Unlocking the Periodic Table of Elements

Regular, repeating pattern

Unlocking the Periodic Table of Elements Dmitri Mendeleev (Russian Chemist) Credited with 1st Periodic Table Classified elements by: Name Atomic Mass Properties 1834 - 1907

Henry Moseley (British Physicist) Credited with Modern Periodic Table Used  atomic # instead of mass Classified and arranged by : Atomic # Arrangement of electrons in valence shell

Parts of the Periodic Table: Periods  7 Horizontal rows Elements 57 – 71 fit into period 6 Elements 89 – 103 fit into period 7 No similarities among the elements in a period Moves from Metals (left) to Nonmetals (right) Valence shells fill up as elements move from left to right

2 8 8

Groups  Vertical columns Elements have similar properties Due to same valence shell electron configuration Also known as “Families” Numbered 1 – 18 from left to right

Metalloids touch the zig-zag line on the right Nonmetal right of zig-zag line Metalloid Poor Metals Metals Large area left of the zig-zag line Metal

So … what exactly is a metal????? What makes something a metal???? What do you think of when you hear the word “metal”

Properties of metals Most are silver or grey Luster – reflects light when polished Conducts heat & electricity Usually high () melting point (MP) Malleable – can be flattened, bent & shaped without breaking e.g. aluminum foil Ductile – can be pulled into thin wire e.g. copper Exceptions: Pure gold and silver (soft metals) Gallium- MP just above room temp Mercury – liquid at room temp

They can give up or lose these electrons easily ***Remember, properties come from the electrons in the valence shell of the atoms*** Most metals have 1 to 3 electrons in their valence shell They can give up or lose these electrons easily They also hold their electrons loosely and can share them with other metal atoms (metallic bonds we will talk about later) Loose sharing of electrons gives rise to the properties of metals such as being malleable, conductive & ductile

Most gold or silver coins and jewelry are alloys. = + Brass (alloy) Zinc (metal) Copper (metal) Carbon (nonmetal) = + Steel (alloy) Iron (metal)

(Lithium, Sodium, Potassium, Ribidium, Cesium, Francium) Group 1 Alkali Metals 6 elements (Li, Na, K, Rb, Cs, Fr) (Lithium, Sodium, Potassium, Ribidium, Cesium, Francium) 1 valence electron (easily lost) Very reactive, combine easily  Exist in nature only as positive ions that will form ionic bonds with negative ions e.g. NaCl

(Beryllium, Magnesium, Calcium, Strontium, Barium, Radium) Group 2 Alkaline Earth Metals 6 elements (Be, Mg, Ca, Sr, Ba, Ra) (Beryllium, Magnesium, Calcium, Strontium, Barium, Radium) Reactive, but not as reactive as alkali metals 2 valence electrons Occur as ions, or combined with other elements e.g. Ca2+ or CaCl2

Transition Metals Shiny MP Good conductors Less reactive, but will combine with other elements Some magnetic (Iron, Cobalt, Nickel) Found in ores (minerals containing large amounts of metal compounds) (remember the alloys)

Rare Earth Metals 2 separate rows at the bottom of the periodic table Lanthanide Series (follows Lanthanum in period 6) *Except for # 61, all occur in nature in small amounts in the earth’s crust Actinide Series (follows Actinium in period 7) *Most synthetic Transuranium Elements – Atomic # > 92, synthetic, radioactive

Properties of Nonmetals Do not have luster Poor conductors of heat and electricity Usually dull and brittle Not malleable and not ductile Many are gases at room temperature The CHONSP elements are very important to life. Carbon is the backbone of macromolecules containing the other nonmetal elements that life depends on.

Group 13 the Boron Group Aluminum = poor metal 3 valence electrons Boron = metalloid Most abundant metal in Earth’s crust

Group 14 the Carbon Group Carbon= nonmetal Silicon = metalloid Germanium = poor metal 4 valence electrons

Group 15 the Nitrogen Group 5 valence electrons Nitrogen = 79% of air we breathe Phosphorus found in DNA, teeth, and bones

Group 16 the Oxygen Group 6 valence electrons Oxygen = Most abundant element in Earth’s crust Sulfur = Proteins, vulcanizing rubber Selenium = light meters, solar cells, photocopiers

Group 17 the Halogen Group Halogen = “salt former” Fluorine = most reactive 7 valence electrons, negative -1 anion Combine with alkali metals to form salt e.g. NaCl

Group 18 the Noble Gases Colorless gases Inert All found in Earth’s atmosphere Glow with color when electrical current passed through gas Neon lights

Hydrogen 1 valence electron Gas Properties of both metals and nonmetals

Sci Kap You CAN Science!

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