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Periodic TableLarry Scheffler
Lincoln High SchoolIB Chemistry 1-2
.1
Periodic Table
.2
3.1 The periodic table
3.1.1 Describe the arrangement of elements in the periodic table in order of increasing atomic number.
3.1.2 Distinguish between the terms group and period.
3.1.3 Apply the relationship between the electron arrangement of elements and their position in the periodic table up to Z = 20. 3.1.4 Apply the relationship between the number of electrons in the highest occupied energy level for an element and its position in the periodic table.
The Periodic Table-Key Questions• What is the periodic table ?• What information does the table provide ?• How can one use the periodic table to predict the
properties of the elements?
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Periodic Table• The development of the periodic table brought a
system of order to what was otherwise an collection of thousands of pieces of information.
• The periodic table is a milestone in the development of modern chemistry. It not only brought order to the elements but it also enabled scientists.
to predict the existence of elements that had not yet been discovered .
.4
Early Attempts to Classify Elements
• Dobreiner’s Triads (1827)• Classified elements in sets of three having
similar properties.• Found that the properties of the middle
element were approximately an average of the other two elements in the triad.
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Dobreiner’s Triads
Element Atomic Mass(amu)
Average Density(g cm-3)
Average
ClBrI
35.579.9126.9
81.21.563.124.95
3.25
CaSrBa
40.187.6137.3
88.71.552.63.5
2.53
Note: In each case, the numerical values for the atomic mass and density of the middle element are close to the averages of the other two elements
.6
Newland’s Octaves -1863• John Newland attempted to classify
the then 62 known elements of his day.
• He observed that when classified according to atomic mass, similar properties appeared to repeat for about every eighth element
• His Attempt to correlate the properties of elements with musical scales subjected him to ridicule.
• In the end his work was acknowledged and he was vindicated with the award of the Davy Medal in 1887 for his work.
.7
Dmitri Mendeleev Dmitri Mendeleev is
credited with creating the modern periodic table of the elements.
He gets the credit because he not only arranged the atoms, but he also made predictions based on his arrangements His predictions were later shown to be quite accurate.
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Mendeleev’s Periodic Table
• Mendeleev organized all of the elements into one comprehensive table.
• Elements were arranged in order of increasing mass.
• Elements with similar properties were placed in the same row.
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Mendeleev’s Periodic Table
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Mendeleev’s Periodic Table
Mendeleev left some blank spaces in his periodic table. At the time the elements gallium and germanium were not known. He predicted their discovery and estimated their properties. .11
Mendeleev’s Periodic TableHere is what he predicted and estimated properties of Germanium along with the actual data.
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The Modern Periodic Table
The Periodic Table has undergone several modifications before it evolved in its present form. The current form is usually attributed to Glenn Seaborg in 1945
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Periodic Table Expanded View•The Periodic Table can be arranged by energy sub levels
•The s-block is Group IA and & IIA,
•the p-block is Group IIIA - VIIIA
•The d-block is the transition metals,
•and the f-block are the Lanthanides and Actinide metals
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Periodic Table Expanded View
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The way the periodic table usually shown is a compressed view. The Lanthanides and actinides (F block) are cut out and placed at the bottom of the table.
The Periodic tableAlkali Metals
Alkaline Earths
Transition Metals
Halogens
Noble Gases
Lanthanides and Actinides
Periodic Table: Metallic Arrangement
1IA
18VIIIA
12IIA
13IIIA
14IVA
15VA
16VIA
17VIIA
2
33
IIIB4IVB
5VB
6VIB
7VIIB
8 9VIIIB
10 11IB
12IIB
4
5
6
7
Metals
Nonmetals
• Layout of the Periodic Table: Metals vs. nonmetals.
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The Three Broad Classes are the Representative, Transition, & Rare Earth
• Main (Representative), • Transition metals, • lanthanides and actinides (rare earth)
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Additional Groupings in the Periodic Table
• Nonmetals, Metals, Metalloids, Noble gases
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Periodic Table: The electron configurations are inherent in the periodic table
•B•2p1
1IA
18VIIIA
12IIA
13IIIA
14IVA
15VA
16VIA
17VIIA
2
33
IIIB4IVB
5VB
6VIB
7VIIB
8 9VIIIB
10 11IB
12IIB
4
5
6
7
H1s1
Li2s1
Na3s1
K4s1
Rb5s1
Cs6s1
Fr7s1
Be2s2
Mg3s2
Ca4s2
Sr5s2
Ba6s2
Ra7s2
Sc3d1
Ti3d2
V3d3
Cr4s13d5
Mn3d5
Fe3d6
Co3d7
Ni3d8
Zn3d10
Cu4s13d10
B2p1
C2p2
N2p3
O2p4
F2p5
Ne2p6
He1s2
Al3p1
Ga4p1
In5p1
Tl6p1
Si3p2
Ge4p2
Sn5p2
Pb6p2
P3p3
As4p3
Sb5p3
Bi6p3
S3p4
Se4p4
Te5p4
Po6p4
Cl3p5
Be4p5
I5p5
At6p5
Ar3p6
Kr4p6
Xe5p6
Rn6p6
Y4d1
La5d1
Ac6d1
Cd4d10
Hg5d10
Ag5s14d10
Au6s15d10
Zr4d2
Hf5d2
Rf6d2
Nb4d3
Ta5d3
Db6d3
Mo5s14d5
W6s15d5
Sg7s16d5
Tc4d5
Re5d5
Bh6d5
Ru4d6
Os5d6
Hs6d6
Rh4d7
Ir5d7
Mt6d7
Ni4d8
Ni5d8
.20
Periodic Table Organization------ Groups or Families
Vertical columns in the periodic table are known as groups or families The elements in a group have similar electron configurations
.21
Periodic Table Organization ---- Periods
Horizontal Rows in the periodic table are known as Periods The Elements in a period undergo a gradual change in properties as one proceeds from left to right
.22