CHE 2A Lecture Notes - Lecture 9: Isoelectronicity, Noble Gas, Electron Affinity
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CHE 2A Full Course Notes
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Give an example: the following species are isoelectronic with the noble gas kr. Arrange them in order of increasing radius: rb+, y3+, se2-, br-, sr2: compare the elements na, o, mg and p. place the elements in order of increasing. Rb 1 sru y3t set br ionization energy: electron affinities can be negative, positive, or neutral. Na p o mg case with ionization energies. Chlorine is most likely to: act as an oxidizing agent, have a small first ionization energy, act as a reducing agent, form a basic oxide, release electrons readily to other atoms. Part 2: lewis structures lose e oxidation: write a plausible lewis structure for each of the following molecules: a. fcl t et c. hoclo n, ch3cho. Replace it with a more acceptable structure: assign formal charges to the atoms in these structures: Fck e o 3 1: si in sif6.
