The best way to describe the formation of a bond depends on the type of bond shown in the figure. Generally, chemical bonds form through either the transfer or sharing of electrons between atoms.

• Ionic bonds form when one atom (usually a metal) transfers electrons to another atom (usually a non-metal), resulting in oppositely charged ions that attract each other.
• Covalent bonds form when two non-metal atoms share electrons to fill their outer electron shells.
• Metallic bonds involve a "sea of electrons" shared among metal atoms.

Without the exact figure, in typical cases where a bond is formed between a carbon atom and a nitrogen atom (common in biological molecules), the bond is usually a covalent bond formed by sharing electrons. If the bond is shown as an interaction involving partial charges or hydrogen atoms and electronegative atoms like oxygen or nitrogen, it may be a hydrogen bond, which is a weaker intermolecular force. Hence, the best description usually is that the bond shown is formed either by sharing electrons (covalent bond) or by transfer of electrons (ionic bond) depending on the atoms involved and the context of the figure. If more specifics about the figure (like the atoms involved or the bond type depicted) can be provided, a more precise answer can be given. Based on general knowledge and typical representations:

• A covalent bond would be described as formed by shared electrons between atoms.
• An ionic bond would be described as formed by electron transfer resulting in positive and negative ions.
• A hydrogen bond would be described as a weak attraction between a hydrogen atom covalently bonded to an electronegative atom and another electronegative atom.

This general framework aligns with standard chemistry explanations of bond formation.