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Updated on 01st July, 2023 , 6 min read
A Lewis base is a molecule or ion that has an electron pair available for sharing. It is also known as a nucleophile. In simple words, it is a substance that can donate its electron pair to form a covalent bond with another substance, which is known as a Lewis acid. The concept of Lewis bases was introduced by Gilbert N. Lewis in 1923, and it has proven to be of great importance in the field of chemistry. In this article, we will discuss various examples of Lewis bases and their applications.
Svante Arrhenius proposed the first acid-base theory in 1884, which describes acid as a substance that contains hydrogen or produces H+ in an aqueous solution, while bases are substances that contain hydroxyl groups or produce OH- in an aqueous solution. Johannes Nicolaus Bronsted and Thomas Martin Lowry independently proposed the Bronsted-Lowry theory of acid-base in 1923, where an acid donates protons, and a base accepts protons. In the same year, Gilbert N. Lewis proposed the Lewis acid and base theory, which is widely accepted and allows for the prediction of a wider variety of acid-base reactions.
Gilbert Lewis, an American chemist, is credited with discovering the concept of bonding electron pairs and the acid-base theory named after him. After studying at Harvard University, he taught at Berkeley College for 34 years, where he contributed significantly to the development of the chemistry program. Although his primary area of research was thermodynamics, he published his work on electrons in 1913. He is also known for his contribution to the development of the Lewis dot structures that are still used today to symbolize the structure of atoms. Lewis was a crucial figure in the development of modern-day chemistry with his discovery of electrons and their properties.
A Lewis base is a substance that has an electron pair available for sharing. When a Lewis base donates an electron pair, it forms a coordinate covalent bond with a Lewis acid. Lewis bases are also known as nucleophiles since they are electron-rich species that seek out positively charged atoms or molecules to bond with.
The following are Lewis base examples of entities that possess the ability to donate an electron pair:
Lewis bases are substances that have a lone pair of electrons, which they can donate to form a coordinate covalent bond with a Lewis acid. The following are Lewis base examples:
Lewis bases have many important applications in chemistry, particularly in the fields of catalysis, synthesis, and materials science. Here are some examples of their applications:
Lewis Base |
Application in Everyday Life |
Ammonia |
Household cleaning products such as window and floor cleaners |
Water |
Used as a solvent, coolant, and reactant in many chemical reactions |
Oxygen |
Essential for respiration in living organisms |
Carbonate ions |
Used in antacid medications to neutralize stomach acid |
Hydroxide ions |
Used in drain cleaners and oven cleaners |
Nitrate ions |
Used in fertilizers for plants |
Acetate ions |
Used in food additives and flavorings |
Sulfur dioxide |
Used in the production of paper and in preserving wine |
Ethylene glycol |
Used as a coolant in car engines |
Chloride ions |
Used as a disinfectant in swimming pools |
Carbon dioxide |
Used in carbonated drinks and in fire extinguishers |
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By - Nikita Parmar 2024-09-06 10:59:22 , 6 min readA Lewis base is a chemical species that has a lone pair of electrons and can donate these electrons to a Lewis acid to form a coordinate covalent bond.
Examples of Lewis bases include ammonia (NH3), water (H2O), pyridine (C5H5N), and fluoride ion (F-).
Lewis acids and bases involve the transfer of electrons, while Bronsted-Lowry acids and bases involve the transfer of protons.
A chelating agent is a multidentate Lewis base that can form multiple coordinate covalent bonds with a Lewis acid. Ethylenediamine (en) and diethylenetriamine (dien) are examples of chelating agents.
The Lewis symbol for a Lewis base is the chemical symbol for the element or molecule, followed by a pair of dots to represent the lone pair of electrons.
A Lewis base bonds with a Lewis acid by donating its lone pair of electrons to an empty orbital on the Lewis acid, forming a coordinate covalent bond.
Lewis bases are generally polar compounds with high electron density and high boiling points. They can also form hydrogen bonds and have the ability to solvate cations.
Lewis bases are used as ligands in organometallic chemistry, as reagents in organic synthesis, and as catalysts in various chemical reactions.
Yes, Lewis bases can act as nucleophiles by donating a pair of electrons to an electrophilic center in a chemical reaction.
While all nucleophiles are Lewis bases, not all Lewis bases are nucleophiles. Nucleophiles are specifically defined as chemical species that can donate an electron pair to an electrophilic center, while Lewis bases have a more general definition of donating a pair of electrons to a Lewis acid.