Highlights the basic points in lewis and langmuir theory of electrovalency.
what are basic point in lewis and Langmuir theory of electrovalency
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Lewis and Langmuir's theories of electrovalency provide important insights into the concept of chemical bonding and the formation of ionic compounds. Here are the key points of their theories:
1. Lewis Theory:
- According to Lewis, atoms gain, lose, or share electrons to attain a stable electron configuration similar to the noble gases.
- The outermost shell of an atom is called the valence shell, and the electrons in this shell are responsible for bonding.
- Atoms tend to gain or lose electrons to achieve a stable octet configuration (eight electrons in the valence shell) like the nearest noble gas.
- A positively-charged ion is formed when an atom loses electrons, while a negatively-charged ion is formed when an atom gains electrons.
- Ionic compounds are formed through the transfer of electrons from a metal atom (which loses electrons and becomes a cation) to a non-metal atom (which gains electrons and becomes an anion).
- The attraction between the oppositely charged ions results in the formation of an ionic bond.
2. Langmuir Theory:
- Langmuir expanded on Lewis' theory by proposing the concept of the octet rule, which states that atoms tend to gain, lose, or share electrons to achieve a stable octet electron configuration.
- Langmuir emphasized that atoms prefer to have a complete outer shell with eight electrons.
- The octet rule applies to elements in the s- and p-blocks of the periodic table.
- Among main group elements, atoms gain or lose electrons to achieve an electron configuration similar to the nearest noble gas.
- Langmuir's theory also explains the formation of ionic compounds through electron transfer between atoms.
To summarize, Lewis and Langmuir's theories of electrovalency explain how atoms bond together by gaining, losing, or sharing electrons to achieve a stable electron configuration, leading to the formation of ionic compounds through electron transfer. These theories highlight the importance of the octet rule and the concept of valence electrons in chemical bonding.