What is the density of platinum

7. Ionization energy

8. Lattice energy

9. Free energy

10. Activation energy

Explanation:

I. Ionization energy: The energy required to convert a ground-state atom in the gas phase to a gaseous positive ion. Thus, it is the minimum energy required to remove or detach an electron from a neutral atom in a gaseous state. Generally, atoms with relatively large atomic radii tend to have a low ionization energy.

II. Lattice energy: The energy change that occurs in the conversion of an ionic solid to widely separated gaseous ions. This ultimately implies that, it is the energy generated during the conversion of an ionic solid into gaseous ions and as such is a measure of the cohesive force binding the ions of an ionic compound using the Born-Haber cycle.

III. Free energy: the energy in a chemical or physical change that is available to do useful work. Thus, it is a thermodynamic quantity that measures the maximum capacity of a system to do work at constant temperature and pressure.

IV. Activation energy: The energy required to form the transition state in a chemical reaction. When the activation energy of a reaction is low, the rate of the reaction would be faster. Therefore, an enzyme speeds or catalyzes the rate of a reaction by lowering its activation energy.