Exams › JEE Main › Chemistry

Given below are two statements : Statement (I) : The first ionization energy of Pb is greater than that of Sn Statement (II) : The first ionization energy of Ge is greater than that of Si. In the light of the above statements, choose the correct answer from the options given below : (1) Statement I is true but Statement II is false (2) Both Statement I and Statement II are false (3) Statement I is false but Statement II is true (4) Both Statement I and Statement II are true

1. Statement I is true but Statement II is false
2. Both Statement I and Statement II are false
3. Statement I is false but Statement II is true
4. Both Statement I and Statement II are true

Correct answer: Statement I is true but Statement II is false

Solution

Statement I is correct because lead (Pb) has a higher ionization energy than tin (Sn) due to its position in the periodic table, where Pb is further down and experiences stronger effective nuclear charge. Statement II is false because germanium (Ge) has a lower first ionization energy than silicon (Si), as Ge is in a higher period and has more electron shielding.

Related JEE Main Chemistry questions

• Which of the following sequences is incorrectly arranged with respect to the property mentioned alongside it?
• For the element having atomic number 120, which symbol and IUPAC systematic name are correctly paired?
• Which sequence correctly represents the ionization energies of carbon, nitrogen, and oxygen atoms?
• Identify the sequence that is not arranged correctly.
• Arrange the following species in order of decreasing radius: F$^-$, F, O, and O$^{2-}$.
• Identify the statement that is not correct:

⚔️ Practice JEE Main Chemistry free + battle 1v1 →