Ch 3 Acids and bases Flashcards
Bronsted Lowry base
Proton acceptor
Conjugate base
What remains of the acid after it has been deprotonated
Conjugate acid
What remains after the base has been protonated
All reactions are accomplished via_______.
The flow of electron density (the motion of electrons)
Acids do not lose protons with the help_____.
Of a base
What does it mean for a reaction to reach equilibrium
There is no longer an observable change in the concentrations of reactants and products.
At equilibrium,the rate of the forward______
Is exactly equivalent to the rate of the reverse reaction
The equilibrium will always favor the formation of the ______
Weaker acid
If A- is very stable (weak base), then HA must be
A strong acid
If A- is very unstable( strong base), then HA must be a
Weak acid
What are the factors that affect the stability of a negative charge?
- The atom bearing the charge 2. Resonance 3. Induction 4. Orbitals
Electronegativity
Measures an atoms affinity for electrons(how willing the atom is to accepting a new charge). Electro negativity increases across a row
And up a column.
What is the dominant effect when comparing the relative acidity of two atoms in the same column
Atom size,the larger atom spreads the charge over a larger volume
A delocalized charge is _________.
More stable than a localized charge
Induction stabilizes a negative charge by______.
Withdrawing electron density away from the negative charged region
A pair of electrons in an sp hybridized orbital is held _______ to the nucleus than a pair of electrons in an sp2 or sp3 hybridized orbital.
Closer. As a result electrons residing in an sp orbital are stabilized by being close to the nucleus
The equilibrium will always favor the more stabilized
Negative charge
Bases stronger then hydroxide ______ be used when the solvent is water
Cannot. If a base stronger than HO- is dissolved in water, the base reacts with water to produce hydroxide. This is called the leveling effect.this is also observed in acidic solutions.
Lewis acid
Is a electron acceptor
Lewis base
Is a electron donor
Bronsted Lowry acid
Proton donor