To determine which element has more neutrons than protons in its most abundant isotope, we need to compare the number of neutrons and protons for each of the given elements.
The number of protons for an element is equal to its atomic number. The number of neutrons can be found by subtracting the atomic number from the atomic weight (typically rounded to the nearest whole number for isotopes).
Let's calculate the number of neutrons for each element:
-
N (Nitrogen):
- Atomic Number = 7
- Atomic Weight ≈ 14.01 (rounds to 14)
- Neutrons = 14 - 7 = 7 neutrons
- Neutrons = Protons (7) → Not more neutrons than protons.
-
O (Oxygen):
- Atomic Number = 8
- Atomic Weight ≈ 16.00 (rounds to 16)
- Neutrons = 16 - 8 = 8 neutrons
- Neutrons = Protons (8) → Not more neutrons than protons.
-
F (Fluorine):
- Atomic Number = 9
- Atomic Weight ≈ 19.00 (rounds to 19)
- Neutrons = 19 - 9 = 10 neutrons
- Neutrons (10) > Protons (9) → More neutrons than protons.
-
Ne (Neon):
- Atomic Number = 10
- Atomic Weight ≈ 20.2 (rounds to 20)
- Neutrons = 20 - 10 = 10 neutrons
- Neutrons = Protons (10) → Not more neutrons than protons.
From the above calculations, the only element that has more neutrons than protons in its most abundant isotope is Fluorine (F).
Therefore, the answer is:
C. F
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