7.periodic trends key

7.periodic trends key - Chem 105 Nielson Recitation 10/2/07...

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Chem 105 Nielson Recitation 10/2/07 Atomic and ionic radius Predicting ions Ionization energy Electron Affinity Group properties 1. Identify the valence electrons of the following elements. a. Cl b. Ge c. La d. Cu 2. Write the electron configuration of the following ions. a. Cu + b. Br - c. Ba 2+ d. P 3- e. Sc 3+ 3. Predict the ion(s) formed from each of the following elements. a. Zn (1) b. In (2) c. Pb (2) d. Ti (2) 4. Predict the larger atomic radius in each pair. a. Mg Ba b. Si Sn c. Sc Ti d. K Ba
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5. Arrange the following groups of elements in order of increasing IE. a. C, Si, Ne Ans. Si < C < Ne b. Li, K, C, N Ans. K < Li < C < N c. Na, Mg, O, P Ans. Na < Mg < P < O 6. Define Z eff , the effective nuclear charge. Z eff = Z – S, where Z = nuclear charge and S = screening constant/shielding power of electrons. The nuclear charge felt by an electron is always less than Z (except for a one electron element like H). E of the electron α -(Z eff ) 2 /n 2 (basically Coulomb’s law!) a. Compare the Z eff experienced by the highest energy electrons in Na, Cl, and K. Short answer: Z eff follows the same trend as Z, it increases going across a period and down a group. Long answer:
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This note was uploaded on 12/09/2009 for the course CHEM 105 taught by Professor Macedone during the Spring '07 term at BYU.

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7.periodic trends key - Chem 105 Nielson Recitation 10/2/07...

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