P. 208 – 58 Write electron configurations for the 2+ cations: a.Feb. Coc. Ni P. 208 – 59 Write electron configurations for the 3+ cations: a.Chromium b.Manganese.

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Presentation transcript:

P. 208 – 58 Write electron configurations for the 2+ cations: a.Feb. Coc. Ni P. 208 – 59 Write electron configurations for the 3+ cations: a.Chromium b.Manganese c.Iron

P. 208 – 66 If ionic compounds are composed of charged particles (ions), why isn’t every ionic compound either positively or negatively charged? P. 196 – 12 Use electron dot structures to determine formulas of the ionic compounds formed when a.Potassium reacts with iodine b.Aluminum reacts with oxygen P What is the formula of the ionic compound composed of calcium cations and chloride anions?

P. 199 – 22 Why do ionic compounds conduct electricity when they are melted or dissolved in water? P. 203 – 23 How do chemists model the valence electrons in metal atoms? P. 203 – 27 Why is it possible to bend metals but not ionic crystals?

P. 207 – 46 Most ionic substances are brittle. Why? 47 – Explain why molten MgCl 2 does conduct an electric current although crystalline MgCl 2 does not? 48 – Explain briefly why metals are good conductors of electricity. 51 – Explain why the properties of all steels are not identical.

P. 203 – 25 Why are alloys more useful than pure metals?