In organic chemistry, synthetic reactions are often carried out by acids and bases. The reaction of a Lewis acid and a Lewis base creates new bonds.
So when a compound reacts chemically, which types of atoms bond with each other? In this regard, the HSAB theory (or HSAB principle) helps us to predict where compounds will react chemically. With regard to acids and bases, the HSAB principle describes them as hard acids and soft bases, for example.
You don’t have to remember exactly which atoms are hard and which ones are soft, because you can check the table. However, it is important to understand the concept of the HSAB theory to understand how a synthetic reaction proceeds.
Although the HSAB theory is an important rule of thumb in inorganic chemistry, organic chemistry uses the HSAB theory more frequently in laboratory experiments. So we will explain how to think about and use the HSAB theory.
Table of Contents
- 1 Meaning of Considering Atoms in Terms of Hardness and Softness
- 2 The HSAB Theory Is Useful for Predicting Organic Chemistry Reactions
- 3 Predicting Synthetic Reactions Using the HSAB Theory
Meaning of Considering Atoms in Terms of Hardness and Softness
There are several definitions of acids and bases. For these acids and bases, the Bronsted-Lowry theory is easy to understand. A molecule that gives an H+ (hydrogen atom) is a Bronsted acid and a molecule that receives an H+ (hydrogen atom) is a Bronsted base.
However, we don’t just consider the definition of Bronsted-Lowry in organic chemistry. This is because in the reaction between acids and bases, the H+ (proton) does not necessarily move.
So we think by Lewis acids and Lewis bases. When a Lewis acid reacts with a Lewis base, the HSAB principle is a method for predicting the ease of reaction.
-The HSAB Theory Is a Rule of Thumb for Making a Bond with Acids and Bases of the Same Nature
So why is it important to learn the HSAB principle? As mentioned above, the HSAB theory is the principle that can predict how chemical reactions will occur.
The HSAB theory is as follows.
- Hard acids form strong bonds with hard bases.
- Soft acids make strong bonds with soft bases.
Making strong bonds means that the reaction is more likely to proceed. For example, if you add a hard acid, the reaction will easily proceed with a hard base instead of a soft base. This feature is the HSAB theory and is involved in the ease with which molecules react with each other.
The Concept of Hard and Soft Atoms (Ions)
So what does it mean for an atom to be hard or soft? There are several factors that affect this, in particularly, which are related to the ease of polarization.
Hard acids and bases are less likely to be polarized. On the other hand, soft acids and soft bases are more easily polarized.
When does a molecule become easily polarized? This is affected by the atomic radius. If the atomic radius is small, electrons are strongly attracted to the nucleus. Because the nucleus contains positively charged protons, negatively charged electrons are attracted to the nucleus and, as a result, are less likely to be polarized.
On the other hand, if the radius of an atom is large, the electrons are away from the nucleus. Therefore, they are less affected by the nucleus and are more easily polarized.
Soft atoms are more likely to be polarized when a compound with a positive or negative charge is in close proximity. There is this difference between hard and soft atoms.
How Do We Remember the HSAB Principle?
According to the HSAB principle, hard and soft ions can be classified as follows.
-Classification of Acids
|Hard acids||H+, Li+, Na+, Mg2+, Ca2+, Al3+, Fe3+, Si4+, BF3, AlCl3, etc.|
|Intermediate acids||Fe2+, Cu2+, Zn2+, R3C+, etc.|
|Soft acids||Cu+, Ag+, Au+, Hg+, Hg2+, BH3, RS+, I2, Br2, etc.|
-Classification of Bases
|Hard bases||H2O, OH–, F–, Cl–, NO3–, ROH, RO–, NH3, RNH2, etc.|
|Intermediate bases||Br–, N3–, NO2–, aniline, pyridine, etc.|
|Soft bases||H–, CN–, R2S, RSH, RS–, I–, R–, R3P, CO, benzene, etc.|
It doesn’t make sense to remember all of these lists exactly. You just need to learn how to remember them roughly and be able to distinguish them.
If the atomic radius is small and the negative charge is low, it is more likely to be a hard acid or base. On the other hand, if the atomic radius is large and the negative charge is high, it tends to be a soft acid or base. The HSAB rule also tends to show the following.
-Atoms (Ions) Are Softer Towards the Bottom of the Periodic Table
Atoms on top of the periodic table have a smaller radius. In contrast, the lower an atom is on the periodic table, the larger its atomic radius is, the softer the acid or base.
For example, H+, alkali metals and alkaline earth metals at the top of the periodic table are hard acids. As for bases, F– and Cl– are also hard bases. But Br– is an intermediate base, and I– is a soft base. This has a lot to do with the ionic radius.
