Introduction
Hybridization of atomic orbitals is a principle described by Pauling and constitutes an important concept in chemistry. Additionally, the description of hybridization depends on the level of the individual in the field. Another important concept related to hybridization is Bent’s Rule which is used to describe the interaction between the different parameters of an atom or a molecule. This paper reviews the article, “Hybridization trends for main group elements and expanding the bent’s rule beyond carbon: more than electronegativity.” (Alabugin, Bresch, & Manoharan, 2014).
Review
In the article, the researchers begin with a simple discussion of the two main concepts that they later evaluate in the paper. They begin with an analysis and description of hybridization in common elements and molecules (Alabugin, Bresch, & Manoharan, 2014, p. 3664). The experiment electronically analyzed the bonds in several compounds consisting of five main elements including B, C, N, O, and F. the main bond analyzed is the H-Y bond whose polarization is dependent on electronegativity. The authors describe hybridization as following a very complicated trend that is dependent on electronegativity and the covalent radius (Alabugin, Bresch, & Manoharan, 2014).
Bent’s rule is limited in application to the elements of the first period. However, Alabugin, Bresch, and Manoharan, (2014) managed to identify a correlation between electronegativity and hybridization (Alabugin, Bresch, & Manoharan, 2014). When two elements X and Y combine, the smaller element (X) forms bonds that link it to the larger element (Y). The electronegativity of the larger element influences the allocation of the p character of the formed bonds. According to Alabugin, Bresch, and Manoharan, (2014), the relationship between the two elements and the bonds formed could be used to expand the application of Bent’s rule to the elements in the second period.
One way that the researchers explained the application of Bent’s rule to the second-period elements is the distribution of the p character into the bonds depending on the radius of the atom and the electronegativity (Alabugin, Bresch, & Manoharan, 2014, p. 3674). They also state that “The bigger and more electronegative a substituent, the more p character will be incorporated into this elements bond.” (Alabugin, Bresch, & Manoharan, 2014, p. 3674). The researchers also went on to describe the influence of lone pairs on the rehybridization range. Accordingly, the elements with lone pairs have a considerably larger rehybridization range compared to those without lone pairs (Alabugin, Bresch, & Manoharan, 2014, p. 3674).
The major part of the discussion focuses on the relationship between atomic size and the relationship with hybridization and bonding. A large s-p gap is present in pure orbitals in O-O and H-H and O-Y polarity are some of the important factors in hybridization. In addition, the researchers highlight the importance of hybridization in influencing the chemical and physical properties of compounds (Alabugin, Bresch, & Manoharan, 2014). The application of Bent’s rule in chemistry is in the analysis of carbon compounds’ structural effects. Additionally, this rule is important in the relationship between hybridization and electronegativity.
Before the research, the relationship between hybridization and electronegativity is only described in a few studies. However, Alabugin, Bresch, and Manoharan (2014) manage to show the relationship between the two about the atomic size and the strength of the bond. They state that the atomic size affects the rehybridization effects and in effect, the chemical and physical properties of the compound formed. The main example provided in the research is the oxygen and fluoride bond that have larger rehybridization effects compared to similar bonds to carbon (Alabugin, Bresch, & Manoharan, 2014). Orbital hybridization trends are dependent on the orbital size and electronegativity when lower period elements form large bonds. The chemical properties of a compound, its reactivity, and its molecular structure are the results of hybridization.
The structure of the research applies chemical properties and terms that make the article complex yet precise. The researchers describe hybridization concerning atomic size and electronegativity for compounds with large bonds. Traditionally, Bent’s rule is limited to elements before carbon in the periodic table. However, the different descriptions in the article demonstrate that the rule could also apply to other elements beyond carbon in the table (Alabugin, Bresch, & Manoharan, 2014). The article is easy to understand and explores the subject consistently and scientifically. In addition, the authors support their hypothesis and use the statistical data to make appropriate conclusions.
Hybridization and Bent’s rule are related in several ways with researchers describing the two concepts in detail. According to Alabugin, Bresch, and Manoharan (2014), the interaction between the different bonds constitutes superhybridization. The hybridization geometry in the paper also provides important information on some of the bonds discussed. The researchers describe the application of Bent’s rule in the elements above carbon in the periodic table. They also manage to strengthen the link between hybridization and electronegativity.
Conclusion
In conclusion, the researchers attempt to show that Bent’s rule applies to elements above carbon in the periodic table. They use hybridization as the basic relationship between the atoms of the selected elements. The bond between atoms determines the level of hybridization and in effect the chemical and physical characteristics of the resultant compounds. The application of the hybridization geometry is adequate to show the relationship between atomic radius, electronegativity, and hybridization. The quality of the research is good and would be applicable in demonstrating the relationship.
References
Alabugin, I., Bresch, S. & Manoharan, M. (2014), Hybridization Trends for Main Group Elements and Expanding the Bent’s Rule beyond Carbon: More than Electronegativity. Journal of Physical Chemistry 118(1), 3663−3677