 He was a German Chemist.  In 1810, he was eventually the professor at the University of Jena.  He discovered similar triads of elements in  In 1817, He discovered the group of elements. He found out that Lithium, Sodium and Potassium had similarity.

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 Triads are some of the first families of elements with similar chemical properties.  There were three in the group.  Their appearance and reactions of the elements were similar to each other. Alkali formers Li7 Na23 K39 Salt formers Cl35.5 Br80 I127

 He began working on the Periodic Table in the late 1860s.  He arranged 63 elements known by there atomic weight.  He also organized them into similar properties.  This is his first sketch of the Periodic Table. 

By: Morgan Williams & Brooke McKenna

 A period is a horizontal column on the periodic table of elements.  There are 7 periods on the periodic table.  And a group is a column that is vertical.  There and 18 groups on the periodic table.

 Groups are numbered in 2 ways, one way is 1-18 which includes all elements even the transition metals.  The second way is 1A-8A they’re known as the main groups.

 Lanthanides- inner transition elements with atomic numbers 58-71, lanthanides are located in the top row of the f block.  Actinides- inner transition elements with the atomic numbers from ; all are radioactive, actinides are located in the bottom row of the f block.  Transition elements- elements in groups 3-12 all are metals, transition elements are located in the D-block.

 Solids- definite shape and volume  Liquid- no definite shape, but definite volume  Gas- no definite shape or volume

 There are 2 liquids  There are 11 gases  Noble gases are generally located on the right side  The rest are solids

By: Mike Ross, Shelby Fausey, and Kaitlyn Carl Periodic Table

Definitions  Metal- Element that has luster, conducts heat and electricity and usually bends without breaking.  Non-metal- Does not conduct heat or electricity. Brittle when solid. Many are gases at room temperature.  Metalloid- Element with some physically & chemically properties of metals and other properties of non-metals.

Metal  Metals are located on the left side of the black outlined step looking line.  There are 61 metals on the periodic table.  Examples of metal are silver, copper, iron, and cobalt. They are used for machinery, coins, and automobiles.

Non-metals  Non-metals are located on the right side of the black line.  There are 18 non-metals on the periodic table  Sulfur, Chlorine, Iodine  most are gases, one is a liquid (Bromine) and the rest are solid.

Metalloids  Metalloids are located on the either side of the black line.  There are 7 metalloids on the periodic table.  Boron, Silicon, and Germanium are examples of metalloids  Metalloids are used mostly in transistors.

Group 1A  Group 1A is the Alkali Metals  Alkali Metals are soft and usually have low melting points and densities. They are also powerful reducing agents.  All react violently with water, and tarnish rapidly even in dry air. They are never uncombined in nature.  Alkali metals are sometimes used in explosives.

Group 2A  Group 2A elements are the Alkaline Earth Metals.  These metals are silvery colored, soft, and react readily with halogens. They then form ionic salts.  Magnesium and calcium are essential elements for all living organisms.

Transition Elements  These elements are in groups 3-12, all are metals.  Some transition elements are Scandium, Titanium, and Vanadium.  They are also known as transition metals. They are very hard and have high melting points and boiling points.  Transition elements are used for structural materials, copper pipes, and coins.

By: Mike Ross, Shelby Fausey, and Kaitlyn Carl Periodic Table

Definitions  Metal- Element that has luster, conducts heat and electricity and usually bends without breaking.  Non-metal- Does not conduct heat or electricity. Brittle when solid. Many are gases at room temperature.  Metalloid- Element with some physically & chemically properties of metals and other properties of non-metals.

Metal  Metals are located on the left side of the black outlined step looking line.  There are 61 metals on the periodic table.  Examples of metal are silver, copper, iron, and cobalt. They are used for machinery, coins, and automobiles.

Non-metals  Non-metals are located on the right side of the black line.  There are 18 non-metals on the periodic table  Sulfur, Chlorine, Iodine  most are gases, one is a liquid (Bromine) and the rest are solid.

Metalloids  Metalloids are located on the either side of the black line.  There are 7 metalloids on the periodic table.  Boron, Silicon, and Germanium are examples of metalloids  Metalloids are used mostly in transistors.

Group 1A  Group 1A is the Alkali Metals  Alkali Metals are soft and usually have low melting points and densities. They are also powerful reducing agents.  All react violently with water, and tarnish rapidly even in dry air. They are never uncombined in nature.  Alkali metals are sometimes used in explosives.

Group 2A  Group 2A elements are the Alkaline Earth Metals.  These metals are silvery colored, soft, and react readily with halogens. They then form ionic salts.  Magnesium and calcium are essential elements for all living organisms.

Transition Elements  These elements are in groups 3-12, all are metals.  Some transition elements are Scandium, Titanium, and Vanadium.  They are also known as transition metals. They are very hard and have high melting points and boiling points.  Transition elements are used for structural materials, copper pipes, and coins.

By Casey Higgins, Shanee Hay, Matthew Hayes

Reactivity  The tendency of a substance to undergo chemical reaction, either by itself or with other materials, and to release energy  Reactivity increases when you go down the group and decreases when you go left to right.

Density Mass per unit volume of a substance. D=mass/volume Density increases as you go down the group.

Atomic radius  The size of an atom.  Moving left to right Atomic radius Decreases and moving top to bottom atomic radius increases.

Ionized energy  Energy required to remove an electron from a specific atom.  moving left to right ionized energy increases and moving top to bottom ionized energy decreases.

Electronegativity  A chemical property that describes the ability of an atom to attract electrons towards itself in covalent bond.  Moving left to right electronegativity increases and moving top to bottom electronegativity decreases.