Question
Which pairs of elements do not have to satisfy the octet rule for stability?
potassium (K) and sodium (Na)
neon (Ne) and argon (Ar)
oxygen (O) and fluorine (F)
helium (He) and hydrogen (H)
potassium (K) and sodium (Na)
neon (Ne) and argon (Ar)
oxygen (O) and fluorine (F)
helium (He) and hydrogen (H)
Answers
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Answered by
GPT-4o mini
The octet rule states that atoms tend to bond in such a way that they have eight electrons in their valence shell, achieving a stable configuration. However, not all elements strictly follow this rule.
In the pairs you've provided:
1. **Potassium (K) and Sodium (Na)**: Both of these are alkali metals which have one electron in their outermost shell and typically lose that electron to achieve stability. They do not satisfy the octet rule.
2. **Neon (Ne) and Argon (Ar)**: Both of these are noble gases that already have full outer electron shells (Neon with 8 electrons and Argon with 8 electrons), so they don't have to satisfy the octet rule, as they are already stable.
3. **Oxygen (O) and Fluorine (F)**: Both of these are nonmetals that typically do follow the octet rule by gaining or sharing electrons to achieve a full octet.
4. **Helium (He) and Hydrogen (H)**: Helium has 2 electrons in its valence shell (which is full for helium, as it is in the first period), while hydrogen has 1 electron and typically seeks to gain one more to achieve the stable configuration of helium (duet rule).
Out of these pairs, **Potassium and Sodium** and **Helium and Hydrogen** are not required to strictly satisfy the octet rule for stability. However, since both potassium and sodium do not follow the octet rule as metals which often have one electron (as they will lose that to achieve stability), and hydrogen seeks just 2 electrons, we can conclude:
- **Potassium (K) and Sodium (Na)** do not satisfy the octet rule.
- **Helium (He)** does not need to satisfy it, and **Hydrogen (H)** follows the duet rule sensibly.
Therefore, **the pairs that do not satisfy the octet rule** are **Potassium (K) and Sodium (Na)**, and to some extent **Helium (He) and Hydrogen (H)** which follow the duet rule instead.
In the pairs you've provided:
1. **Potassium (K) and Sodium (Na)**: Both of these are alkali metals which have one electron in their outermost shell and typically lose that electron to achieve stability. They do not satisfy the octet rule.
2. **Neon (Ne) and Argon (Ar)**: Both of these are noble gases that already have full outer electron shells (Neon with 8 electrons and Argon with 8 electrons), so they don't have to satisfy the octet rule, as they are already stable.
3. **Oxygen (O) and Fluorine (F)**: Both of these are nonmetals that typically do follow the octet rule by gaining or sharing electrons to achieve a full octet.
4. **Helium (He) and Hydrogen (H)**: Helium has 2 electrons in its valence shell (which is full for helium, as it is in the first period), while hydrogen has 1 electron and typically seeks to gain one more to achieve the stable configuration of helium (duet rule).
Out of these pairs, **Potassium and Sodium** and **Helium and Hydrogen** are not required to strictly satisfy the octet rule for stability. However, since both potassium and sodium do not follow the octet rule as metals which often have one electron (as they will lose that to achieve stability), and hydrogen seeks just 2 electrons, we can conclude:
- **Potassium (K) and Sodium (Na)** do not satisfy the octet rule.
- **Helium (He)** does not need to satisfy it, and **Hydrogen (H)** follows the duet rule sensibly.
Therefore, **the pairs that do not satisfy the octet rule** are **Potassium (K) and Sodium (Na)**, and to some extent **Helium (He) and Hydrogen (H)** which follow the duet rule instead.
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