Question
How does the reactivity of neon (atomic number 10, period 2, group 18) differ from that of sodium (atomic number 11, period 3, group 1)? Explain your reasoning in easy words based on the properties of neon and sodium that you can infer based on their atomic numbers, periods, and groups.(4 points)
Answers
GPT-4o mini
The reactivity of neon and sodium is quite different due to their positions on the periodic table and their atomic structures. Here’s a breakdown:
1. **Group Characteristics**:
- **Sodium (Na)** is in Group 1, which is known as the alkali metals. Elements in this group are very reactive because they have one electron in their outer shell. Sodium easily loses this electron to achieve a stable configuration similar to noble gases.
- **Neon (Ne)** is in Group 18, which consists of noble gases. These elements are very stable and non-reactive because they have a full outer shell of electrons (8 electrons). Neon doesn’t need to gain or lose any electrons, making it very unreactive.
2. **Atomic Structure**:
- **Sodium** has 11 total electrons (2 in the first shell, 8 in the second, and 1 in the third). Its single outer electron makes it eager to react and form bonds.
- **Neon**, on the other hand, has 10 total electrons (2 in the first shell and 8 in the second). Since the second shell is full, neon does not seek to gain or lose electrons and prefers to remain as it is.
3. **Position on the Periodic Table**:
- Sodium is lower down on the periodic table (period 3), which means it is larger and its outer electron is further from the nucleus, making it easier to lose that electron.
- Neon is in period 2, meaning it has smaller atomic size. The electrons are held more tightly due to less shielding, contributing to its high stability and low reactivity.
4. **Conclusion**:
- In summary, sodium is highly reactive because it easily loses its one valence electron, while neon is very stable and unreactive because it has a complete outer electron shell. This fundamental difference arises from their group classifications and their electronic structures based on their atomic numbers.
1. **Group Characteristics**:
- **Sodium (Na)** is in Group 1, which is known as the alkali metals. Elements in this group are very reactive because they have one electron in their outer shell. Sodium easily loses this electron to achieve a stable configuration similar to noble gases.
- **Neon (Ne)** is in Group 18, which consists of noble gases. These elements are very stable and non-reactive because they have a full outer shell of electrons (8 electrons). Neon doesn’t need to gain or lose any electrons, making it very unreactive.
2. **Atomic Structure**:
- **Sodium** has 11 total electrons (2 in the first shell, 8 in the second, and 1 in the third). Its single outer electron makes it eager to react and form bonds.
- **Neon**, on the other hand, has 10 total electrons (2 in the first shell and 8 in the second). Since the second shell is full, neon does not seek to gain or lose electrons and prefers to remain as it is.
3. **Position on the Periodic Table**:
- Sodium is lower down on the periodic table (period 3), which means it is larger and its outer electron is further from the nucleus, making it easier to lose that electron.
- Neon is in period 2, meaning it has smaller atomic size. The electrons are held more tightly due to less shielding, contributing to its high stability and low reactivity.
4. **Conclusion**:
- In summary, sodium is highly reactive because it easily loses its one valence electron, while neon is very stable and unreactive because it has a complete outer electron shell. This fundamental difference arises from their group classifications and their electronic structures based on their atomic numbers.
put in paragraph
GPT-4o mini
The reactivity of neon and sodium differs significantly due to their positions on the periodic table and their atomic structures. Sodium (Na), located in Group 1 (alkali metals), is highly reactive because it has one electron in its outer shell that it readily loses to achieve a stable electronic configuration similar to that of noble gases. With 11 total electrons (2 in the first shell and 8 in the second), this single outer electron makes sodium eager to react and form bonds. In contrast, neon (Ne) is found in Group 18 (noble gases) and is very stable and non-reactive because it has a full outer shell of electrons (8 electrons). With a total of 10 electrons (2 in the first shell and 8 in the second), neon does not need to gain or lose any electrons, which contributes to its unreactiveness. Furthermore, sodium's position in period 3 makes it larger, with its outer electron further from the nucleus, facilitating its loss. In comparison, the smaller atomic size of neon in period 2 results in electrons being held more tightly due to less shielding, enhancing its stability. In summary, sodium’s high reactivity arises from its willingness to lose an outer electron, while neon’s lack of reactivity is attributed to its complete outer electron shell, highlighting the fundamental differences tied to their atomic numbers, groups, and electronic structures.
make shorter and in easy words
GPT-4o mini
Neon and sodium react very differently because of their positions on the periodic table and their atomic structures. Sodium (Na) is in Group 1, known as alkali metals, which means it is highly reactive. It has one electron in its outer shell that it easily loses to become stable. With 11 electrons total, this outer electron makes sodium eager to bond with other elements. In contrast, neon (Ne) is in Group 18, which consists of noble gases. Neon is very stable and doesn't react because it has a full outer shell of 8 electrons and doesn't need to gain or lose any. Sodium is larger and its outer electron is further away from the nucleus, making it easier to lose, while neon’s smaller size holds its electrons tightly, keeping it stable. In short, sodium is reactive because it can easily lose an outer electron, while neon is unreactive due to its complete outer shell.