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Understanding Ionization Energy Trends in Atoms

Explore the periodic trends in ionization energy, the energy required to remove valence electrons from atoms. Learn how ionization energy changes with atomic number and across periods and groups in the periodic table, impacting the ease of electron removal. Practice identifying higher ionization energy between elements through example comparisons. Discover the relationship between atomic size, electron distance from the nucleus, and nucleus-electron attraction affecting ionization. Enhance your understanding of atom properties and behavior with this insightful guide.

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Understanding Ionization Energy Trends in Atoms

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  1. Chapter 1 Activity 6: Atoms with More than one Electron

  2. PERIODICITY There are general trends in the properties of atoms and their ions. These trends can be explained using the periodic table.

  3. PERIODICITY Can you name a trend that we have talked about this year? Think about what you graphed • Atomic Mass vs Atomic # • As Atomic # increases, Atomic Mass increases • Atomic Radius vs Atomic # • As Atomic # increases, Atomic Radius increases down a group, but decreases across a period.

  4. Background Electrons can move between energy levels (Bohr’s model supported by line spectra) The nucleus and electrons are attracted to each other (opposites attract) Electrons that are far away from the nucleus can escape the attraction of the nucleus (atoms can lose electrons) Losing an electron is called ionization

  5. Ionization Energy Ionization energy is the energy required to remove a valence electron from an atom. Valence electron= outermost electron that is farthest from the nucleus. period group

  6. Ionization energy vs. atomic number

  7. Ionization Energy in kJ/mol D I

  8. Ionization Energy • Energy needed to remove a loosely held electron from an atom • Decreases as you move down a group • Atom gets bigger, more energy levels • Nucleus is further from the outer most electron (valence electrons) • Nucleus & electron attraction decreases, so it is easier to take an electron away. D

  9. Ionization Energy • Energy needed to remove a loosely held electron from an atom • Increases as you move across a period • Nonmetals hold onto their electrons tighter • Atom is smaller, so nucleus is closer to valence electron making it harder to remove. I D

  10. Ionization Energy Practice He or Xe? (kJ/mol) Which has more ionization energy? He Xe2372 kJ/mol 1170 kJ/mol

  11. Ionization Energy Practice Li or Ne? (kJ/mol) Which has more ionization energy? Li Ne520 kJ/mol 2081 kJ/mol

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