7.4 Ionization Energy

• What happens as more electrons are removed?

  Ionization energy increases.
• Which blocks show larger I₁ range, s/p or transition metals?

  s- and p-block elements.
• How does atomic size affect ionization energy?

   Smaller atoms have higher ionization energy.
• Why is Boron lower than Beryllium in I₁?

   Due to its higher-energy 2p electron.
• In which order are electrons removed?

  From the highest principal quantum number first.
• What is ionization energy (IE)?

  The energy required to remove an electron from a neutral atom.
•  How does 1st IE change across a period?


  Increases due to higher nuclear charge pulling electrons more tightly.
•  How does 1st IE change down a group?

  Decreases because outer electrons are further from the nucleus.
• What are the two exceptions for IE in Periods 2 & 3?

   Be & B (Period 2), Mg & Al (Period 3).
•  How can higher IEs indicate an element’s likely ionic charge?

   Large jumps in IE show when an element reaches a stable electron configuration, predicting its ion charge.
• How does 2nd and 3rd ionization energy affect charge prediction for elements?

   Elements with low successive IEs until a big jump tend to lose electrons until reaching a stable configuration, like Al³⁺.
• What does I₁ refer to?

  Energy to remove the first electron from a neutral atom.