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Which of the following is incorrect?

Correct answer: A. IE1 of Li > IE1 of Be

  • A. IE1 of Li > IE1 of Be
  • B. IE1 of Be > IE1 of B
  • C. IE1 of Li < IE1 of Ca
  • D. IE1 of He > IE1 of Ne

Explanation

The incorrect statement is Option A: IE1 of Li > IE1 of Be. This is incorrect because ionization energy increases across a period from left to right, and Be is to the right of Li in the same period. Consequently, Be has a higher ionization energy than Li.Option B is incorrect because, while ionization energy generally increases across a period, B actually has a slightly lower ionization energy than Be due to its electron configuration.Option C is correct in stating that Li has a lower ionization energy than Ca, which is influenced by the position of Ca further down the periodic table.Option D accurately reflects that He has a higher ionization energy than Ne, as ionization energy decreases down a group.

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About Periodic Properties and Trends

Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.

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