What does a fluoride ion have in common with a neon atom and a sodium ion?

They are isoelectronic (meaning that they have the same number of electrons.

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What does fluoride ion have in common with a neon atom and a sodium ion?

To understand what a fluoride ion, a neon atom, and a sodium ion have in common, we need to consider their electron configurations and the elements they belong to.

1. Fluoride ion (F-): Fluoride is an anion, meaning it has gained an extra electron. It has the same number of protons as a fluorine atom (9), but one more electron, resulting in a net negative charge.

2. Neon atom (Ne): Neon is a noble gas, located in Group 18 (Group 8A) of the periodic table. As a noble gas, its electron configuration is very stable. It has a total of 10 electrons, and the outermost electron shell (valence shell) is completely filled with 8 electrons.

3. Sodium ion (Na+): Sodium forms a cation by losing one electron. It has the same number of protons as a sodium atom (11), but one less electron, resulting in a net positive charge.

Now, what do these three particles have in common?

All three have their outermost electron shell configuration as follows:
- Fluoride ion: 2 electrons in the first shell, 7 electrons in the second shell (completing it).
- Neon atom: 2 electrons in the first shell, 8 electrons in the second shell (completing it).
- Sodium ion: 2 electrons in the first shell, 8 electrons in the second shell (completing it).

Therefore, both the fluoride ion, neon atom, and sodium ion have the same electron configuration in their outermost electron shell, which is a stable configuration. This configuration, commonly known as the "octet rule," is associated with high stability because it resembles the electron configuration of noble gases, which tend to be chemically unreactive.

So, in summary, a fluoride ion, a neon atom, and a sodium ion all have similar outer electron shell configurations, specifically 2 electrons in the first shell and 8 electrons in the second shell, making them chemically stable.