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chalkboard challenge: the periodic table and periodicity

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chalkboard challenge: the periodic table and periodicity

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    1. Chalkboard Challenge:The Periodic Table and Periodicity Copyright © 2002 Glenna R. Shaw and FTC Publishing All Rights ReservedCopyright © 2002 Glenna R. Shaw and FTC Publishing All Rights Reserved

    3. Most of the elements on the Table are of this type, exhibiting properties of luster, electrical conductivity, ductility, and malleability. Regions of the Table, I for 100

    4. The unreactive, Group 18 elements. Regions of the Table, I for 200

    5. Elements 90-103 Regions of the Table, I for 300

    6. The highly-reactive, Group 1 elements. Regions of the Table, I for 400

    7. The highly-reactive, Group 17 elements. Regions of the Table, I for 500

    8. This broad classification of elements consist of insulators, and are generally gases or brittle solids at room temperature. Regions of the Table, II for 100

    9. These “stair-step” elements exhibit properties of both insulators and conductors. Regions of the Table, II for 200

    10. Elements 58-71. Regions of the Table, II for 300

    11. The Group 11 elements were often used in historical times as currency. Regions of the Table, II for 400

    12. The Group 2 elements take a 2+ charge when they become cations. Regions of the Table, II for 500

    13. This Russian scientist is credited with inventing the Table, around the year 1870. History of the Table for 100

    14. Mendeleev based his Table on this property of the elements. History of the Table for 200

    15. The British scientist Henry Moseley modified Mendeleev’s Table, using this property of the elements. History of the Table for 300

    16. This principle states that the properties exhibited by elements repeat at regular intervals. History of the Table for 400

    17. Using his Table, Mendeleev was able to predict the properties of these substances, without having any prior knowledge about them. History of the Table for 500

    18. The general term that refers to the size of a neutral atom. Periodicity for 100

    19. The general term that refers to the size of a cation or an anion. Periodicity for 200

    20. The amount of energy required to remove an electron from an atom. Periodicity for 300

    21. The tendency for a bonded atom to attract electrons to itself. Periodicity for 400

    22. The tendency for the kernel electrons to block the valence electrons from the positive, attractive force of the nucleus. Periodicity for 500

    23. Within a group, this is the direction in which the atomic radius increases. Trends for 100

    24. Within a period, this is the direction in which the atomic radius increases. Trends for 200

    25. Within a group, this is the direction in which the shielding effect increases. Trends for 300

    26. Within a period, this is the direction in which ionization energy increases. Trends for 400

    27. Within a group, this is the direction in which the ionization energy increases. Trends for 500

    28. Across the entire Periodic Table, this is the direction in which electronegativity increases. Final Challenge

    29. Game Over “Luck is for the ill-prepared.” Alex Hess

    30. Double Score

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