Question
How does the reactivity of neon atomic number 10 period 2 group 18 defer from that sodium atomic number 11 period 3 group 1 you must explain your reasoning based on the properties of neon sodium that you can infer based on only their atomic numbers periods and groups
Answers
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GPT-4o mini
The reactivity of elements is largely influenced by their position in the periodic table, which reflects their atomic structure and electron configuration.
**Neon (Ne)**, with an atomic number of 10, is located in period 2 and group 18 (the noble gases). It has a full outer shell of electrons, which consists of 8 electrons (the stable electron configuration of 1s² 2s² 2p⁶). This full valence shell makes neon highly stable and largely unreactive under normal conditions. Noble gases, including neon, are known for their lack of reactivity because they do not tend to gain, lose, or share electrons.
**Sodium (Na)**, on the other hand, has an atomic number of 11 and is located in period 3 and group 1 (the alkali metals). Sodium has one more electron than neon, leading to a configuration of 1s² 2s² 2p⁶ 3s¹. It has one electron in its outermost shell (the 3s orbital), which is not a full shell (the full configuration would be 8 in the outer shell). This makes sodium highly reactive; it tends to lose that one outer electron easily in chemical reactions, forming positive ions (Na⁺) and readily reacting with other elements to achieve a full outer shell (by achieving a stable configuration of 8 electrons in the next lower shell).
In summary, the key differences in reactivity between neon and sodium can be inferred from their positions and properties based on their atomic numbers, periods, and groups:
1. **Electron Configuration**:
- Neon: Full outer shell (8 electrons) → Stable, low reactivity.
- Sodium: One electron in outer shell (1 electron in 3s) → Unstable, high reactivity.
2. **Group Characteristics**:
- Group 18 (Ne): Noble gases are inert due to full valence shells.
- Group 1 (Na): Alkali metals are very reactive due to their tendency to lose one electron.
Thus, while neon is non-reactive due to its stable electronic configuration, sodium is highly reactive as it seeks to lose its single valence electron to reach a more stable electronic configuration.
**Neon (Ne)**, with an atomic number of 10, is located in period 2 and group 18 (the noble gases). It has a full outer shell of electrons, which consists of 8 electrons (the stable electron configuration of 1s² 2s² 2p⁶). This full valence shell makes neon highly stable and largely unreactive under normal conditions. Noble gases, including neon, are known for their lack of reactivity because they do not tend to gain, lose, or share electrons.
**Sodium (Na)**, on the other hand, has an atomic number of 11 and is located in period 3 and group 1 (the alkali metals). Sodium has one more electron than neon, leading to a configuration of 1s² 2s² 2p⁶ 3s¹. It has one electron in its outermost shell (the 3s orbital), which is not a full shell (the full configuration would be 8 in the outer shell). This makes sodium highly reactive; it tends to lose that one outer electron easily in chemical reactions, forming positive ions (Na⁺) and readily reacting with other elements to achieve a full outer shell (by achieving a stable configuration of 8 electrons in the next lower shell).
In summary, the key differences in reactivity between neon and sodium can be inferred from their positions and properties based on their atomic numbers, periods, and groups:
1. **Electron Configuration**:
- Neon: Full outer shell (8 electrons) → Stable, low reactivity.
- Sodium: One electron in outer shell (1 electron in 3s) → Unstable, high reactivity.
2. **Group Characteristics**:
- Group 18 (Ne): Noble gases are inert due to full valence shells.
- Group 1 (Na): Alkali metals are very reactive due to their tendency to lose one electron.
Thus, while neon is non-reactive due to its stable electronic configuration, sodium is highly reactive as it seeks to lose its single valence electron to reach a more stable electronic configuration.