it is the energy required for a mole of atom to loose a mole of electron.
The ionisation enthalpy of potassium is lower than that of sodium.
yes, it is correct.
This value is identical for isotopes.
The elements with the highest ionization enthalpy are helium, neon, and argon. These noble gases have full valence electron shells and are very stable, making it difficult to remove an electron from them.
The properties like electronegativity , ionisation energy , enthalpy changes vary periodically with atomic number.
The ionisation enthalpy of potassium is lower than that of sodium.
yes, it is correct.
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This value is identical for isotopes.
The elements with the highest ionization enthalpy are helium, neon, and argon. These noble gases have full valence electron shells and are very stable, making it difficult to remove an electron from them.
atoms having low Ionisation enthalpy and ones having high electronegativity form ionic bond
The properties like electronegativity , ionisation energy , enthalpy changes vary periodically with atomic number.
Due to low ionisation enthalpy, metals easily lose an electron and attain positive charge. eg. Na+, K+
Oxygen has less ionization enthalpy than fluorine because oxygen has a smaller nuclear charge compared to fluorine, leading to weaker attraction between the nucleus and the electrons. This makes it easier to remove an electron from an oxygen atom compared to a fluorine atom.
Ionisation potential and ionisation energy are essentially the same concept - they both refer to the amount of energy required to remove an electron from an atom or molecule. The terms are often used interchangeably in practice.
To calculate the enthalpy change of a reaction, subtract the total enthalpy of the reactants from the total enthalpy of the products. This difference represents the enthalpy change of the reaction.
The enthalpy vs temperature graph shows how enthalpy changes with temperature. It reveals that as temperature increases, enthalpy also tends to increase. This indicates a positive relationship between enthalpy and temperature.