Ions and the octet rule

The octet rule provides a way to predict what kind of ion an atom will form. The rule usually applies to the representative elements. The rule has many exceptions, but is still very useful. The breaks down for elements in periods 3 through 7.

The Octet Rule: Main-group elements are more stable when they have a complete outer shell of valence electrons. In other words, the main-group elements tend to react so they have eight valence electrons. Click here for practice exercise

 

Example: What kind of ion do you expect to be formed by calcium? Answer: Calcium will form a Ca2+ cation. This is based on the fact that calcium is in Group 2A. It is a metal with two valence electrons. The electron configuration for the 20 electrons in calcium is 1s22s22p63s23p64s2. This can be written in a "shorthand" notation as [Ar]4s2. Here the 18 inner electrons in the 1s22s22p63s23p6 are represented by the symbol [Ar]. The outer electrons are in the 4s subshell. The neutral atom is converted to the +2 ion when the outer electrons are removed. The octet rule predicts an atom will form an ion with a rare gas electron configuration. The rare gas in this case is the rare gas from the previous period.   Particle Electron configuration Shorthand configuration core electrons are indicated by rare gas symbol Ca atom 1s22s22p63s23p64s2 [Ar]4s2 Ca2+ cation 1s22s22p63s23p6 [Ar] Note the shorthand notation shows the rare gas core and the subshells for the outer electrons.

 Createded by Dr. Walt Volland revised March 28, 2005 all rights reserved