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Questions and Answers
What is a characteristic of a Lewis base?
What is a characteristic of a Lewis base?
Which of the following is an example of a metal ion that can act as a Lewis acid?
Which of the following is an example of a metal ion that can act as a Lewis acid?
What is a common use of boron compounds like BF3?
What is a common use of boron compounds like BF3?
Which of the following is a characteristic of ammonia (NH3) as a Lewis base?
Which of the following is a characteristic of ammonia (NH3) as a Lewis base?
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What is a common feature of Lewis acids with empty orbitals?
What is a common feature of Lewis acids with empty orbitals?
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Which of the following is an example of a Lewis base with a lone pair of electrons?
Which of the following is an example of a Lewis base with a lone pair of electrons?
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In the equation NH3 + H+ → NH4+, what is the role of NH3?
In the equation NH3 + H+ → NH4+, what is the role of NH3?
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Which of the following species acts as a Lewis acid in the equation BF3 + F- → BF4-?
Which of the following species acts as a Lewis acid in the equation BF3 + F- → BF4-?
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In the equation Zn2+ + 4NH3 → Zn(NH3)4²⁺, what is the role of Zn2+?
In the equation Zn2+ + 4NH3 → Zn(NH3)4²⁺, what is the role of Zn2+?
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What is the role of NH3 in the equation NH3 + HCl → NH4Cl?
What is the role of NH3 in the equation NH3 + HCl → NH4Cl?
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Which of the following species acts as a Lewis acid in the equation BF3 + NH3 → F3BNH3?
Which of the following species acts as a Lewis acid in the equation BF3 + NH3 → F3BNH3?
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Study Notes
Lewis Bases With Lone Pairs
- A Lewis base is a species that donates an electron pair to form a covalent bond
- Lewis bases typically have a lone pair of electrons that are available for bonding
- Examples of Lewis bases:
- Amines (e.g. NH3, RNH2)
- Phosphines (e.g. PH3)
- Ethers (e.g. ROR')
- Thiols (e.g. RSH)
Metal Ions As Lewis Acids
- Metal ions can act as Lewis acids by accepting electron pairs to form covalent bonds
- Metal ions have empty orbitals that can accommodate electron pairs
- Examples of metal ions that act as Lewis acids:
- Fe3+, Cu2+, Zn2+
- Metal ions can form complexes with Lewis bases, such as water, ammonia, or chloride ions
Ammonia As A Lewis Base
- Ammonia (NH3) is a common Lewis base
- NH3 has a lone pair of electrons that can be donated to form a covalent bond
- NH3 can form complexes with metal ions, such as Cu2+ or Zn2+
- NH3 can also act as a solvent for many reactions
Boron Compounds As Lewis Acids
- Boron compounds, such as BF3 and BCl3, are Lewis acids
- Boron compounds have empty orbitals that can accept electron pairs
- BF3 and BCl3 can form complexes with Lewis bases, such as amines or ethers
- Boron compounds are often used as catalysts in organic reactions
Lewis Acids With Empty Orbitals
- Lewis acids can have empty orbitals that can accept electron pairs
- Examples of Lewis acids with empty orbitals:
- BF3
- BCl3
- AlCl3
- These Lewis acids can form complexes with Lewis bases, such as amines or ethers
- Lewis acids with empty orbitals are often used as catalysts in organic reactions
Lewis Bases
- A Lewis base is a species that donates an electron pair to form a covalent bond
- Lewis bases typically have a lone pair of electrons available for bonding
- Examples of Lewis bases include amines (e.g. NH3, RNH2), phosphines (e.g. PH3), ethers (e.g. ROR'), and thiols (e.g. RSH)
Lewis Acids
- Metal ions can act as Lewis acids by accepting electron pairs to form covalent bonds
- Metal ions have empty orbitals that can accommodate electron pairs
- Examples of metal ions that act as Lewis acids include Fe3+, Cu2+, and Zn2+
Ammonia (NH3)
- Ammonia (NH3) is a common Lewis base that can donate electron pairs to form covalent bonds
- NH3 has a lone pair of electrons
- NH3 can form complexes with metal ions, such as Cu2+ or Zn2+, and act as a solvent for many reactions
Boron Compounds
- Boron compounds, such as BF3 and BCl3, are Lewis acids that can accept electron pairs
- Boron compounds have empty orbitals
- BF3 and BCl3 can form complexes with Lewis bases, such as amines or ethers, and are often used as catalysts in organic reactions
Characteristics of Lewis Acids
- Lewis acids can have empty orbitals that can accept electron pairs
- Examples of Lewis acids with empty orbitals include BF3, BCl3, and AlCl3
- These Lewis acids can form complexes with Lewis bases, such as amines or ethers, and are often used as catalysts in organic reactions
Lewis Bases
- A Lewis base is a species that donates an electron pair to form a covalent bond
- Lewis bases typically have a lone pair of electrons available for bonding
- Examples of Lewis bases include amines (e.g. NH3, RNH2), phosphines (e.g. PH3), ethers (e.g. ROR'), and thiols (e.g. RSH)
Metal Ions as Lewis Acids
- Metal ions can act as Lewis acids by accepting electron pairs to form covalent bonds
- Metal ions have empty orbitals that can accommodate electron pairs
- Examples of metal ions that act as Lewis acids include Fe3+, Cu2+, and Zn2+
Ammonia as a Lewis Base
- Ammonia (NH3) is a common Lewis base with a lone pair of electrons that can be donated to form a covalent bond
- NH3 can form complexes with metal ions, such as Cu2+ or Zn2+
- NH3 can also act as a solvent for many reactions
Boron Compounds as Lewis Acids
- Boron compounds, such as BF3 and BCl3, are Lewis acids with empty orbitals that can accept electron pairs
- BF3 and BCl3 can form complexes with Lewis bases, such as amines or ethers
- Boron compounds are often used as catalysts in organic reactions
Lewis Acids with Empty Orbitals
- Lewis acids can have empty orbitals that can accept electron pairs
- Examples of Lewis acids with empty orbitals include BF3, BCl3, and AlCl3
- These Lewis acids can form complexes with Lewis bases, such as amines or ethers, and are often used as catalysts in organic reactions
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Description
Learn about Lewis bases, electron pair donors, and metal ions as Lewis acids in forming covalent bonds.
