Class 12 Exam  >  Class 12 Videos  >  L16 : Ionization Enthalpy - D & F Block Elements, Chemistry, Class 12

L16 : Ionization Enthalpy - D & F Block Elements, Chemistry, Class 12 Video Lecture

FAQs on L16 : Ionization Enthalpy - D & F Block Elements, Chemistry, Class 12 Video Lecture

1. What is ionization enthalpy?
Ans. Ionization enthalpy is the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions with a positive charge. It is a measure of the tendency of an atom to lose electrons and form positive ions.
2. How does ionization enthalpy vary across the d-block elements?
Ans. Ionization enthalpy generally increases across the d-block elements from left to right due to increasing nuclear charge and decreasing atomic size. However, there are exceptions or irregularities in this trend due to the presence of partially filled or completely filled d orbitals.
3. Why do transition metals have higher ionization enthalpy compared to s-block elements?
Ans. Transition metals have higher ionization enthalpy compared to s-block elements due to the presence of partially filled d orbitals. The electrons in these d orbitals are closer to the nucleus and experience greater nuclear attraction, making it more difficult to remove them and thus requiring more energy.
4. What factors affect ionization enthalpy in d-block elements?
Ans. The ionization enthalpy in d-block elements is affected by factors such as atomic size, nuclear charge, shielding effect, and the stability of the electronic configuration. Atomic size and nuclear charge generally increase ionization enthalpy, while shielding effect and stability of electronic configuration can decrease it.
5. How does ionization enthalpy change within a d-block series?
Ans. Within a d-block series, ionization enthalpy generally increases as the atomic number increases. This is because of the increasing nuclear charge and decreasing atomic size. However, there may be small irregularities due to the filling of d orbitals and the stability of electronic configurations.
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