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2 Who developed the Periodic Table? Dimitri Mendeleev – (Russian Chemist) developed the first Periodic Table with 63 elements that was known at the time. He found that as the atomic mass increased, a repeating patterns of properties developed.

3 Rearranging Table Henry Moseley- English scientist In 1913 he rearranged the periodic table by the atomic number and chemical properties. This is the periodic table we use today

4 and COLUMNS called GROUPS or FAMILIES. Mendeleev arranged these elements into ROWS called PERIODS… Arrangement of the Periodic Table

5 You can think about it like this… You have to use a PERIOD at the end of a sentence……..that goes left to right. And a COLUMN hold up the porch on the house where your GROUP / FAMILY lives.

6 Periods represent the number of outer rings. Energy Level 2: Li, Be, B, C, N, O, F & Ne Locate them on your periodic table These outer rings are also called Valence Shell or Energy Levels. 2 nd Row = 2 Rings electron

This is period number 3 Which means it has 3 energy levels This is period number 3 Which means it has 3 energy levels Period #’s run down the side of the Periodic Table.

8 The Group Numbers run on top Of the Periodic Table This is group 1 the alkali group. Families have similar but not identical characteristics 1 IA 2 IIA 18 VIIIA 17 VIIA 15 VA 16 VIA 14 IVA 13 IIIA

9 Metals Non-Metals Transition Metals Inner Transition Metals Metalloids

10 Properties of Metals Good conductors of heat and electricity Malleable, Ductile Have Luster High melting & boiling points High density Mostly solids – except for Hg (liquid) Fr Left of the STAIRS

11 Properties of Nonmetals Poor conductors of heat and electricity Dull, Brittle Low melting and boiling points Most are GASES, some SOLIDS, and only 1 Liquid - Bromine Right of the STAIRS F

12 Properties of Metalloids Conduct heat and electricity… not as well as TRUE metals Shiny or dull Have other properties of metals and nonmetals Touch the STAIRS

13 Characteristics  Groups 3 through 12 or IIIB to IIB  Has 1 or 2 valence electrons  Located between Metals & Non-metals  From Left to Right – they lose properties of Metals and gain properties of Non-Metals  Iron, copper, and silver are examples  Less active than alkali metals and alkaline earth metals  Many gemstones contain transition metal

14 Characteristics  Group IA or 1  Has 1 Valence electron  Highly reactive  Li, Na, K, Rb, Cs, Fr  Make salts such as NaCl and KCl  Lithium - Treatment for bi-polar disorder

15 Characteristics  Group IIA or 2  Has 2 Valence electrons  Not found readily in nature  Found in gemstones and fireworks  Magnesium burns brightly.  Strong and light material used to make cars, planes, and baseball bats  Calcium makes bones strong.

16 Characteristics  Group VIIA or 17  Has 7 Valence electrons  Highly reactive group of Non-Metals  Chlorine is the most abundant  Chlorine bleaches are used in disinfecting water.  Bromine used are as dyes in cosmetics  Iodine (shiny gray) is essential in the production of thyroxin.

17 Characteristics  Group VIIIA or 18  Have 2 or 8 Valence electrons  Most Stable Group of Elements, He, Ne, Ar, Kr, Xe, Rn  Noble gases normally don’t mix with other compounds  Uses: Neon lights, laser lights...

18  Has 1 Valence Electron  Most abundant element  Put with Metals because it acts more like a Metal than a Non-Metal  Has properties of both Alkali Metals & Halogens  Used in everything from water to acids and bases. Characteristics

19 Inner Transition Elements Lanthanide seriesLanthanide series Actinide Series All are radioactive Most are synthetic