Physisorption and Chemisorption — Explained

Detailed Explanation

Adsorption, a fundamental surface phenomenon, involves the accumulation of molecular species on the surface rather than in the bulk of a solid or liquid. This process is distinct from absorption, where the adsorbate penetrates the entire volume of the adsorbent. The driving force for adsorption arises from the unbalanced or residual forces present on the surface atoms or molecules of the adsorbent. These forces seek saturation, leading to the attraction and retention of adsorbate molecules.

Conceptual Foundation: The Nature of Surface Forces

Atoms or molecules within the bulk of a material are surrounded by similar species and experience balanced forces of attraction from all directions. However, atoms or molecules on the surface are not uniformly surrounded.

They possess residual attractive forces directed outwards from the surface. These unbalanced forces are responsible for the surface tension in liquids and the ability of solid surfaces to attract and hold other molecules.

The extent of adsorption depends significantly on the nature of both the adsorbate and the adsorbent, as well as external conditions like temperature and pressure.

Key Principles and Laws Governing Physisorption and Chemisorption

Physisorption (Physical Adsorption):

Physisorption is characterized by weak, non-specific interactions between the adsorbate and the adsorbent. The primary forces involved are Van der Waals forces, which include:

Dipole-dipole interactions: — Between polar molecules.
Dipole-induced dipole interactions: — Between a polar molecule and a non-polar molecule.
London dispersion forces: — Between all types of molecules, arising from temporary fluctuations in electron distribution.

These forces are relatively weak, typically $20-40 \text{ kJ/mol}$, comparable to the enthalpy of liquefaction of gases. This low enthalpy of adsorption means that physisorption is an exothermic process, but the heat released is modest.

Consequently, physisorption is favored at low temperatures. As temperature increases, the kinetic energy of adsorbate molecules increases, making it easier for them to overcome the weak attractive forces and desorb from the surface.

This explains why physisorption decreases with increasing temperature.

Physisorption is also a reversible process. By increasing the temperature or decreasing the pressure, the adsorbed gas can be easily desorbed from the surface. This reversibility is a direct consequence of the weak nature of the Van der Waals forces.

Furthermore, physisorption is non-specific; any gas can physisorb on any solid surface, provided the conditions (low temperature, high pressure) are suitable. Gases that are easily liquefiable (i.e., have higher critical temperatures) are more readily physisorbed because their intermolecular forces are stronger, making them easier to condense onto the surface.

Physisorption can also lead to the formation of multiple layers of adsorbate molecules on the surface, as the Van der Waals forces can act between adsorbed molecules as well as between the adsorbate and the adsorbent.

Chemisorption (Chemical Adsorption):

Chemisorption involves the formation of chemical bonds (covalent, ionic, or metallic) between the adsorbate molecules and the surface atoms of the adsorbent. This process is highly specific, meaning it only occurs if there is a chemical affinity between the adsorbate and the adsorbent. For example, hydrogen gas chemisorbs on transition metals like nickel or platinum, forming metal hydrides on the surface, but not readily on non-metals.

The enthalpy of chemisorption is significantly higher than that of physisorption, typically ranging from $80-240 \text{ kJ/mol}$, which is comparable to the enthalpy of chemical reactions. This strong interaction implies that chemisorption is generally an irreversible process. Once a chemical bond is formed, a substantial amount of energy is required to break it and desorb the adsorbate. Desorption often requires much higher temperatures than physisorption.

Unlike physisorption, chemisorption is often favored at higher temperatures, up to a certain point. This is because chemisorption frequently requires an activation energy. The adsorbate molecules need sufficient kinetic energy to overcome this energy barrier and form chemical bonds with the surface.

Once the bonds are formed, further increase in temperature can lead to desorption or even decomposition of the adsorbed species. Therefore, the extent of chemisorption typically increases with temperature initially, reaches a maximum, and then decreases.

Chemisorption is also characterized by monolayer formation. Each surface atom can typically form only one chemical bond with an adsorbate molecule, leading to a single layer of adsorbed species covering the surface. Once the surface is saturated with a monolayer, no further chemisorption can occur at that site.

Energy Profiles of Adsorption:

Visualizing the energy changes during adsorption helps understand the differences. For physisorption, the potential energy of the system decreases smoothly as the adsorbate approaches the surface, reaching a minimum at the equilibrium adsorption distance.

There is no activation energy barrier. For chemisorption, the potential energy curve often shows an initial increase (activation energy barrier) before a significant drop to a much lower energy minimum, indicating the formation of a strong chemical bond.

This activation energy is crucial for many catalytic processes.

Real-World Applications:

Both types of adsorption are vital in various fields:

Catalysis: — Many industrial catalysts (e.g., in Haber process for ammonia synthesis, hydrogenation of oils) rely on chemisorption. Reactant molecules chemisorb onto the catalyst surface, forming activated complexes that react more readily, and then products desorb.
Gas Masks: — Activated charcoal in gas masks primarily uses physisorption to remove toxic gases and vapors from the air, due to its high surface area and porous structure.
Chromatography: — Separation techniques like gas chromatography and liquid chromatography utilize both physisorption and chemisorption principles for separating mixtures based on differential adsorption onto a stationary phase.
Water Purification: — Activated carbon filters remove impurities from water through physisorption.
Vacuum Technology: — Adsorbents are used to create and maintain high vacuum by adsorbing residual gases.

Common Misconceptions:

1
Adsorption vs. Absorption: — The most common mistake is confusing these two. Adsorption is a surface phenomenon; absorption is a bulk phenomenon. A simple analogy: water on a towel's surface (adsorption) vs. water soaking into the towel (absorption).
2
Chemisorption always requires high temperature: — While many chemisorption processes require an activation energy, leading to an initial increase in adsorption with temperature, excessively high temperatures will eventually lead to desorption due to increased kinetic energy of the adsorbate and weakening of the chemical bonds.
3
Physisorption is useless: — Despite being weak, physisorption is crucial in applications requiring reversible processes, high surface area utilization (multilayer formation), and non-specific removal of substances, such as in gas masks or purification filters.
4
All adsorption is exothermic: — Both physisorption and chemisorption are exothermic processes, meaning they release heat. This is because the formation of attractive forces or chemical bonds leads to a more stable, lower energy state for the system.

NEET-Specific Angle:

For NEET, understanding the distinct characteristics of physisorption and chemisorption is paramount. Questions frequently test the differences in:

Nature of forces (Van der Waals vs. chemical bonds)
Enthalpy of adsorption (low vs. high)
Reversibility (reversible vs. irreversible)
Specificity (non-specific vs. highly specific)
Effect of temperature (decreases with T vs. increases then decreases with T)
Layer formation (multilayer vs. monolayer)
Activation energy (negligible vs. often significant)

Be prepared to identify examples of each type and relate them to practical applications. Numerical problems are less common in this specific subtopic, but conceptual understanding of the factors affecting each type is frequently tested.