-Binding to a Hard Atom Makes the Ion Harder, and Binding to a Carbon Makes it Softer
Atoms with high electronegativity (F, O, N, etc.) are hard atoms. When these hard atoms are bonded together, the ions tend to be hard, such as NO3– and NH3– On the other hand, if the molecule is bound to a carbon atom, it tends to be a soft ion.
Of course, it is often difficult to distinguish between these criteria alone; the HSAB theory is just a rule of thumb.
-High Valence Metal Ions are hard
Metal ions with high valence tend to be hard, such as Al3+, Fe3+, and Si4+.
On the other hand, Fe2+ is an acid in the intermediate range, even for the same iron ion. If the valence changes, the hardness and softness of the ion will be different.
Reactivity Differs Between Electrostatic and Orbital Interactions
Now we understand that there are differences between Lewis acids and Lewis bases, with each molecule being harder or softer. So why do these differences occur? And why do hard ions tend to form bonds with each other and soft ones with each other?
Two factors are involved: electrostatic and orbital interactions.
The force of attraction between positive and negative charges is called electrostatic interaction. In the case of hard acids and bases with small atomic radius, electrostatic interactions play a major role in chemical reactions. Hard acids and hard bases react with each other because they are more likely to undergo chemical reactions with acids and bases.
On the other hand, in the case of a large atomic radius, synthetic reactions often proceed due to the overlap of molecular orbitals rather than chemical reactions depending on the degree of polarization. Molecular orbitals include HOMO (binding orbitals) and LUMO (anti-bonding orbitals), and electrons move through the orbitals in the molecule due to the influence of each other.
With a large atomic radius, it is more important for the molecular orbitals to overlap to form bonds than the effects of positive and negative charges. This is why softer acids and bases are more likely to react.
The HSAB Theory Is Useful for Predicting Organic Chemistry Reactions
So what does learning the HSAB theory do for you? As mentioned above, one of the areas of inorganic chemistry is the HSAB theory. We learn the HSAB theory in complex chemistry.
However, in practice, the HSAB theory is used more often in organic chemistry than in inorganic chemistry. This is because it can predict the reactions that will occur depending on whether the reagents to be reacted with are hard or soft. So try to figure out whether the molecules are hard or soft.
For example, consider a situation when the following nucleophilic substitution reaction (SN2 reaction) occurs.
Comparing alkoxide (RO–) and thiolate (RS–), alkoxide is more basic than thiolate. Therefore, it may seem that alkoxide and iodomethane react more quickly than thiolate and iodomethane. In fact, however, thiolate and iodomethane react faster than alkoxide and iodomethane.
Why is this the case? This can be explained by the HSAB principle. Sulfur atoms have a larger atomic radius than oxygen atoms. Iodine ions also have a large atomic radius. This is why soft acids and bases interact with orbitals and quickly react chemically to form new bonds.
Example Reactions with Grignard Reagent under the HSAB Principle
Learning the HSAB principle also helps us to understand regioselectivity. In organic chemistry, it is very important to predict where a reagent will react.
Compounds with magnesium metal in the molecule are Grignard reagents. Grignard reagents containing magnesium are hard nucleophiles and are strong bases. Grignard reagents are negatively charged and attack the carbonyl carbons that are positively polarized.
In other words, a chemical reaction occurs when a hard acid reacts with a hard base. The reaction is caused by acids and bases. The HSAB theory explains the 1,2 addition that occurs with Grignard reagent.
On the other hand, even for the same organometallic compound, the reactivity of the organocopper reagent changes. Organocopper reagents are called Gilman reagents. The Gilman reagent contains copper in the molecule, and copper is a soft metal with a large atomic diameter.
Therefore, it attacks the carbon in the double bond, which is the soft part of the molecule. It attacks the double bond, not the carbonyl carbon, because the effect of the overlapping molecular orbitals is stronger than the effect of the acid and base. This results in 1,4 addition (Michael addition).
The difference between the 1,2 and 1,4 addition (Michael addition) in organometallic compounds is frequently used as an example of a reaction in the HSAB theory. Of course, for other organic reactions, the HSAB theory can also be used to predict the progress of the reaction.
Predicting Synthetic Reactions Using the HSAB Theory
There is a method of remembering everything about how chemical reactions occur. However, it’s hard to remember. So, try to understand the rules of how a chemical reaction occurs. That way, you will be able to guess the reaction mechanism without having to remember them.
One of these rules is the HSAB principle. For atoms and ions, there are different types of atoms and ions, hard and soft, respectively. For acids and bases, they have different properties.
We don’t have to remember all the hard and soft molecules for acids and bases. Just try to learn what properties a compound has that makes it hard (or soft).
This will allow you to predict the rate and regioselectivity of the chemical reaction. The HSAB theory is used more frequently in organic chemistry than complexes in inorganic chemistry. Use the HSAB principle in organic chemistry reactions to be able to predict what kind of reaction will occur.