Concept:

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 History of Periodic Table
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Mendeleev (1869) arranged elements based on atomic mass
Anton van den Broek proposed that elements should be arranged to nuclear charge instead of atomic mass
Moseley confirmed these findings with x-ray spectra and arranged them by atomic number.
Therefore, atomic number will increase from left to right.

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H - Hydrogen
Li - Lithium
Na - Sodium
K - Potassium
Be -Beryllium
Mg - Magnesium
Ca - Calcium
Ba – Barium
Fe - Iron
Ni – Nickel
Pt - Platinum
Cu - Copper
Ag -Silver
Au – Gold
Zn - Zinc
Hg - Mercury
B - Boron
Al – Aluminum
C - Carbon
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Si - Silicon
Ge – Germanium
Sn - Tin
Pb - Lead
N - Nitrogen
P - Phosphorus
As -Arsenic
Sb - Antimony
Bi – Bismuth
O - Oxygen
S - Sulfur
Se - Selenium
F - Fluorine
Cl - Chlorine
Br - Bromine
I - Iodine
He - Helium
Ar - Argon
Kr –Krypton
Ne – Neon

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(blue area; groups 1-12 except H, and under stair-step line groups 13-15)
Good conductors of heat and electricity
Solid at room temperature (except for Hg)
Reflects light (luster)
Malleable (hammered into sheets)
Ductile (stretched/drawn into wire)

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Alkali Metals
Group 1 (one valence electron)
Softer than most other metals
Silvery/shiny
Most reactive of all metals (reacts rapidly with oxygen and water)
Do not occur in nature in elemental form
Stored (kerosene)
Fr - radioactive

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Alkaline Earth Metals
Group 2 (2 valence electrons)
Not found as free elements in nature
Gives fireworks color, bright red lights, aircraft

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Groups 3-12 (elements in transformation)
Form colored compounds
Often occur in nature as uncombined elements
“Iron Triad” (Fe, Co, Ni – 8, 9, 10)
 Used to make steel and other metal mixtures
“Coinage Metals” (Cu, Ag, Au – 11)
 Stable, malleable, found in nature as free elements

 Zn, Cd, Hg (group 12)
 Used to coat other metals
 Cd – rechargeable batteries
 Hg – liquid thermometers

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ALL are radioactive and unstable
Lanthanides (Atomic Number 58-71)
Actinides (Atomic Number 90-103)

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Gases or brittle solids at room temperature
Can form ionic or covalent bonds
Not malleable
Not ductile
Most do not conduct heat or electricity
Generally not shiny
All, except H, are found on right of periodic table (in yellow)

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Group 17 “ Halogens ”
Most reactive non-metal
7 electrons in outer nrg level, one needed to make it complete
Gains an electron from metal  forms a salt
In gaseous state form reactive diatomic covalent molecules (identified by distinctive colors)
F – most chemically active of all elements
Cl – most abundant halogen
Br – only nonmetal that is liquid at room temp

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Group 18 “ Noble gases ”
Full outer energy level “happy” so they exist as isolate atoms
Stable & Relatively unreactive

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Elements along stair-step line (except for Al)
Can form ionic and covalent bonds with other elements metallic and nonmetallic properties
Semiconductors

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Mixed groups
Group 13 – Boron Group (Al most abundant metal)
Group 14 – Carbon group
Group 15 – Nitrogen Group
Group 16 – Oxygen Group

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Synthetic Elements
Elements not typically found on Earth
Made in a lab
With exception to Technetium 43 and
Promethium 61, each synthetic element has more than 92 protons

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Plutonium (94) used in bombs and control rods of nuclear reactors
Americium – smoke detectors
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Transuranium Elements – elements with 92+
Synthetic and unstable; disintegrate quickly
Not considered metals, nonmetals, or metalloids

 Period
 Horizontal rows (across)
 Use to tell energy level
 Group
 Vertical columns (down)
 Elements within a group have similar properties due to valence electrons
 Use to tell valence electrons
 Valence electrons
 the electrons in the outer most energy level that are available to chemically react
 Correlates to the group number for main group elements

 Energy levels (nrg)
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1-7 Correlate to periods (rows) on table
1 st nrg level can only hold 2 e. 8 e are needed for each nrg level to make that level complete and stable. Nrg levels closest to nucleus have lower nrg
Level 1 up to 2 e
Level 2 up to 8 e
Level 3 up to 18 e
Level 4 up to 32 e

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Valence electrons for main group elements
Group 1 – 1; give up 1
Group 2 – 2; give up 2
Group 13 – 3; give up 3
Group 14 - 4
Group 15 – 5; gain 3
Group 16 – 6; gain 2
Group 17 – 7; gain 1
Group 18 – 8; gain 0

 Electron cloud structure
 Lewis Dot structure