CHEM101 Lecture Notes - Lecture 4: Diamagnetism, Paramagnetism, Electron Configuration
5 Oct 2018
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CHEM101 Lecture 3: Magnetic Properties of the Elements, Periodic Table and Atomic Properties, Core and Valence Electrons, Electrostatic Attraction between Electrons and Nucleus
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CHEM101 Lecture Notes - Lecture 4: Diamagnetism, Paramagnetism, Electron Configuration
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CHEM101 Lecture Notes - Lecture 5: Nonmetal, Effective Nuclear Charge, Atomic Number
Document Summary
The periodic table can be divided into different blocks. The s block this includes group 1 and 2 elements which have the s orbitals being filled. The p block this includes group 13 (3a) and 18 (8a) elements which have the p orbitals being filled. The d block this includes the transition elements group 3 (3b) and 12 (2b) elements which have the d orbitals being filled. The f block this includes the inner transition elements (actinides and lanthanides) which have the f orbitals being filled. Draw the orbital box diagram showing valence electrons, and write the condensed ground-state electron configuration for ga: Cations of the main group elements are formed by loosing electrons until a noble gas electron configuration is achieved. Anions of the main group elements are formed by gaining electrons until a noble gas electron configuration is achieved. Both anions have noble gas electron configuration of ns2np6.
