What are the basic points of Lewis and langmiur theory of electrovalency
The Lewis and Langmuir theories are related to the concept of electrovalency, also known as ionic bonding. Here are the basic points of these theories:
1. Lewis Theory:
- Developed by Gilbert N. Lewis, it defines electrovalency as the transfer of electrons from one atom to another to form an ionic bond.
- According to this theory, an atom can gain or lose electrons to achieve a stable electron configuration, usually the same as that of a noble gas.
- Atoms that lose electrons become positively charged ions (cations), while atoms that gain electrons become negatively charged ions (anions).
- The electrostatic attraction between oppositely charged ions leads to the formation of an ionic bond.
2. Langmuir Theory:
- Developed by Irving Langmuir, it expands on Lewis' theory and explains how the formation of electrovalent bonds occurs.
- Langmuir proposed that atoms attain a stable electron configuration by either gaining or losing electrons to achieve a full outermost energy level (octet rule).
- According to this theory, for an atom to donate or accept electrons, it must have a partially filled or vacant outer energy level.
- The outermost energy level can be considered to have s and p orbitals, so elements with fewer than eight electrons in their valence shell can lose or gain electrons to achieve stability.
To understand these theories better, you can study the principles of electrovalency, electron configurations, trends in the periodic table, and the octet rule. These concepts will provide you with a solid foundation to comprehend and apply Lewis and Langmuir theories.