What is the significance of the terms — ‘isolated gaseous atom’ and ‘ground state’ while defining the ionization enthalpy and electron gain enthalpy? Hint : Requirements for comparison purposes.
Ruhul Amin Alig
❓ What is the significance of the terms — ‘isolated gaseous atom’ and ‘ground state’
while defining the ionization enthalpy and electron gain enthalpy?
Hint : Requirements for comparison purposes.
The terms "isolated gaseous atom" and "ground state" are important when defining ionization enthalpy and electron gain enthalpy, because they provide a standard reference point for comparing the energies involved in these processes.
An isolated gaseous atom is one that is not bonded to any other atoms and is in a state where its electrons are not being affected by any external influences such as nearby ions or molecules. By considering the ionization enthalpy of an isolated gaseous atom, we can measure the energy required to remove an electron from an atom that is not influenced by any external factors.
Similarly, the ground state refers to the lowest possible energy level that an atom can occupy. By considering the electron gain enthalpy of an isolated gaseous atom in its ground state, we can measure the energy released or absorbed when an electron is added to an atom in its most stable energy state.
Using these standard reference points for comparison purposes allows us to make meaningful comparisons between different elements, and to establish trends in the properties of elements across the periodic table. For example, comparing the ionization enthalpies of isolated gaseous atoms allows us to identify trends in the reactivity and chemical behaviour of different elements, while comparing the electron gain enthalpies of isolated gaseous atoms in their ground states allows us to predict the formation and stability of various chemical compounds.
