Chapter 7 - 1 Effective Nuclear Charge Section 7.2 Zeff = Z...

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1 1 Effective Nuclear Charge Z eff = Z – S Z eff = effective nuclear charge Z = number of protons in the nucleus S = average number of electrons between the nucleus and the electron in question The positive charge experienced by outer-shell electrons is always less than the full nuclear charge because the inner-shell electrons partly offset the positive charge of the nucleus. Section 7.2 2 Effective Nuclear Charge & Electron Shielding 3 +++ e - e- e- e- e- e- e- e- e- e- e- +++ +++
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2 4 Atomic Radius Within each group, the atomic radius tends to increase from top to bottom. Within each period, the atomic radius tends to increase moving right to left. Section 7.3 5 Atomic Radius Section 7.3 6 E-Instruction Which of the following atoms has the largest radius? A. N B. As C. F D. Br
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3 7 Ionic Size - Cations No general periodic trend. The comparisons will be different whether an anion is formed or a cation is formed. valence shell = 3 valence shell = 2 Na 1s 2 2s 2 2p 6 3s 1 Na + 1s 2 2s 2 2p 6 Section 7.3 8 Ionic Size - Anions can not make any prediction simply based on valence shell valence shell = 2 valence shell = 2
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Chapter 7 - 1 Effective Nuclear Charge Section 7.2 Zeff = Z...

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