Chapter 2-Polar Covalent Bonds; Acids and Bases Flashcards
Polar covalent bonds
Bonding electrons are attracted more strongly to one atom than the other so the electron distribution is not symmetrical
Electronegativity on table
Left to Right- electronegativity increases
Top to Bottom - decreases
Electrostatic potential maps
Red- electron rich
Blue- electron poor
Inductive effect
Shifting of electrons in a sigma bond in response to the electronegativity of nearby atoms
Dipole movement equation
μ = Q x r
Bronsted-lowry acid
Donates a hydrogen ion (proton)
Bronsted-lowry base
Accepts a hydrogen ion (proton)
Ka formula
Ka= [H3O+][A-] / [HA]
PKa formula
-logKa
Stronger acid pKa and Ka
pKa is smaller
Ka is larger
Weaker acid pKa and Ka
pKa is larger
Ka is smaller
A strong acid has a
Weak conjugate base
A weak acid has a
Strong conjugate base
A strong acid loses a H+
Easily meaning it’s conjugate holds it weakly making it a weak base
A weak acid loses an H+
With difficulty so it’s conjugate holds onto it tightly, making it a strong base
Organic acids
Presence of positively polarized hydrogen atom (blue on map)
Organic bases
Presence of an atom with a lone pair of electrons (red on map) that can bond to a H
Lewis acid
Accepts an electron pair
Lewis base
Donates an electron pair
Protonate
Add a proton to
Dispersion forces
Happen between neighbouring molecules
Hydrogen bond
H bonded to O or N
- very strong dipole
Hydrophilic substances
Have many OH groups and can therefore form hydrogen bonds in water and dissolve
