كيمياء غير عضويه(acidity and basicity)

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Acids and Bases
Your organic teachers are quite likely to ask you questions like identify the most acidic protons or the most basic site in a molecule. These facts can be important for determining where a molecule is likely to react when treated with a base or acid respectively. Many students can not do this efficiently. The following topics are covered here:

· Definitions : Bronsted, Lewis
· Acidity : K[sub]a and pKa
· Common acids in organic chemistry
· Basicity :
· Common bases in organic chemistry
Remember that acidity and basicity are the based on the same chemical reaction (but looking at it from opposite sides) and both happen simultaneously. In the following simple example the base, B, removes a proton from the acid, H-A:

Definitions
There are three theories used to describe acids and bases :}}

_Acids _Bases
_{Bronsted-theory} _{A proton donor} _{A proton acceptor}
_Lewis-theory _{An electron pair acceptor} _{An electron pair donor}
_{Now, some terminology:

Look at this equation and see how it fits the Bronsted-Lowry and Lewis definitions.
Acidity
Here are some general guidelines of principles to look for that can help you address the issue of acidity:
First, consider the simplified general equation of a simple acid reaction:}_{· The more stable the conjugate base, A[sup]-, is then the more the equilibrium favours the product side (Ka > 1), i.e. more dissociation of H-A
· More dissociation of H-A then the stronger H-A is as an acid, or
· The more the equilibrium favours products, the more H+ there is....
· The more H+ there is then the stronger H-A is as an acid....
· So looking for factors that stabilise the conjugate base, A-, gives us a "tool" for assessing acidity.
· The larger Ka implies more dissociation of HA and so the stronger the acid.
· The larger Ka is, the more negative the pKa so the lower the pKa, the stronger the acid.
Key factors that affect the stability of the conjugate base, A-,
HF > H2O > NH3 > CH4 Electronegativity. When comparing atoms within the same row of the periodic table, the more electronegative the anionic atom in the conjugate base, the better it is at accepting the negative charge.
HI > HBr > HCl > HF Size. When comparing atoms within the same group of the periodic table, the easier it is for the conjugate base to accommodate negative charge (lower charge density). The size of the group also weakens the bond H-X (note this trend should be applied with care since it only works within a group).
RCO2H > ROH Resonance. In the carboxylate ion, RCO2- the negative charge is delocalised across 2 electronegative oxygen atoms which makes it more stable than being localised on a specific atom as in the alkoxide, RO-.
General acidity trend of common organic acids (this is a very useful sequence to remember and to be able to rationalise):

Basicity
A convenient way to look at basicity is based on electron pair availability.... the more available the electrons, the more readily they can be donated to form a new bond to the proton and, and therefore the stronger base.
Key factors that affect electron pair availability in a base, B

CH3- > NH2- > HO- > F- Electronegativity. When comparing atoms within the same row of the periodic table, the more electronegative the atom donating the electrons is, the less willing it is to share those electrons with a proton, so the weaker the base.
F- > Cl- > Br- > I- Size. When comparing atoms within the same group of the periodic table, the larger the atom the weaker the H-X bond and the lower the electron density making it a weaker base.
RO- > RCO2- Resonance. In the carboxylate ion, RCO2- the negative charge is delocalised across 2 electronegative atoms which makes it the electrons less available than when they localised on a specific atom as in the alkoxide, RO-.
General acidity trend of some common organic bases:
Note that organic chemists tend to think about bases by looking at the pKa's of their conjugate acids, i.e. think about B- by looking at the acidity of BH. The implications are that the higher the pKa of the related conjugate acid, BH, the stronger the baseb B-.
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