To determine which element will pair with a group 6 non-metal, like oxygen (O), in a 1:1 ratio, we need to examine the valence electrons for each option. Here’s the detailed step-by-step solution:
1. Understanding Valence Electrons:
- Oxygen (O) is a group 6 element with 6 valence electrons. To achieve a stable octet (8 electrons), oxygen needs 2 more electrons.
2. Evaluating Each Option:
- Sulfur (S): Sulfur also belongs to group 6 of the periodic table and has 6 valence electrons, similar to oxygen. Because both elements require additional electrons to complete their octet, pairing sulfur with oxygen in a 1:1 ratio would not be sufficient for either to become stable.
- Nitrogen (N): Nitrogen is a group 5 element with 5 valence electrons. It needs an additional 3 electrons to complete its octet. Pairing nitrogen with oxygen in a 1:1 ratio would result in an imbalanced electron sharing where neither element achieves stability.
- Magnesium (Mg): Magnesium is a group 2 element with 2 valence electrons. Magnesium can lose these 2 electrons, achieving a stable configuration, while oxygen can gain these 2 electrons to complete its octet. Therefore, Mg will pair with O in a 1:1 ratio, resulting in a stable compound.
- Sodium (Na): Sodium is a group 1 element with 1 valence electron. It can lose this 1 electron to achieve stability, but oxygen requires 2 electrons to complete its octet. Pairing sodium with oxygen in a 1:1 ratio would not suffice as oxygen needs another electron to become stable.
3. Conclusion:
- The element that pairs well with oxygen (O) in a 1:1 ratio to achieve stable octet configurations for both atoms is magnesium (Mg).
Therefore, the correct answer is magnesium (Mg), which corresponds to the option:
magnesium (Mg).
