what does fluorine ion have in common with a neon atom and a sodium ion?
Both are isoelectronic with Ne; i.e., their outside shells are filled with eight electrons and all have the same number of electrons (that is the isoelectronic part).
Fluorine ion, neon atom, and sodium ion are all related to each other in terms of their electron configuration and their position in the periodic table. Here's a step-by-step breakdown of their similarities:
1. Electron Configuration:
- Fluorine ion (F-) has gained one electron to achieve a stable electron configuration of 2s22p6, which is the same as the electron configuration of a neon atom.
- Neon atom (Ne) has a completely filled electron configuration of 2s22p6, which makes it a stable noble gas.
- Sodium ion (Na+) has lost one electron from its neutral state to achieve a stable electron configuration of 2s22p6, which is the same as neon and fluorine ion.
2. Noble Gas Configuration:
- Fluorine ion, neon, and sodium ion all have a noble gas configuration, meaning their electron configurations resemble that of a noble gas.
- Neon is a noble gas with a completely filled electron configuration, while both fluorine ion and sodium ion have electron configurations resembling that of neon due to gaining or losing electrons.
3. Position in the Periodic Table:
- Fluorine (F) and neon (Ne) are both found in the second period of the periodic table, specifically in group 18 and group 17, respectively.
- Sodium (Na) is found in the third period of the periodic table in group 1.
In summary, fluorine ion, neon atom, and sodium ion have similarities in terms of electron configuration, noble gas configuration, and their relative positions in the periodic table.
To understand what fluorine ion (F-), a neon atom (Ne), and a sodium ion (Na+) have in common, let's start by examining their electron configurations.
Fluorine (F) has an atomic number of 9, which means it has 9 protons and 9 electrons. In its neutral state, fluorine has an electron configuration of 1s2 2s2 2p5, with one electron missing from its 2p orbital.
When fluorine gains one electron, it becomes a fluorine ion (F-) with 10 electrons. Its new electron configuration is 1s2 2s2 2p6, with a completely filled outermost electron shell.
Neon (Ne), on the other hand, has an atomic number of 10, with 10 protons and 10 electrons. It has a stable electron configuration of 1s2 2s2 2p6, with a completely filled outermost electron shell.
Lastly, sodium (Na) has an atomic number of 11, with 11 protons and 11 electrons. In its neutral state, sodium has an electron configuration of 1s2 2s2 2p6 3s1, with one electron in its outermost shell.
When sodium loses one electron, it becomes a sodium ion (Na+) with 10 electrons. Its new electron configuration is 1s2 2s2 2p6, which is the same as that of neon.
Now, let's see what these three species have in common:
1. They all have 10 electrons: Both the fluorine ion and the sodium ion have an electron configuration of 1s2 2s2 2p6, which matches the completely filled electron configuration of neon.
2. They are all stable: Neon is stable due to its full outermost electron shell, and both the fluorine ion and sodium ion achieve stability by gaining or losing electrons, respectively, to achieve a completely filled outermost electron shell.
In summary, fluorine ion, neon atom, and sodium ion all have the same electron configuration with 10 electrons, resembling the electron configuration of neon, which is a stable noble gas.