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2. What is the periodic table?
compact way of organizing elements
contains a lot of information
allows us to make predictions about behavior and properties of elements
Elements
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5. History of the Periodic Table
End of the 1700’s – less than 30 elements known
Many elements discovered during 1800’s
Many experiments done to determine atomic masses

7. John Newlands
1864: if elements arranged by atomic mass - properties repeat every 8th element
Law of Octaves
did not work for all known elements
Key idea was correct: Properties of elements do repeat in periodic way

8. Mendeleev & Meyer Mendeleev produced 1st accepted PT: 1869
Elements ordered by ↑ atomic mass into columns with similar properties
Predicted existence & properties of undiscovered elements
Not totally correct
more accurate atomic mass calculations showed some elements weren’t in right place

10. Remember 1860’s: No subatomic particles yet discovered
Dalton’s billiard ball model of the atom

11. 1913 – Henry Moseley by 1913, protons & electrons discovered
Neutrons were predicted
Moseley determined atoms of each element contain unique # protons (= atomic number)
rearranged Mendeleev’s PT by atomic number instead of mass
problems with elements in wrong place disappeared

12. Periodic Law
There is a periodic repetition of chemical and physical properties of elements when arranged by increasing atomic number

13. Glenn Seaborg: 1950’s
Lanthanide and Actinide Series

16. Newlands
Seaborg
Mendeleev
Mosley

17. Vocabulary of PT Columns called groups or families
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Columns called groups or families
Today: #1 thru 18, Arabic numerals
Past: A & B groups, Roman numerals
A-Group
Columns 1,2,13-18 (= representative elements)
IA – 8A
B-Group
Transition metals (columns 3-12)
IB - 8B
Rows are called series or periods
#1 thru 7

18. Column numbering (1  18) left to right
Period numbering (1  7) top to bottom

19. Structure of Periodic Table
Closely related to electron configuration of each element
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20. Energy Levels = Row Number
Elements in same row have same # of principal energy levels
so # of principal energy levels = to row #
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21. Going Across Row 2: 2-8 Ne 18 (VIIIA) 2-7 F 17 (VIIA) 2-6 O 16 (VIA)
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2-8 Ne
18 (VIIIA)
2-7 F
17 (VIIA)
2-6 O
16 (VIA)
2-5 N
15 (VA)
2-4 C
14 (IVA)
2-3 B
13 (IIIA)
2-2 Be
2 (IIA)
2-1 Li
1 (IA)
Configuration
Element
Family

22. Going Down Column 1: 2-8-18-32-18-8-1 Fr 7 2-8-18-18-8-1 Cs 6
COPY Fr 7 Cs 6 Rb 5 K 4
2-8-1 Na 3
2-1 Li 2 1 H
Configuration
Element
Period

23. Number of Valence Electrons
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14 or IVA 3
13 or IIIA 2
2 or IIA 1
1 or IA
Number of Valence Electrons
Group

24. Valence Electrons Chemical behavior determined by # valence electrons
Elements with same # valence electrons will have similar chemical properties
Elements in same column have similar chemical properties
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25. Classifying the Elements
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2/3 (75%) of elements are metals
Remaining elements: non-metals & metalloids (semi-metals)
Metalloids:
some properties of metals & some properties of nonmetals
Staircase:
dividing line between metals & nonmetals
elements to left are metals (except H)
elements to right are non-metals

26. Properties of Metals Malleable – flattened into sheets
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Malleable – flattened into sheets
Ductile – drawn into wires & tubes
have Luster
Good Conductors of heat & electricity
Solid at room temperature (except Hg)
Metals lose electrons & form positive ions “Metals are losers”
Low ionization energy
Low electronegativity

27. Properties of Nonmetals
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generally gases or solids (except Br2)
solids are Brittle
solids are Dull
poor conductors of heat & electricity
Nonmetals gain electrons & form negative ions
“Nonmetals are winners”
High ionization energy
High electronegativity
Properties: OPPOSITE of metals

28. Properties of Metalloids
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7 metalloids:
5 on right of staircase: B,Si,As,Te,At
2 on left of staircase: Ge,Sb
Each metalloid has some metallic and some nonmetallic properties
Example:Si
shiny like metal but brittle like nonmetal

29. Names of Families (AKA group A elements)
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Group 1 = Alkali Metals
Group 2 = Alkaline Earth Metals
Groups 3-12: Transition metals
Group 13 = Boron family
Group 14 = Carbon family
Group 15 = Nitrogen family
Group 16 = Oxygen family
Group 17 = Halogens
Group 18 = Noble Gases

30. Transition Metals Groups 3 through 12 AKA group B elements
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Groups 3 through 12
AKA group B elements
Actinide & Lanthanide series
inner transition elements
put the COLOR in your life
form brightly colored salts/solutions

31. Elements that are gases at STP
Diatomics:
H2, N2, O2, F2, Cl2
Monatomics: noble gases
He, Ne, Ar, Kr, Xe, Rn
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32. Two Elements: liquid at room temperature
Br2 (non-metal) and Hg (metal)
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33. All other elements are solids at room temperature