The Formation of Chemical Bonds

During the formation of chemical bonds, it has been established that atoms of some elements have a greater tendency to attract the valence electrons involved in the bond as compared to others. In modern chemistry generally, the electronegativity of metals is always lower and increases from left to right across the staple periodic table. This is basically because metals have a fewer number of electron valences hence tend to enhance their stability by losing electrons to form cations. In addition, a potential increase in the atomic nuclear charge contributes to the trend. However, research has discovered that some transition metals have a higher electronegativity than the electrons on their right thus exempting them from the trend. 

This can be attributed to the fact that transition metals are characterized by partially filled subshells within their free cations. Therefore, the elements of transition metals gradually decrease from left to right across the periodic table row. This is basically a result of an expeditious increase in effective nuclear charge in addition to increasing atomic number across the row. Also, the atomic radii of transition metals increase down the group with the increase in atomic size. Moreover, there is a lower increase in ionization energies of transition metals across the table. Finally, transition metals are steadily less reactive and highly noble hence results in a unique electronegativity trend from right to left across the periodic table. As a result of unique traits, therefore, transition metals will always remain an exemption from the electromagnetic trends of metals.