are the following statements correct or not? justify your answer . for both a and b.
Dear student,
(b) Ionization enthalpy of Sodium is lower than that of potassium. - Incorrect
Na and K lie in the same group, when we go down the group the atomic size increases. As the atomic size decreases, the outer most electron experiences less attraction by the nucleus, by which less energy is required to remove the outer most electron. Thus K with bigger atomic size has lower ionization energy than Na.
(a) Cesium has the highest ionization enthalpy. - Incorrect
Cesium lies in the alkali metal group and as the whole group it has very low ionization enthalpy. Also since it has very big atomic size, its ionization is even lower than the other alkali metals making it the element with the least ionization enthalpy in the periodic table.
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(b) Ionization enthalpy of Sodium is lower than that of potassium. - Incorrect
Na and K lie in the same group, when we go down the group the atomic size increases. As the atomic size decreases, the outer most electron experiences less attraction by the nucleus, by which less energy is required to remove the outer most electron. Thus K with bigger atomic size has lower ionization energy than Na.
(a) Cesium has the highest ionization enthalpy. - Incorrect
Cesium lies in the alkali metal group and as the whole group it has very low ionization enthalpy. Also since it has very big atomic size, its ionization is even lower than the other alkali metals making it the element with the least ionization enthalpy in the periodic table.
Hope this information clears your doubt about the topic.
If you have any more doubts, just post it on the forum and our experts will help you out as soon as possible.
Regards,