ABSTRACT:
In this article, we will discuss about the hybridization of atomic orbitals. Hybridization is the process of formation of degenerate molecular orbitals (having same energy and shape) from atomic orbitals. We will discuss here three types of hybridization sp, sp2 and sp3. This theory provides a framework for understanding the spatial arrangement of atoms in a molecule based on the hybridization of atomic orbitals. In this article, we will explore the concept of hybridization in detail, along with examples and references.
INTRODUCTION OF HYBRIDIZATION OF ATOMIC ORBITALS:
In the field of chemistry, understanding the structure and bonding of molecules is crucial for predicting their properties and behavior. Hybridization of atomic orbitals is a fundamental concept that helps explain the formation of chemical bonds and the resulting molecular geometries. Hybridization is a process in which atomic orbitals mix to form new hybrid orbitals with different shapes and energies. This process occurs when atoms form covalent bonds by sharing electrons. Hybrid orbitals are formed by combining atomic orbitals from the same atom or different atoms involved in bonding.
TYPES OF HYBRIDIZATION OF ATOMIC ORBITALS:
There are several types of hybridization that can occur, depending on the number and types of atomic orbitals involved. The most common types of hybridization are sp, sp2, and sp3 hybridization.
1. SP HYBRIDIZATION:
In sp hybridization, one s orbital and one p orbital from the same atom combine to form two sp hybrid orbitals. These orbitals are linear in shape and oriented at an angle of 180 degrees to each other. An example of sp hybridization found in the molecule ethyne (C2H2), where the carbon atoms sp hybridized and form a triple bond.
2. SP2 HYBRIDIZATION:
In sp2 hybridization, one s orbital and two p orbitals from the same atom combine to form three sp2 hybrid orbitals. These orbitals are trigonal planar in shape and oriented at an angle of 120 degrees to each other. An example of sp2 hybridization found in the molecule ethene (C2H4), where the carbon atoms sp2 hybridized and form a double bond.
3. SP3 HYBRIDIZATION:
In sp3 hybridization, one s orbital and three p orbitals from the same atom combine to form four sp3 hybrid orbitals. These orbitals are tetrahedral in shape and oriented at an angle of 109.5 degrees to each other. An example of sp3 hybridization found in the molecule methane (CH4), where the carbon atom sp3 hybridized and forms four single bonds.
OTHER EXAMPLES OF HYBRIDIZATION OF ATOMIC ORBITALS:
1. WATER (H2O):
In water, the oxygen atom is sp3 hybridized, forming four sp3 hybrid orbitals. Two of these orbitals overlap with the 1s orbitals of hydrogen atoms to form two sigma (σ) bonds, resulting in a bent molecular geometry.
2. AMMONIA (NH3):
In ammonia, the nitrogen atom is sp3 hybridized, forming four sp3 hybrid orbitals. Three of these orbitals overlap with the 1s orbitals of hydrogen atoms to form three sigma (σ) bonds, resulting in a pyramidal molecular geometry.
CONCLUSION:
Hybridization of atomic orbitals is a fundamental concept in chemistry that helps explain the formation of chemical bonds and the resulting molecular geometries. By combining atomic orbitals, hybrid orbitals are formed, which determine the spatial arrangement of atoms in a molecule. The examples discussed in this article illustrate the diverse range of hybridization types and their impact on molecular structure. By understanding hybridization, chemists can gain insights into the properties and behavior of different compounds, enabling them to make informed predictions and design new molecules for various applications.
REFERENCES:
Pauling, L. (1931). The nature of the chemical bond. Application of results obtained from the quantum mechanics and from a theory of paramagnetic susceptibility to the structure of molecules. Journal of the American Chemical Society, 53(4), 1367-1400. https://pubs.acs.org/doi/10.1021/ja01355a027
Miessler, G. L., & Tarr, D. A. (2013). Inorganic chemistry. Pearson Education. https://celqusb.files.wordpress.com/2017/12/inorganic-chemistry-g-l-miessler-2014.pdf
Housecroft, C. E., & Sharpe, A. G. (2012). Inorganic chemistry. Pearson Education. https://cdn.bc-pf.org/resources/chemistry/inorg_chem/Housecroft_sharpe_inorganic_chemistry.pdf
