periodic variations in nucleus, ions etc
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periodic variations in nucleus, ions etc

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Questions and Answers

Which electron configuration is described in the text?

  • 1s^2 2s^2 2p^6
  • 2s^2 2p^4 3s^1
  • 2s^2 2p^4
  • 1s^2 2s^2 2p^4 (correct)

    • Why is removing an electron from a cation more difficult than from a neutral atom?

  • Due to the stronger electrostatic attraction to the cation. (correct)
  • Due to the larger size of the cation.
  • Due to the presence of more electrons in the cation.
  • Due to the lower positive charge on the cation.

    • What happens to successive ionization energies for one element?

  • They remain constant.
  • They become negative.
  • They fluctuate.
  • They increase. (correct)
  • They decrease.

    • Why is the rapid increase in ionization energy observed after the third ionization for Sc and Ga?

    <p>Due to the removal of core electrons.</p> Signup and view all the answers

    In general, what happens to ionization energies as you move across a period from left to right?

    <p>They increase.</p> Signup and view all the answers

    Why is removing an electron from a cation with a higher positive charge more difficult?

    <p>Due to an increase in electrostatic attraction.</p> Signup and view all the answers

    What factor makes removing an electron from Tl easier compared to Al?

    <p>Distance from the nucleus</p> Signup and view all the answers

    Why does IE3(Al) require more energy than IE1(Al)?

    <p>Al2+ exerts a stronger pull on electrons compared to Al.</p> Signup and view all the answers

    Which element has the highest value for IE1?

    <p>O</p> Signup and view all the answers

    What type of ions exert a stronger pull on electrons compared to neutral atoms?

    <p>Cations</p> Signup and view all the answers

    Which element has the highest value for IE2?

    <p>Pb</p> Signup and view all the answers

    Which element would have the highest value for IE1?

    <p>Br</p> Signup and view all the answers

    What factor contributes to the difficulty in removing an electron from a cation compared to a neutral atom?

    <p>Greater electrostatic attraction to the cation</p> Signup and view all the answers

    Why is removing an electron from Al easier than from Tl?

    <p>Tl's electron is in a higher n orbital</p> Signup and view all the answers

    What is the trend observed in ionization energies as you move from Al to Tl?

    <p>Increasing due to stronger pull on electrons</p> Signup and view all the answers

    What makes removing an electron from Al(Al2+) require more energy than from Al?

    <p>Cation Al2+ exerts a stronger pull on electrons</p> Signup and view all the answers

    Compared to Ba, which element is expected to have the lowest value for IE1?

    <p>O</p> Signup and view all the answers

    What contributes to the large increase in ionization energies after the third ionization for Sc and Ga?

    <p>Removal of core electrons</p> Signup and view all the answers

    What makes removing an electron from a cation with a higher positive charge more difficult?

    <p>Greater electrostatic attraction</p> Signup and view all the answers

    Which element has the lowest value for IE3?

    <p>Pb</p> Signup and view all the answers

    Which element has the lowest value for IE1: O, Po, Pb, or Ba?

    <p>Ba</p> Signup and view all the answers

    Which process requires more energy: IE1 for Al or IE3 for Al?

    <p>IE3 for Al</p> Signup and view all the answers

    Explain why IE1(Tl) < IE1(Al).

    <p>Removing the 6p1 electron from Tl is easier than removing the 3p1 electron from Al due to the higher n orbital being farther from the nucleus.</p> Signup and view all the answers

    Predict the order of increasing energy for the following processes: IE1 for Ca, IE1 for Sc, IE2 for Ge, IE3 for As.

    <p>IE1 for Sc &lt; IE1 for Ca &lt; IE3 for As &lt; IE2 for Ge</p> Signup and view all the answers

    Which ionization energy process involves removing a core electron?

    <p>IE2 for Na</p> Signup and view all the answers

    Why is removing an electron from a cation with a higher positive charge more difficult?

    <p>The stronger positive charge of the cation exerts a greater pull on the electron, making it harder to remove.</p> Signup and view all the answers

    Compare the ionization energies for K and Ca.

    <p>IE1 for K &lt; IE1 for Ca</p> Signup and view all the answers

    Explain why IE1(Al) < IE3(Al).

    <p>The cation Al^2+ exerts a stronger pull on the electron during the third ionization, requiring more energy.</p> Signup and view all the answers

    Which element exhibits a rapid increase in ionization energy after the third ionization?

    <p>Sc and Ga</p> Signup and view all the answers

    Explain why IE3(Al) requires more energy than IE1(Al).

    <p>The cation Al^2+ exerts a stronger pull on the electron during the third ionization compared to the neutral Al atom.</p> Signup and view all the answers

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