Ionization energy decreases in _____ as atomic number increases.
Ionization energy decreases in _____ as atomic number increases.
Step-1:
Ionization energy definition: The ionization energy is the energy needed to remove an electron from the outer shell of isolated atom. It is denoted as IE. The atomic size, effective nuclear charge and screening effect are the factors that influence the ionization energy.
Step-2:
Trend of ionization energy across a period: The ionization energy increases on moving from left to right across the period due to the decrease in size of atom on increasing the atomic number and thus, the electrons in valence shell goes closer to the nucleus. There is more energy needed to remove an electron from outermost shell.
Trend of ionization energy down the group: The ionization energy decreases down the group because of the increase in number of valence shells.
Final answer:
Ionization energy decreases in group as atomic number increases.
Step-1:
Ionization energy definition: The ionization energy is the energy needed to remove an electron from the outer shell of isolated atom. It is denoted as IE. The atomic size, effective nuclear charge and screening effect are the factors that influence the ionization energy.
Step-2:
Trend of ionization energy across a period: The ionization energy increases on moving from left to right across the period due to the decrease in size of atom on increasing the atomic number and thus, the electrons in valence shell goes closer to the nucleus. There is more energy needed to remove an electron from outermost shell.
Trend of ionization energy down the group: The ionization energy decreases down the group because of the increase in number of valence shells.
Final answer:
Ionization energy decreases in group as atomic number increases.
