Unit 2 – The Periodic Table

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Presentation transcript:

Unit 2 – The Periodic Table

Development of the Periodic Table 1817 – Dobereiner Grouped elements in TRIADS… Three elements with similar properties

Development of the Periodic Table 1870 – Mendeleev Created an 8 Column table based on ATOMIC MASS Elements with similar properties were in the same column

Development of the Periodic Table Problems : Some elements did not fit the order. Tellurium (Te) and Iodine (I) There were gaps in the table Able to predict the properties and masses of the unknown elements very accurately.

Development of the Periodic Table 1913 – Moseley Arranged elements with increasing ATOMIC NUMBER PERIODIC LAW: Properties of the elements are a periodic function of their atomic number

Modern Periodic Table The table is arranged by valence electrons…. Definition: The electrons in the outermost level of the atom. Bohr Model: Level 1 = 2 electrons. Level 2 = 8 electrons. Level 3 = 18 electrons. Level 4 = 32 electrons.

Modern Periodic Table

Modern Periodic Table

Modern Periodic Table OCTET RULE… 8 electrons in the outer level = FULL VALENCE SHELL. Full Valence Shell = Unreactive = Very Stable. Atoms react with other atoms to make a situation where all atoms end up with FULL VALENCE SHELLS. They may add electrons. They may lose electrons. They may share electrons.

1. Gases or BRITTLE solids. Metals vs. Nonmetals METALS NONMETALS 1. Typically Solids. 1. Gases or BRITTLE solids. 2. Shiny. 2. Dull. 3. Conductor 3. Insulators LOSE electrons GAIN electrons

Metals vs. Nonmetals REMEMBER… Metals: 3 or less valence electrons. 5 or more valence electrons. Metalloids: Properties of both Metals and Nonmetals. Semiconductors.

Metals vs. Nonmetals