chill_factor said:because there's a lot of exceptions especially for transition metals.
but in general these are useful:
electronegativity
orbital completion and octet rule
acid/base
symmetry
redox potential
chill_factor said:other atoms nearby: usually doesn't matter except for 2 things: enzymes and catalysts, but neither are atoms.
mather said:anyone?
The main factors that affect the interaction between atoms are the distance between atoms, the strength of the attractive and repulsive forces between atoms, the electronic structure of the atoms, and the presence of any external influences such as temperature or pressure.
The closer two atoms are to each other, the stronger the attractive forces between them become. This is due to the overlap of electron clouds and the resulting increase in electrostatic forces. As the distance between atoms increases, the strength of the interaction decreases.
The electronic structure of atoms determines the number and arrangement of electrons, which in turn affects the strength and type of interactions between atoms. For example, atoms with a full outer electron shell tend to be stable and have weaker interactions, while atoms with incomplete outer shells are more reactive and have stronger interactions.
Attractive forces, such as Van der Waals forces and hydrogen bonds, pull atoms closer together and promote interactions. On the other hand, repulsive forces, like the Pauli exclusion principle and Coulomb's law, push atoms apart and can prevent them from interacting. The balance between these two types of forces determines the overall strength of the interaction between atoms.
Yes, external influences can significantly impact the interaction between atoms. For example, increasing temperature can cause atoms to vibrate more vigorously, weakening their interactions. Similarly, high pressure can compress atoms and bring them closer together, increasing the strength of their interactions.