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Ionization enthalpy - Elements & Periodicity Video Lecture - Class 11

FAQs on Ionization enthalpy - Elements & Periodicity Video Lecture - Class 11

1. What is ionization enthalpy?
Ans. Ionization enthalpy is the energy required to remove one mole of electrons from one mole of gaseous atoms or ions to form one mole of gaseous ions with a single positive charge.
2. How does ionization enthalpy vary across the periodic table?
Ans. Ionization enthalpy generally increases from left to right across a period and decreases from top to bottom within a group in the periodic table. This is due to the increasing nuclear charge and decreasing atomic size.
3. Why does ionization enthalpy increase across a period?
Ans. Ionization enthalpy increases across a period because the effective nuclear charge increases, resulting in a stronger attraction between the electrons and the nucleus. As a result, more energy is required to remove an electron.
4. Why does ionization enthalpy decrease down a group?
Ans. Ionization enthalpy decreases down a group because the atomic size increases, leading to a weaker attraction between the electrons and the nucleus. The outermost electrons are further away from the nucleus, making it easier to remove them.
5. Which element has the highest ionization enthalpy?
Ans. Helium (He) has the highest ionization enthalpy among all the elements. This is because it has a stable electron configuration with a full outermost shell, making it difficult to remove an electron.
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