Ross Transition Metals Table - 5' x 3' Banner Classroom Size
$179.00
The First Transition Metals Periodic Table
Designed to be Learned!
1. Explains and Predicts Transition Metal Properties - the behavior of the transition metals can be baffling. Why does scandium show only the 3+ common oxidation state, but vanadium has 2+, 3+, 4+ and 5+ common oxidation states? Why does zinc react with acid, while its neighbor copper does not? Why is gold so unreactive? Why can chromium metal form both the ionic base chromium II hydroxide Cr(OH)2 and the covalent chromic acid H2CrO4 ? This table addresses all of those issues and more.
2. Logical, Easy To Learn Structure - the electron orbital structures that underlie the transition metals are actually easier to learn than the behaviors themselves. This table Requires the least possible student effort to provide the greatest possible accuracy of student recall. Avoids the problem of "unlearning" in the future.
3. Is Scientifically Tenable - This pedagogical model of the d-block elements has fewer errors than the alternatives. Students can build upon it as they increase their knowledge of more sophisticated models.
4. Emphasizes Four Trends - First, the inner core shrinks monotonically from Group 3 to Group 12. Second, the d-orbitals shrink, but in Group 3 are extend outside the inner core. They shrink to a minimum in Group 5, grow to Group 7, shrink again to Group 9, and then disappear beneath the surface of the inner core by Groupp 12. Third, the d-electrons favor groups of 5 electrons, and 10 electrons. Thus, Group 6 and Group 11 elements tend to have just one electron in the outer s-orbital. Fourth, the s-orbitals remain relatively constant in size.
Designed to be Learned!
1. Explains and Predicts Transition Metal Properties - the behavior of the transition metals can be baffling. Why does scandium show only the 3+ common oxidation state, but vanadium has 2+, 3+, 4+ and 5+ common oxidation states? Why does zinc react with acid, while its neighbor copper does not? Why is gold so unreactive? Why can chromium metal form both the ionic base chromium II hydroxide Cr(OH)2 and the covalent chromic acid H2CrO4 ? This table addresses all of those issues and more.
2. Logical, Easy To Learn Structure - the electron orbital structures that underlie the transition metals are actually easier to learn than the behaviors themselves. This table Requires the least possible student effort to provide the greatest possible accuracy of student recall. Avoids the problem of "unlearning" in the future.
3. Is Scientifically Tenable - This pedagogical model of the d-block elements has fewer errors than the alternatives. Students can build upon it as they increase their knowledge of more sophisticated models.
4. Emphasizes Four Trends - First, the inner core shrinks monotonically from Group 3 to Group 12. Second, the d-orbitals shrink, but in Group 3 are extend outside the inner core. They shrink to a minimum in Group 5, grow to Group 7, shrink again to Group 9, and then disappear beneath the surface of the inner core by Groupp 12. Third, the d-electrons favor groups of 5 electrons, and 10 electrons. Thus, Group 6 and Group 11 elements tend to have just one electron in the outer s-orbital. Fourth, the s-orbitals remain relatively constant in size.
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