Ionization Energy Insights Looking at Trends in Elements in Group IV

The video discusses the ionization energy trends in the carbon family, noting a decrease from carbon to lead. Carbon has high ionization energy due to its small size and high electronegativity. As we move down the group, ionization energy decreases due to increased atomic size. Germanium and tin show reduced ionization energy due to filled 3D and 4D orbitals, while lead has the lowest ionization energy due to effective screening by filled 4F orbitals.

What is the trend in ionization energy as you move from carbon to silicon?

• It increases due to a decrease in atomic size.

• It decreases due to an increase in atomic size.

• It fluctuates randomly.

• It remains constant.

Why does carbon have a higher ionization energy compared to other elements in its group?

• Because its valence electron is strongly attracted to the nucleus.

• Because it has a lower electronegativity.

• Because it has a larger atomic size.

• Because it has more protons than other elements.

What effect do the filled 3D and 4D orbitals have on the ionization energy of germanium and tin?

• They have no effect on the ionization energy.

• They cause the ionization energy to fluctuate.

• They increase the ionization energy.

• They decrease the ionization energy due to shielding.

Which element in the carbon family has the lowest ionization energy?

• Silicon

• Tin

• Lead

• Carbon

What is the role of 4F orbitals in the ionization energy of lead?

• They effectively shield the valence electrons, reducing ionization energy.

• They increase the ionization energy by attracting valence electrons.

• They have no role in the ionization energy.

• They cause the ionization energy to increase due to repulsion.