Define ionization enthalpy and explain it trends in groups and periods.
Answers
Answer:
ionisation enthalpy is defined as the energy needed to remove an electron from the gaseous atom, where the smaller the atom higher is the energy needed to remove the electron since there is a high attraction force on the outermost electron in the periodic table, from left to right, the size of atom decreases.
Answer:
Ionization enthalpy of an element can be defined as the amount of energy required to remove an electron from an isolated gaseous atom in its gaseous state.
Trends in ionisation enthalpy in a group:
The first ionisation enthalpy of elements decreases as we move down in a group. While moving down in a group, atomic number increases and the number of shells also increases. Outermost electrons are far away from the nucleus and thus can be removed easily.
Trends in ionisation enthalpy across a period:
As we move from left to right across a period,ionisation energy of elements increases. This is due to the decrease in size of atoms across a period. The valence electrons get closer to the nucleus of an atom as we move from left to right due to increased nuclear charge.
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