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Periodic Table Family Album

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Periodic Table Family Album - Page Text Content

FC: The Periodic Table Family Photo Album | By: Armanni Adamson Date: October 26, 2011 Period: 2nd Teacher: Mrs Smith-Brown Class: Chemistry

1: Table Of Contents The founding fathers The element families Subatomic Particles Periodic Table Trends

2: The Founding Fathers | Antonie Lavoisier (1743-1749) He made a list of all the elements that were known at that time. He categorized them into four groups. The four groups were gases, metals, nonmetals, and earths. | John Newlands (1837-1898) He put the elements in order by increasing atomic number. He also noticed a pattern in every eighth element that the properties were alike. He also created the law of octaves.

3: Lothar Meyer (1830-1895) He showed a connection between atomic mass and element properties. He also arranged the elements by increasing atomic mass just like Lavoisier. | Dmitri Mendeleev (1834-1907) He organized the elements in the periodic table by increasing atomic mass. He also predicted elements that were undiscovered with their atomic mass and left blank spaces on the periodic table for them. | Henry Moseley (1887-1915) He discovered the atomic number of a element, which is the number of protons in an element. He put the elements in order by increasing atomic number.

4: The Famalies Of the Periodic Table

6: The S Orbital | Alkali Metals | Hydrogen | Uses: ~*Batteries Dietary Salt Sodium Pump Potassium Pump Cesium Atomic Clocks | Chemical Properties: corrosive flammable\ decomposes burning tarnishes

7: Alkaline Earth Metals | Uses: Space Telescopes Precious Gems Crop Fields Fireworks New Engine Alloys | Physical Properties:\ silvery low melting points densities increases soft strong

8: The D Orbital | Transitional Metals

9: Uses: Steel Strategic Materials Iron core Copper Microchips Paint Pigments | Chemical Properties: acidity tarnish oxidize Heat combustion reactivity | Physical Properties: reflect light paramagnetic high densities high melting points malleable

10: The P Orbital | Boron Group | Uses: Detergent CDs and DVDs HD DVDS\ Flat Screen TVs Cardiac Scans | Chemical Properties: acidity reactivity oxidation toxicity tarnishes

11: Carbon Group | Uses: Graphite Golf Shafts Diamond Cutting Nano-tubes Computer chips Glass | Physical Properties: metalloid silvery-white ductile malleable soft

12: The P Orbital | Nitrogen group | Uses: fixing Bacteria Cryotherapy Safety Matches Flame Retardants Soothing Upset Stomaches | Chemical Properties: acidity reactivity oxidation toxicity tarnishes

13: Oxygen group | Uses: Photosynthesis Water the dual nature of ozone Economic indicator Photocopies | Physical Properties: colorless odorless brittle white shiny

14: The P Orbital | Halogen group | Uses: fluoridation BleachHalogen Lights Iodine deficiency with salt | Chemical Properties: acidity reactivity oxidation toxicity tarnishes

15: Noble Gases | Uses: the Sn lighting medicine ease breathing a natural radioactive gas | Physical Properties: gases liquids solids nonmetals colorless

16: The F Orbital | Lanthanide series | Uses: flint Auer metal oil refining industry streetlights search lights | Chemical Properties: radio active toxicity decomposition oxidation reactivity

17: Actinide series | Uses: bombs nuclear weapons nuclear reactors ionization chambers smoke detectors | Physical Properties: paramagnetic reflects light high density high melting points metals

18: Subatomic Particles | Protons: 17 Neutrons: 35-17=18 Electrons: 17 Quarks: 34

19: Lewis Model | Bohr Model | The lewis dot diagram only draws the valence electrons. | The Bohr model shows all the electrons in the element.

20: Orbital Notation

21: Orbital Notation shows you how many electrons are in an orbital for a given element.

22: Periodic Table | Groups | Periods

23: Atomic Number | Element Name Symbol | Atomic Mass | The Periodic table is arranged by increasing atomic mass. Elements in groups have similar properties.

24: Trends Of the Periodic Table

25: Ionization is the energy that is needed to take electrons from gaseous atoms. It increases when going from left to right and decreases when going down.

26: Atomic Radius is the measure of the size of an atom. The size increases going from right to left and it also increases going down a period.

27: Electronegativity show if a element's atom can be chemically bonded to attract electrons. The possibility of it attracting increases from left to right and going up a group.

28: Bibliograph Los Alamos National Laboratory (2001) Crescent Chemical Company (2001) Lange's Handbook of Chemistry (1952) CRC Handbook of Chemistry & Physics (18th Ed.)

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  • By: Armanni A.
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