11 - Chemistry 1000 Lecture 11 The alkali metals Marc R...

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Chemistry 1000 Lecture 11: The alkali metals Marc R. Roussel
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Naming monatomic ions and simple ionic compounds Main group metal cations: name of metal + word “ion” Examples: sodium ion (Na + ), magnesium ion (Mg 2+ ) Monatomic anions: replace -ine in element name by -ide . The word “ion” may be used at times, but isn’t strictly necessary. Examples: fluoride (ion) (F - ), oxide (ion) (O 2 - ) Simple ionic compounds: Name the cation first, then the anion. No account is taken of the numbers of ions of each type since these numbers are known from the charges of the ions. Examples: sodium chloride (NaCl), magnesium fluoride (MgF 2 ), lithium oxide (Li 2 O)
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The alkali metals I Group 1, except H I Soft metals I Lowest ionization energies and electronegativities in periodic table Li Na K Rb Cs I 1 / kJ mol - 1 520.2 495.6 418.8 403.0 375.7 χ 1.0 0.9 0.8 0.8 0.7
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Redox chemistry I Alkali metal ions have among the most negative reduction potentials Reduction potential: Half-cell potential for gaining electrons In this case, M + (aq) + e - M (s) Li + Na + K + Rb + Cs + E / V - 3 . 040 - 2 . 71 - 2 . 931 - 2 . 98 - 3 . 026 = The alkali metals are very powerful reducing agents.
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