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chapter 23_24 - Transition Metals Chapter 23 Sections 23.5...

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Unformatted text preview: Transition Metals Chapter 23: Sections 23.5 and 23.7 Coordination Compounds Chapter 24 General Chemistry II, Professor Maggie Ciszkowska General Chemistry II, Professor Maggie Ciszkowska Transition Metals Chapter 23: Sections 23.5 and 23.7 General Chemistry II, Professor Maggie Ciszkowska General Chemistry II, Professor Maggie Ciszkowska Physical Properties of Metals • Read about physical properties of metals in your Textbook . Metallic Bonding Metallic Bonding General Chemistry II, Professor Maggie Ciszkowska General Chemistry II, Professor Maggie Ciszkowska Electron-Sea Model of Metallic Bonding • Read about metallic bonding in your Textbook. Metallic Bonding Metallic Bonding General Chemistry II, Professor Maggie Ciszkowska General Chemistry II, Professor Maggie Ciszkowska Transition Metals Transition Metals General Chemistry II, Professor Maggie Ciszkowska General Chemistry II, Professor Maggie Ciszkowska Physical Properties • Transition metals occupy the d block of the periodic table. • Almost all have two s electrons (exceptions group 6B and group 1B). • Physical properties of transition metals can be classified into two groups: atomic properties ( e.g . size) and bulk properties ( e.g . melting point). • The atomic trends tend to be smooth for the transition metals. Transition Metals Transition Metals General Chemistry II, Professor Maggie Ciszkowska General Chemistry II, Professor Maggie Ciszkowska Transition Metals Transition Metals General Chemistry II, Professor Maggie Ciszkowska General Chemistry II, Professor Maggie Ciszkowska tomic radius reaches a inimum around roup 8B (Fe, Co, Ni), then increases for groups and 2 (Cu and Zn). In general tomic size increases down a roup. Sc Ti V Cr Mn Fe Co Ni Cu Zn Electron Configurations and Oxidation States Even though the ( n - 1) d orbital is filled after the ns orbital, electrons are lost from the orbital with highest n first. That is, transition metals lose s electrons before the d electrons. Example: Fe: [Ar]3d 6 4s 2 Fe 2+ : [Ar]3d 6 d-Electrons are responsible for some important properties: – transition metals have more than one oxidation state, – transition metal compounds are colored (caused by electronic transitions), – transition metal compounds have magnetic properties. Transition Metals Transition Metals General Chemistry II, Professor Maggie Ciszkowska General Chemistry II, Professor Maggie Ciszkowska Electron Configurations and Oxidation States • All oxidation states for metals are positive. • The 2+ oxidation state is common because it corresponds to the loss of both s electrons. (Exception: Sc where the 3+ oxidation state is isoelectronic with Ar.) • The maximum common oxidation state is +7 for Mn....
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