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| German Chemist. In 1817 discovered Law of Triads |
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| Groups of 3 Related Elements have similar properties |
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| English Chemist. In 1863 discovered the Law of Octaves |
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| The same properties appear every 8th element when elements are listed in order of their atomic masses. |
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| Russian Chemist. During 1860's developed the 1st periodic table. Suggested periods of varying lengths based on atomic masses. Predicted Properties of yet undiscovered elements (Gallium, Germanium, Scandium) |
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| Properties of elements are periodic functions of their atomic masses. |
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| Properties of elements are functions of their atomic numbers. (Developed by Henry Moseley) |
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| British Scientist. In 1913 he developed the Modern Periodic Law. |
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| The number of protons in an atom. In a neutral atom this refers to the number of electrons. |
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| Vertical Columns of elements. AKA Family |
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| Horizontal Rows of elements. AKA series |
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| Alkali Metal, Alkaline Earth Metals, Lanthanoids, Actinoids, Transition Metals, Chalcogens, Halogens, Noble Gases |
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| An atom with 8 electrons in its outer shell is particularly stable. (an atom will try to have 8 electrons in its outer shell) |
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S - Helium and First 2 Columns in Periodic Table
P - Last 6 Columns (minus Helium)
D - Transition Metals (middle area) (n-1 for easy electron configuration)
F - Lower 2 rows. (n-2 for easy electron configuration) |
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| Shiny, Malleable, Ductile, Conduct heat & electricity, Have few electrons in outer shell, lose electrons in chemical reactions |
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| Dull, Brittle, Non-Ductile, Insulator of heat & electricity, Have many electrons in outer shell, gain electrons during chemical reactions |
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| Elements adjacent to bold diagonal line. |
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| Factors in Ionization Energy |
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Definition
Greater Nuclear Charge (direct relationship)
Greater Principle Quantum # (Inverse Relationship)
Greater Shielding effect (Inverse Relationship)
Half/Completely filled sublevels (No Relationship) |
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| Towards upper right corner, half filled or full shells |
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| Towards bottom left corner, more electrons than protons |
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| Closer to upper right corner, more electrons gained in reaction |
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| Increases from left -> Right. Increases from top -> Bottom. Noble gases have no electronegativity. Fluorine has highest electronegativity. Francium has the lowest. |
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| Higher in middle of table. Lower on the ends |
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| Higher in the middle of the table. Lower on the edges. |
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