summarie the tet elow

Question

Neon (Ne) and sodium (Na) exhibit very different reactivities due to their positions in the periodic table, characterized by their atomic numbers, periods, and groups.
1. **Group and Reactivity:**
- **Sodium (Na)** is in Group 1, which is known as the alkali metals. These elements are characterized by their high reactivity, particularly with water and halogens, due to their single electron in their outermost shell. This one valence electron makes sodium keen to lose it, thus forming a positively charged ion (Na⁺) and achieving a more stable electron configuration similar to that of noble gases.
- **Neon (Ne)**, on the other hand, is in Group 18, which comprises the noble gases. Noble gases are known for their lack of reactivity because they have complete outer electron shells. Neon has eight electrons in its outer shell, which fulfills the octet rule, making it highly stable and unlikely to engage in chemical reactions under normal conditions.

2. **Period and Electron Configuration:**
- Sodium is in Period 3, meaning it has three electron shells. The electron configuration of sodium is 1s² 2s² 2p⁶ 3s¹. The presence of one electron in the 3s orbital leads to its reactivity, as it can readily lose that electron to form a Na⁺ ion.
- Neon is in Period 2, with the electron configuration 1s² 2s² 2p⁶. Its full outer shell (2s and 2p subshells filled) makes it stable and nonreactive. The filled valence shell means that neon does not easily gain, lose, or share electrons.

3. **Overall Summary of Reactivity:**
- Sodium, due to its single valence electron, is very reactive and readily loses that electron to become stable, leading to various chemical reactions.
- In contrast, neon, with its complete outer shell, is chemically inert and does not participate in reactions under standard conditions.

In conclusion, the reactivity of neon differs significantly from that of sodium due to their complete versus incomplete valence shells, reflecting the fundamental principles behind the properties of elements in different groups of the periodic table.

Answer 1

Neon (Ne) and sodium (Na) have vastly different reactivities due to their positions in the periodic table. Sodium is located in Group 1, known as alkali metals, and is highly reactive due to its single valence electron, which it readily loses to form a Na⁺ ion and achieve stability. In contrast, neon is in Group 18, the noble gases, and is chemically inert because it has a full outer shell of eight electrons, fulfilling the octet rule and making it unlikely to engage in chemical reactions.

Sodium, found in Period 3, has the electron configuration 1s² 2s² 2p⁶ 3s¹. Its lone 3s electron contributes to its reactivity. Neon, in Period 2, possesses a stable electron configuration of 1s² 2s² 2p⁶, which results in its nonreactive nature.

Overall, sodium's reactivity stems from its incomplete valence shell, while neon’s stability arises from its complete outer shell, illustrating key differences between elements in different groups of the periodic table.