the general tends of enthalpy changes of atomization, combustion, bond making, bond breaking, formation, neutralization and so on

The general trends of enthalpy changes for atomization, combustion, bond making, bond breaking, formation, neutralization, and so on can be observed by analyzing the energy changes associated with these processes. Here are the steps to understand these trends:

1. Atomization: This process involves breaking a molecule into its individual atoms. The enthalpy change for atomization is typically positive, as energy is required to overcome the attractive forces between the atoms in the molecule.

2. Combustion: Combustion reactions involve the reaction of a substance with oxygen to produce carbon dioxide and water. The enthalpy change for combustion is usually negative, indicating that energy is released during the reaction.

3. Bond making: When new bonds are formed between atoms, energy is released, resulting in a negative enthalpy change. This is because the formation of bonds leads to a more stable arrangement of atoms.

4. Bond breaking: Conversely, breaking existing bonds requires energy input, resulting in a positive enthalpy change. This is because energy is needed to overcome the attractive forces holding the atoms together in a bond.

5. Formation: The enthalpy change for the formation of a compound from its constituent elements can be positive or negative, depending on the specific compound. If the compound is more stable than its constituent elements, the enthalpy change will be negative, indicating energy release. If the compound is less stable, the enthalpy change will be positive, indicating energy absorption.

6. Neutralization: Neutralization reactions involve the reaction of an acid with a base to form a salt and water. The enthalpy change for neutralization is typically negative, indicating energy release.

By analyzing these different processes, we can observe the general trends of enthalpy changes. However, it is important to note that the specific values of enthalpy changes can vary depending on the specific compounds and conditions involved in the reaction.