Chapter 4 - Analyzing Organic Reactions Flashcards
Lewis acid:
- definition
- tend to be what kind of molecule
- orbital vacancy and how that helps
- electron acceptor in the formation of a covalent bond
- Tend to be electrophiles
- Have vacant p-orbitals into which they can accept an electron pair, or have positively polarized atoms
Lewis base:
- definition
- tend to be what kind of molecules
- electron behavior
- anions or cations?
- electron donor in the formation of a covalent bond
- Tend to be nucleophiles
- Have a lone pair of electrons that can be donated
- Often are anions that carry a negative charge
coordinate covalent bonds:
When Lewis acids and bases interact
covalent bonds in which both electrons in the bond came from the same starting atom (the Lewis base)
Bronsted-Lowry definition:
- acid
- base
- Acid is a species that can donate a proton
- Base is a species that can accept a proton
Acid Dissociation constant (Ka):
- what it measures
- equation
measures the strength of an acid in solution
pKa:
- in acidic molecules
- electronegativity
- bond strength
- in basic molecules
- equation relating it to Ka
- More acidic molecules will have a smaller (or even negative) pKa
- The more electronegative at atom, the higher the acidity
- Less bond strength, the higher the acidity
- More basic molecules will have a larger pKa
- pKa = –log Ka
α-hydrogens and the the α-carbon:
α-hydrogens are connected to the α-carbon, which is a carbon adjacent to the carbonyl
Common Functional Groups:
- Groups that act like acids
- Groups that act like bases
- Functional groups that act as acids: alcohols, aldehydes, and ketones (at the α-carbon), carboxylic acids, and most carboxylic acid derivatives
- Amines and amides are the main functional groups that act as bases - form peptide bonds
Nucleophiles:
- definition
- look out for what molecules
- good nucleophiles tend to be what
- what makes them more reactive
- “nucleus-loving” species with either lone pairs or pi bonds that can form new bonds to electrophiles
- Look out for carbon, hydrogen, oxygen or nitrogen (CHON) with a minus sign or lone pair to identify most nucleophiles
- Good nucleophiles tend to be good bases
- The more basic the nucleophile, the more reactive it is
Factors that determine Nucleophilicity: (4 - just list)
Charge
Electronegativity
Steric Hindrance
Solvent
Factors that determine Nucelophilicity - Charge:
nucleophilicity increases with increasing electron density (more negative charge)
Factors that determine Nucleophilicity - Electronegativity:
nucleophilicity decreases as electronegativity increases because these atoms are less likely to share electron density
Factors that determine Nucleophilicity - Steric Hindrance:
bulkier molecules are less nucleophilic
Factors that determine Nucleophillicity - Solvent:
protic solvents can hinder nucleophilicity by protonating the nucleophile or through hydrogen bonding
Solvent effects with Nucleophilicity:
- in polar protic solvents
- in polar aprotic solvents
- in protic solvents
- in aprotic solvents
- In polar protic solvents, nucleophilicity increases down the periodic table
- In polar aprotic solvents, nucleophilicity increases up the periodic table
- In protic solvents, nucleophilicity decreases in the order: I- > Br- > Cl- > F-
- In aprotic solvents, nucleophilicity decreases in the order: F- > Cl- > Br- > F (Because there are no protons to get in the way of the attacking nucleophile)