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Dmitri Mendeleev

Dmitri Mendeleev. “The elements, if arranged according to their atomic weights, exhibit an apparent periodicity of properties.”. Periodic Trends. St. Kn. Lt. Fi. Dt. E. Oj. Ns. A. Pr. J. Q. Ch. Br. T. Id. Rx. G. Mc. H. Atomic Radius. 1. Atomic Radius. Across Period

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Dmitri Mendeleev

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  1. Dmitri Mendeleev “The elements, if arranged according to their atomic weights, exhibit an apparent periodicity of properties.”

  2. Periodic Trends

  3. St Kn Lt Fi Dt E Oj Ns A Pr J Q Ch Br T Id Rx G Mc H Atomic Radius

  4. 1. Atomic Radius Across Period Atomic size DECREASES Because nuclear charge (# p+) increases, as e- are added to same n, pulls e- in tighter Down Group Atomic size INCREASES Because more n (shells), more shielding, e- further away from nucleus

  5. Sc Kn Lt Fi Dt E Oj Ns A Pr J Q Ch Br T Id Rx G Mc H Electronegativity

  6. 2. Electronegativity The ability to attract e- Across Period EN INCREASES Because nuclear charge (# p+) increases Down Group EN DECREASES Because more n, more shielding, e- further away from nucleus

  7. Sc Kn Lt Fi Dt E Oj Ns A Pr J Q Ch Br T Id Rx G Mc H Ionization Potential

  8. 3. Ionization Potential/Energy IE: Energy required to remove e- Higher the IE: more difficult to remove e- Across Period IE INCREASES* * with decrease @ each subshell Why? Down Group IE DECREASES Why?

  9. 4. Ionic Radius Ion- Charged atom Cation Positive (+) ion (neutral atom looses e-) Anion Negative (-) ion (neutral atom gains e-)

  10. St Kn Lt Fi Dt E Oj Ns A Pr J Q Ch Br T Id Rx G Mc H Ionic Radius

  11. 4. Ionic Radius Across Period IR DECREASES* * with jump up in size @ metalloids Down Group IR INCREASES Compare to neutral atom Ex. Br Valence e-are the outermost e- of an atom

  12. 5. Metallic Properties Across Period MP DECREASES Down Group MP INCREASES

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