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Chapter 11

Chapter 11. The Periodic Table. I. History of the Periodic Table. Johann Wolfgang Döbereiner and triads John Newlands and the Law of Octaves Dmitri Mendeleev and the 1 st periodic table. Mendeleev’s Periodic Table. Mendeleev’s Predictions. Periodic Law.

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Chapter 11

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  1. Chapter 11 The Periodic Table

  2. I. History of the Periodic Table • Johann Wolfgang Döbereiner and triads • John Newlands and the Law of Octaves • Dmitri Mendeleev and the 1st periodic table

  3. Mendeleev’s Periodic Table

  4. Mendeleev’s Predictions

  5. Periodic Law • Basis: Element arranged according to their atomic masses present a clear periodicity of properties • Modern: The properties of elements repeat periodically when the elements are arranged in increasing order by their atomic numbers

  6. Regions of the Periodic table

  7. Representative Elements -EC • Valence v. core electrons

  8. Representative Elements - Ions • Generalization of atom/ion stability • Usually means 8 valence = octet rule

  9. Transition Elements - EC • Remember the exceptions to filling d orbitals

  10. Periodic Trends – Atomic/ionic radii • Worksheet: Atomic Size

  11. Periodic trends – 1st Ionization Energy • Definition • Increases across a period (L to R), decreases down a group (top to bottom) exceptions

  12. Periodic Trends – 2nd Ionization Energy *The teal colored cells represent ionization energies where the valence shell is now (n-1). (Why do you think there is such a large jump in the ionization energies when the n-1 shell is now valence?)

  13. Periodic Trends - Electronegativity • Definition • Increases across a period (L to R), decreases down a group (top to bottom)

  14. Periodic Trends - All *Note: The electron affinity of an element is the energy given off when a neutral atom in the gas phase gains an extra electron to form a negatively charged ion

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