Learn the basics about the ionic bonding of calcium chloride, lithium fluoride and potassium oxide, as a part of the overall properties of matter topic.
An ionic bond is defined as the electrostatic attraction between oppositely charged ions.
In this video, we will learn about ionic bonding in lithium fluoride (LiF) and potassium oxide (K2O).
Lithium is a Group 1 metal, and will therefore have one electron in its valence shell. Its electronic structure is 2, 1.
Fluorine is a halogen and has seven electrons in its valence shell. Its electronic structure is 2, 7.
Lithium transfers its valence electron to fluorine, forming a Li+ ion and a F- ion.
It is a common misconception that there must be eight electrons in an electron shell for a species to be stable. As long as the electron shell in question is full, it will be stable.
This is seen with lithium – the first electron shell can only hold two electrons, and this shell is full, so a Li+ ion is stable.
Note that it has the same electronic structure as a He atom.
The Li+ ion and the F- ion are oppositely charged, and will be electrostatically attracted to one another, thereby forming an ionic bond.
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