The enthalpy of atomisation is influenced by several key factors, including the type of bonding, bond strength, and the electron configuration of the elements involved.

The enthalpy of atomisation is defined as the energy required to convert one mole of a substance in its standard state into individual atoms. This process is inherently endothermic, meaning it requires the input of energy. The amount of energy necessary for atomisation varies based on several factors.

One primary factor is the type of bonding present in the substance. For instance, covalent bonds typically require more energy to break than ionic bonds. This is due to the nature of covalent bonding, which involves the sharing of electrons between atoms, resulting in a stronger bond. Conversely, ionic bonds involve the transfer of electrons from one atom to another, resulting in a comparatively weaker bond that is easier to break.

The strength of the bond is another significant factor affecting the enthalpy of atomisation. Generally, the stronger the bond, the more energy is needed to break it. Factors influencing bond strength include the atomic size of the participating elements and the number of electron pairs shared. For example, a triple bond is stronger than a double bond, which in turn is stronger than a single bond. Consequently, substances containing triple bonds will exhibit higher enthalpies of atomisation than those with double or single bonds.

The electron configuration of an element also plays a crucial role. Elements that possess a full or nearly full outer electron shell tend to require more energy for atomisation, as their electrons are held more tightly by the nucleus. This explains why noble gases, which have complete outer electron shells, exhibit high enthalpies of atomisation.

Additionally, the structural characteristics of a substance can influence its enthalpy of atomisation. For example, substances with a network covalent structure, such as diamond or quartz, exhibit high enthalpies of atomisation due to their extensive networks of covalently bonded atoms. Breaking these robust bonds necessitates a significant amount of energy.

In conclusion, the enthalpy of atomisation is determined by several factors, including the type of bonding, bond strength, electron configuration, and the structural arrangement of the substance. A thorough understanding of these factors can aid in predicting the enthalpy of atomisation for various substances.