" A Lewis acid (named for the American physical chemist Gilbert N. Lewis) is a chemical species that contains an empty orbital which is capable of accepting an electron pair from a Lewis base to form a Lewis adduct."
These are acids that can accept an electron pair from a donor molecule. Examples include boron trifluoride (BF3), aluminium chloride (AlCl3), and iron(III) oxide (Fe2O3).
Acids and Bases: The concept of acids and bases is essential when studying Lewis acids. Acids are substances that donate hydrogen ions while bases accept hydrogen ions.
Bronsted-Lowry Theory of Acids and Bases: This theory defines acids as proton donors and bases as proton acceptors. It also touches upon the concept of pH and conjugate acids and bases.
Lewis Theory of Acids and Bases: According to the Lewis theory, acids are electron pair acceptors, while bases are electron pair donors. This theory forms the basis for understanding Lewis acids.
Electronegativity: Electronegativity is a measure of the tendency of an atom to attract electrons towards itself. It is important to know about electronegativity as it helps to determine the Lewis acid strength of elements.
Lewis Acid Strength: The strength of a Lewis acid is determined by how easily it can accept an electron pair. Some factors that affect Lewis acid strength include the size of the atom, its charge, and its electronegativity.
Lewis Bases: Lewis bases are electron pair donors. Learning about Lewis bases is important as they are the counterpart of Lewis acids, and chemical reactions occur when they come into contact with Lewis acids.
Hard and Soft Acids and Bases (HSAB): The HSAB theory defines two groups of Lewis acids and bases: Hard and soft. Hard acids are small and have high electronegativity, while soft acids are bigger, and have lower electronegativity.
Coordination Complexes: Coordination complexes are compounds that contain a central metal ion surrounded by ligands. Understanding coordination complexes is essential for learning about Lewis acids as metal ions can act as Lewis acids.
Acid-Base Reactions: Acid-base reactions involve the transfer of protons or electron-pairs. It is important to study acid-base reactions when learning about Lewis acids as they form a basis for understanding chemical reactions involving Lewis acids.
Types of Lewis Acid-Base Reactions: Various types of Lewis acid-base reactions include adduct formation, ligand exchange, and redox reactions. Knowing the different types of Lewis acid-base reactions is essential for understanding the mechanism behind chemical reactions.
Metal ions: Metal ions such as Al3+, Fe3+, and Au3+ are common Lewis acids as they have vacant d-orbitals that can accept electrons from a Lewis base.
Metal complexes: Metal complexes contain a metal ion surrounded by ligands, which can act as Lewis acids. For example, the Cu2+ ion in the Cu(NH3)42+ complex can accept electrons from ammonia molecules.
Protons: Protons, often referred to as H+, are common Lewis acids in aqueous solutions. They accept electrons from water molecules to form hydronium ions (H3O+).
Boron compounds: Boron compounds such as BCl3, BF3, and B(OR)3 are commonly used as Lewis acids. They have a vacant p-orbital on the boron atom, which can accept electrons from a Lewis base.
Carbocations: Carbocations are positively charged organic molecules that can act as Lewis acids by accepting electrons from Lewis bases. For example, the tert-butyl cation (C(CH3)3+) is a common Lewis acid in organic chemistry.
Nonmetal ions: Nonmetal ions such as BF4-, ClO4-, and PF6- can act as Lewis acids by accepting electrons from Lewis bases.
Lewis acid-base adducts: Lewis acid-base adducts are formed when a Lewis acid accepts electrons from a Lewis base. For example, the adduct formed between BCl3 and NH3 is a Lewis acid-base adduct.
Organic acids: Organic acids contain a carbon atom that is electron-deficient and can act as a Lewis acid. For example, carboxylic acids such as acetic acid (CH3CO2H) can donate a proton and accept a pair of electrons.
Inorganic acids: Inorganic acids such as HCl, HBr, and HI are common Lewis acids in aqueous solutions. They donate a proton and accept a pair of electrons to form a hydronium ion.
Metal oxide/hydroxide ions: Metal oxide and hydroxide ions such as AlO2-, Al(OH)2+, and Fe(OH)2+ are examples of Lewis acids that can accept a pair of electrons to form a coordinate bond.
"A Lewis acid is a chemical species that contains an empty orbital capable of accepting an electron pair from a Lewis base to form a Lewis adduct."
"A Lewis base is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a dative bond with a Lewis acid to form a Lewis adduct."
"For example, NH3 is a Lewis base because it can donate its lone pair of electrons."
"Trimethylborane (Me3B) is a Lewis acid as it is capable of accepting a lone pair."
"In a Lewis adduct, the Lewis acid and base share an electron pair furnished by the Lewis base, forming a dative bond."
"In the context of a specific chemical reaction between NH3 and Me3B, a lone pair from NH3 will form a dative bond with the empty orbital of Me3B to form an adduct NH3•BMe3."
"The terms nucleophile and electrophile are more or less interchangeable with Lewis base and Lewis acid, respectively."
"The term nucleophilicity emphasizes the kinetic aspect of reactivity, while Lewis basicity emphasizes the thermodynamic aspect of Lewis adduct formation."
"These terms, especially their abstract noun forms nucleophilicity and electrophilicity, emphasize the kinetic aspect of reactivity."
"Lewis acidity emphasizes the thermodynamic aspect of Lewis adduct formation."
"A Lewis acid is a chemical species that contains an empty orbital capable of accepting an electron pair."
"In a Lewis adduct, the Lewis acid and base share an electron pair furnished by the Lewis base, forming a dative bond."
"In the context of a specific chemical reaction between NH3 and Me3B, a lone pair from NH3 will form a dative bond with the empty orbital of Me3B to form an adduct NH3•BMe3."
"Lewis acidity emphasizes the thermodynamic aspect of Lewis adduct formation, while electrophilicity emphasizes the kinetic aspect of reactivity."
"Lewis basicity refers to the ability of a species to donate electrons."
"A Lewis base is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a dative bond with a Lewis acid."
"The terms nucleophile and electrophile are more or less interchangeable with Lewis base and Lewis acid, respectively."
"A Lewis acid is a chemical species that contains an empty orbital capable of accepting an electron pair from a Lewis base."
"Lewis basicity emphasizes the thermodynamic aspect of Lewis adduct formation, while nucleophilicity emphasizes the kinetic aspect of reactivity."