number: 10
- Period: 2
- Group: 18 (noble gases)
Neon has the electronic configuration of \(1s^2 2s^2 2p^6\). As a noble gas in group 18, neon has a complete outer shell with 8 electrons (the full valence shell configuration of \(s^2 p^6\)), making it very stable and nonreactive under standard conditions. Neon does not tend to form bonds with other elements because it does not need to gain, lose, or share electrons to achieve stability.
Summary of Reactivity Differences:
- Electron Configuration: Sodium has one electron in its outer shell, which it can easily lose, while neon has a full outer shell and a stable electronic configuration, making it nonreactive.
- Group Characteristics: Sodium, as an alkali metal, is highly reactive and readily forms bonds with many elements. In contrast, neon, being a noble gas, is chemically inert due to its stable electronic configuration.
- Trends in Reactivity: As you move across the periodic table, reactivity among metals increases down the group (for alkali metals like sodium), while noble gases like neon exhibit very little to no reactivity due to their stable electron arrangements.
In conclusion, due to their positions in the periodic table, sodium is highly reactive due to its single valence electron, while neon is largely unreactive, having a complete outer shell of electrons.
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