Study Set Content:
- orbitals are in a plane with an angle of 120 from each other
- DOUBLE BOND
- Trigonal
- Planar geometry
sp2 hybrid orbitals
Head-on overlap gives what is called a
sigma bond
Sideways overlap gives a
pi bond
- Carbon can form a triple bond sharing six electrons
- Carbon 2s orbital hybridizes with a single p orbital giving two sp hybrids sp orbitals are linear geometry, 180 apart on x-axis
Sp1
- Shortest and strongest carbon—carbon bond
sp1
bonds that are neither fully ionic nor fully covalent but are somewhere between the two extremes.
Polar Covalent Bonds
intinsic ability of an atom to attract the shared electrons in a covalent bond
Electronegativity
a device for electron bookkeeping
Formal charges
Some molecules have structures that cannot be shown with a single representation. Represented by structures that contribute to the final structure but differ in the position of the p bond or lone pair.
Such structures are delocalized and are represented by
Resonance forms
Structure with resonance forms, that does not alternate between the forms.
Resonance hybrids
Rules for Resonance Forms
Individual resonance forms are imaginary.
Resonance forms differ only in the placement of their p or nonbonding electrons.
- is stable because it is symmetrical
- has a single, changing structure called a resonance hybrid
Allylic Carbocation
- the two individual structures of an allylic carbocation
- their special relationship is indicated by a double headed arrow placed between them
- the only difference between the resonance forms is the position of the bonding electrons
- atoms remain in same place in both resonance forms
Resonance forms
is a substance that donates a hydrogen ion
Bronsted-Lowry acid
is a substance that accepts a hydrogen ion.
Bronsted-Lowry base
that the concentration of solvent is ignored in the equilibrium expression and that brackets [ ] around a substance refer to the concentration of the enclosed species in moles per liter.
that the concentration of solvent is ignored in the equilibrium expression and that brackets [ ] around a substance refer to the concentration of the enclosed species in moles per liter.
- have their equilibria toward the right and thus have larger Ka
Stronger acids
- have their equilibria toward the left and have smaller acidity constants
Weaker acids
is the negative common logarithm of the Ka (-log Ka)
pKa
There is an inverse relationship between the acid strength of an acid and the base strength of its conjugate base. A strong acid yields a weak conjugate base, and a weak acid yields a strong conjugate base.
There is an inverse relationship between the acid strength of an acid and the base strength of its conjugate base. A strong acid yields a weak conjugate base, and a weak acid yields a strong conjugate base.
