The Lewis dot structure is a diagram that represents the valence electrons of an atom or ion. Here, we will look at the Lewis dot structures for the chloride ion (Cl⁻) and the silver cation (Ag⁺).
Chloride Ion (Cl⁻)
Chlorine (Cl) is in Group 17 of the periodic table, which means it has 7 valence electrons. When chlorine gains one electron to form the chloride ion (Cl⁻), it has a total of 8 valence electrons. The Lewis dot structure for Cl⁻ is as follows:
[Cl:]
In this structure, the symbol ‘Cl’ represents the chlorine atom, and the dots around it represent the valence electrons. The extra electron gained by chlorine is shown as an additional dot, making a total of 8 electrons around the chlorine atom.
Silver Cation (Ag⁺)
Silver (Ag) is in Group 11 of the periodic table, which means it has 1 valence electron. When silver loses this electron to form the silver cation (Ag⁺), it has no valence electrons left. The Lewis dot structure for Ag⁺ is as follows:
Ag⁺
In this structure, the symbol ‘Ag’ represents the silver atom, and the ‘+’ sign indicates that it has lost one electron. Since Ag⁺ has no valence electrons, there are no dots around the symbol.
Understanding these Lewis dot structures helps in visualizing the electron configuration and bonding behavior of these ions.