Question

Which one of the following elements will require the highest energy to take out an electron from them?

• A. Ge
• B. C
• C. Si
• D. Pb

Answer 1

Answer: (B)

C

Answer 2

Ionization energy is the energy required to remove an electron from a gaseous atom. All the given elements (C, Si, Ge, Pb) belong to Group 14 of the periodic table. The general trend for ionization energy in a group is that it decreases as we move down the group. This is because atomic size increases down a group, leading to a weaker attraction between the nucleus and the outermost electrons due to increased distance and shielding effect.

The order of these elements in Group 14 from top to bottom is:

1. Carbon (C)
2. Silicon (Si)
3. Germanium (Ge)
4. Lead (Pb)

Following the trend, Carbon (C) is at the top of the group, meaning it has the smallest atomic size among these elements and the strongest attraction for its valence electrons. Therefore, it will require the highest energy to remove an electron.

The order of ionization energy will be: C > Si > Ge > Pb.

Thus, Carbon (C) will require the highest energy to take out an electron.