Question

The element expected to form largest in achieve the nearest noble gas configuration.

• A. F
• B. N
• C. Na
• D. O

Answer 1

The Correct Option is B

To solve this problem, we need to determine which element among F, N, Na, and O is expected to form the largest ion in order to achieve the nearest noble gas configuration.

The noble gas configuration refers to the electron arrangement of the nearest noble gas to an element, which is a stable configuration with a full outer shell of electrons. Most elements achieve this configuration by gaining, losing, or sharing electrons.

1. Fluorine (F): Fluorine has the atomic number 9 with an electron configuration of 1s² 2s² 2p⁵. It needs to gain 1 electron to achieve the noble gas configuration of Neon (Ne), which would result in the F⁻ ion.
2. Nitrogen (N): Nitrogen has the atomic number 7 with an electron configuration of 1s² 2s² 2p³. It needs to gain 3 electrons to achieve the noble gas configuration of Neon (Ne), which would result in the formation of the N³⁻ ion.
3. Sodium (Na): Sodium has the atomic number 11 with an electron configuration of 1s² 2s² 2p⁶ 3s¹. It needs to lose 1 electron to achieve the noble gas configuration of Neon (Ne), resulting in the Na⁺ ion.
4. Oxygen (O): Oxygen has the atomic number 8 with an electron configuration of 1s² 2s² 2p⁴. It needs to gain 2 electrons to achieve the noble gas configuration of Neon (Ne), resulting in the O²⁻ ion.

Among the given options, the ion that will be the largest is the one that has gained the most electrons because gaining electrons increases the size of the ion due to increased electron-electron repulsion. In this case, Nitrogen (N) gains 3 electrons to form N³⁻, which would result in the largest ion compared to F⁻, O²⁻, and Na⁺.

Conclusion: Therefore, the element expected to form the largest ion to achieve the nearest noble gas configuration is Nitrogen (N).