Which bond is the most stable?

Sigma bonds are the strongest covalent chemical bonds. Sigma bonds also occur when an s and a p orbital share a pair of electrons or when two p orbitals that are parallel to the internuclear axis share a pair of electrons (see Figure 3-4).

sciencedirect.com - Covalent Bond - an overview | ScienceDirect Topics

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1 Introduction

The coordination compounds found their applications long before the establishment of coordination chemistry. Bright red coloured alizarin dyes were under applications even before the fifteenth century. This bright red dye, now characterized as a chelated complex of hydroxyanthraquinone with calcium and aluminium metal ions, is shown in Figure 1. Figure 1. Structure of alizarin dye. Later, in the sixteenth century, the formation of a well-known member of today's coordination chemistry family, the tetraamminecupric ion [Cu(NH 3 ) 4 ]+2, was recorded upon contact between brass alloy and ammonium chloride. Addition of Prussian blue Fe 4 [Fe(CN) 6 ] 3 ·xH 2 O increased the use of coordination compounds in dyes and pigments. A platinum complex K 2 [PtCl 6 ] offered an application for the refinement of platinum metal. Thus, before the coordination chemistry was structured, the coordination compounds, complexes and chelates found their applications. A systematic investigation of structure and bonding in coordination chemistry began with the inquisitiveness of Tassaert (1798), which was extended by distinguished chemists like Wilhelm Blomstrand, Jorgensen and Alfred Werner [1] until the end of the nineteenth century. In the events, Werner's coordination theory (1893) became the base of the modern coordination chemistry. It is worth noting that the electron was discovered subsequent to Werner's theory. The bonding in compounds like CoCl 3 and NH 3 were easily understood and explained and hence such compounds were regarded as simple compounds. For instance, the +3 formal oxidation of cobalt in cobalt chloride is balanced by three uni-negative chloride ions and the coexistence of these ionic moieties to form a molecule is understood and explained. Similarly, the valence shell (n = 2) of nitrogen (N = 7) contains five electrons and four orbitals (2s, 2p x , 2p y and 2p z ). Keeping an electron pair in one of these orbitals while the other three remains half filled, an opportunity for three hydrogen atoms to contribute one electron each for the formation of a covalent bond with nitrogen, can also be explained. Thus an ammonia molecule has three N H covalent bonds and one lone pair of electrons over the nitrogen atom. It is worth noticing here that all the valencies of all the atoms in both the molecules are fully satisfied and hence there is no further scope of bonding. A ‘complex’ situation arises when one comes to know that the molecule CoCl 3 can encompass six ammonia molecules, resulting into a third independent entity. This situation was fully understood and explained by Werner's coordination theory, followed by naming the entity as ‘complex’.

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Does bonding create energy?

Energy is released when bonds form. Bond formation represents a stable configuration for atoms, sort of like relaxing into a comfy chair.

thoughtco.com - Is Energy Released When Chemical Bonds Are Formed? - ThoughtCo

One of the biggest challenges for chemistry students is understanding whether energy is required or released when chemical bonds are broken and formed. One reason this can be confusing is that a complete chemical reaction can go either way. Exothermic reactions release energy in the form of heat, so the sum of the energy released exceeds the amount required. Endothermic reactions absorb energy, so the sum of the energy required exceeds the amount that is released. In all types of chemical reactions, bonds are broken and reassembled to form new products. However, in exothermic, endothermic, and all chemical reactions, it takes energy to break the existing chemical bonds and energy is released when the new bonds form.

Breaking Bonds → Energy Absorbed

Forming Bonds → Energy Released

Breaking Bonds Requires Energy

You have to put energy into a molecule to break its chemical bonds. The amount needed is called the bond energy. After all, molecules don't spontaneously break. For example, when is the last time you saw a pile of wood spontaneously burst into flames or a bucket of water turn into hydrogen and oxygen? Energy must be applied for these reactions to occur.

Forming Bonds Releases Energy

Energy is released when bonds form. Bond formation represents a stable configuration for atoms, sort of like relaxing into a comfy chair. You release all your extra energy when you sink into the chair and it takes more energy to get you back up again.

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