periodic table
DESCRIPTION
Periodic Table. Mendeleev. Dmitri Mendeleev (1869, Russian) Organized elements by increasing atomic mass . Elements with similar properties were grouped together. There were some discrepancies. Mendeleev. Dmitri Mendeleev (1869, Russian) - PowerPoint PPT PresentationTRANSCRIPT
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Periodic Table
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Mendeleev• Dmitri Mendeleev (1869, Russian)– Organized elements
by increasing atomic mass.
– Elements with similar properties were grouped together.
– There were some discrepancies.
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Mendeleev• Dmitri Mendeleev (1869, Russian)– Predicted properties of undiscovered
elements.
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Moseley
• Henry Mosely (1913, British)
– Organized elements by increasing atomic number.
– Resolved discrepancies in Mendeleev’s arrangement.
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Mendeleev’s Periodic Table
Dmitri Mendeleev
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Modern Russian Table
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Stowe Periodic TableStowe Periodic Table
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A Spiral Periodic TableA Spiral Periodic Table
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“Mayan” Periodic
Table
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The Periodic Table
Period
Group or family
Period
Group or Family
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• Horizontal rows are called Periods or Series There are 7 periods
6
3
4
5
1
7
2
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• Vertical columns are called Groups.• Elements are placed in columns by similar
properties.• Also called families
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• Main Group Elements• Transition Metals• Inner Transition
Metals
Blocks
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1A
2A 3A 4A 5A 6A 7A
8A• The elements in the A groups are called the representative elements
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The group B are called the transition elements
These are called the inner transition elements and they belong here
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• Group 1A are the alkali metals• Group 2A are the alkaline earth metals
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• Group 7A is called the Halogens• Group 8A are the noble gases
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• Metals• Nonmetals• Metalloids
Metallic Character
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Easily lose valence electron (Reducing agents)
React violently with water Large hydration energy React with halogens to form
salts
The Properties of a Group: Alkali Metals
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Examples of Metals
Potassium, K reacts with water and must be stored in kerosene
Zinc, Zn, is more stable than potassium
Copper, Cu, is a relatively soft metal, and a very good electrical conductor.
Mercury, Hg, is the only metal that exists as a liquid at room temperature
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Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.
Nonmetals are poor conductors of heat and Electricity
Nonmetals tend to be brittle
Many nonmetals are gases at room temperature
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Examples of Nonmetals
Sulfur, S, was once known as “brimstone”
Microspheres of phosphorus, P, a reactive nonmetal
Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure
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Properties of Metalloids
Metalloids straddle the border between metals and nonmetals on the periodic table.
They have properties of both metals and nonmetals.
Metalloids are more brittle than metals, less brittle than most nonmetallic solids Metalloids are semiconductors of electricity Some metalloids possess metallic luster
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Silicon, Si – A Metalloid Silicon has metallic luster Silicon is brittle like a nonmetal Silicon is a semiconductor of electricity
Other metalloids include:
Boron, B Germanium, Ge Arsenic, As Antimony, Sb Tellurium, Te
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Periodicity Explained
• Valence = Outer shell electrons• The orbitals fill up in a regular
pattern• The outer shell electron
configuration repeats• The properties of atoms therefore
repeat when placed in order of Atomic Number
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1s1
1s22s1
1s22s22p63s1
1s22s22p63s23p64s1
1s22s22p63s23p64s23d104p65s1
1s22s22p63s23p64s23d104p6 5s24d10 5p66s1
1s22s22p63s23p64s23d104p65s24d105p6 6s24f145d106p67s1
H1
Li3
Na11
K19
Rb37
Cs55
Fr87
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He2
Ne10
Ar18
Kr36
Xe54
Rn86
1s22s22p63s23p64s23d104p6
1s22s22p63s23p64s23d104p65s24d105p6
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p6
1s2
1s22s22p6
1s22s22p63s23p6
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• Alkali metals all end in s1
• Alkaline earth metals all end in s2
• really have to include He but it fits better later.
• He has the properties of the noble gases.
s2s1 s- block
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Transition Metals - d block
d1 d2 d3 d4 d5 d6 d7 d8 d9 d10
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The p-block p1 p2 p3 p4 p5 p6
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f - block
• inner transition elements
f1 f5f2 f3 f4
f6 f7 f8 f9 f10 f11 f12 f14
f13
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Writing Electron configurations the easy
way
Yes there is a shorthandYes there is a shorthand
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Electron Configurations repeat
• The shape of the periodic table is a representation of this repetition.
• When we get to the end of the column the outermost energy level is full.
• This is the basis for our shorthand.
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The Shorthand• Write the symbol of the noble gas
before the element.• Then the rest of the electrons.• Aluminum - full configuration.
• 1s22s22p63s23p1
• Ne is 1s22s22p6
• so Al is [Ne] 3s23p1
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More examples• Ge = 1s22s22p63s23p64s23d104p2
• Ge = [Ar] 4s23d104p2
• Hf = 1s22s22p63s23p64s23d104p65s2
4d105p66s24f145d2
• Hf=[Xe] 6s24f145d2
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The Shorthand Again
Sn- 50 electrons
The noble gas before it is Kr
[ Kr ]
Takes care of 36
Next 5s2
5s2
Then 4d10
4d10Finally 5p2
5p2