Matter UnitPeriodic Table Notes
The Periodic TableThe Periodic Table
Dmitri Mendeleev (1834 - 1907)Dmitri Mendeleev (1834 - 1907)
P
Zn As
Sb
Pt Bi
Midd. -1700
Cr Mn
Li
K
N O F
Na
BBe
H
Al Si Cl
Ca Ti V Co Ni Se Br
Sr Y Zr Nb Mo Rh Pd Cd Te I
Ba Ta W Os Ir
Mg
Ce Tb Er
Th U
1735-1843
Discovering the Periodic Table
C
S
Fe Cu
Ag Sn
Au Hg Pb
Ancient Times
He
Sc Ga Ge
Rb Ru In
Cs Tl
Pr Nd Sm Gd Dy Ho Tm Yb
La
1843-1886 Ne
Ar
Kr
Xe
Po Rn
Ra
Eu Lu
Pa
Ac
1894-1918
Tc
Hf Re At
Fr
Pm
Np Pu Am Cm Bk Cf Es Fm Md No Lr
1923-1961
Rf Db Sg Bh Hs Mt
1965-
Journal of Chemical Education, Sept. 1989
Elements are arranged:
Vertically into Groups
Horizontally Into Periods
Why?
If you looked at one atom of every element in a group you would
see…
Each atom of a group has the same number of electrons in its outermost
shell.
• An example…
Valence electrons are the electrons in the outermost energy level.The number of “valence” electrons in an atom
affects the way an atom bonds. The way an atom bonds determines many
properties of the element.This is why elements within a group usually
have similar properties.
The group 2 atoms all have 2 electrons in their outer shells
Be (Beryllium)
Atom
Mg (Magnesium) Atom
If you looked at an atom from each element in a period
you would see…
Each atom of the period has the same number of
electron shells or energy levels.
An example…
The period 4 atoms each have 4 electron containing shells
K (Potassium)
AtomFe (Iron) Atom
Kr (Krypton)
Atom
4th Shell
Each group has distinct properties
• The periodic Table is divided into several groups based on the properties of different atoms.
Alkali Metals
•Soft, silvery colored metals
•Very reactive!!!
Group 1A: Alkali MetalsGroup 1A: Alkali MetalsGroup 1A: Alkali MetalsGroup 1A: Alkali Metals
Cutting sodium metalCutting sodium metal
Reaction of potassium + H2O
http://www.youtube.com/watch?v=m55kgyApYrY&safety_mode=true&persist_safety_mode=1&safe=active
Alkali Metals reacting with water:
• Li (Lithium) – least reactive
• Na (Sodium)
• K (Potassium)
• Rb (Rubidium)• Cs (Cesium) – more reactive
What would you expect from Francium?!?!
MagnesiumMagnesium
Magnesium Magnesium oxideoxide
Group 2A: Alkaline Earth MetalsGroup 2A: Alkaline Earth Metals
Alkaline Earth Metals
• Silvery-White Metals
• Fairly reactive
• Many are found in rocks in the earth’s crust
Transition Metals
• Malleable (easily bent/hammered into wires or sheets)
• Most are good conductors of electricity
How many things can you think of that have Transition Metals in
them?
Metalloids
Lie on either side of the “staircase”
• They share properties with both metals and non-metals
• Si (Silicon) and Ge (Germanium) are very important “semi-conductors”
Metals and Nonmetals
Li
3
He
2
C
6
N
7
O
8
F
9
Ne
10
Na
11
B
5
Be
4
H
1
Al
13
Si
14
P
15
S
16
Cl
17
Ar
18
K
19
Ca
20
Sc
21
Ti
22
V
23
Cr
24
Mn
25
Fe
26
Co
27
Ni
28
Cu
29
Zn
30
Ga
31
Ge
32
As
33
Se
34
Br
35
Kr
36
Rb
37
Sr
38
Y
39
Zr
40
Nb
41
Mo
42
Tc
43
Ru
44
Rh
45
Pd
46
Ag
47
Cd
48
In
49
Sn
50
Sb
51
Te
52
I
53
Xe
54
Cs
55
Ba
56
Hf
72
Ta
73
W
74
Re
75
Os
76
Ir
77
Pt
78
Au
79
Hg
80
Tl
81
Pb
82
Bi
83
Po
84
At
85
Rn
86
Fr
87
Ra
88
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
Ce
58
Pr
59
Nd
60
Pm
61
Sm
62
Eu
63
Gd
64
Tb
65
Dy
66
Ho
67
Er
68
Tm
69
Yb
70
Lu
71
Th
90
Pa
91
U
92
Np
93
Pu
94
Am
95
Cm
96
Bk
97
Cf
98
Es
99
Fm
100
Md
101
No
102
Lr
103
La
57
Ac
89
1
2
3
4
5
6
7
METALS
Nonmetals
Metalloids
What are semiconductors used in?
Nonmetals
• Brittle
• Do not conduct electricity
• Nonmetals
• Most are poisonous
• Fairly reactive – react with alkali metals (eg) Na+ and Cl-
Halogens
Chlorine Gas was used as a chemical weapon during World War I.
It was used by the Germans in World War II.
Chlorine Gas• The Germans were the first to use Chlorine gas
at Ypres in 1915• Chlorine gas is a lung irritant• The symptoms of gas poisoning are bright red
lips, and a blue face• People affected die a slow death by suffocation• Decades later men who thought they had
survived the war died from lung diseases such as Emphysema
CHLORINE
• Nonmetals
• Unreactive
• Gases at room temperature
Noble Gases
Jellyfish lamps made with noble gases artist- Eric Ehlenberger
Colors Noble Gases produce in lamp tubes:
• Ne (Neon): orange-red
• Ar (Argon): pale lavender
• He (Helium): pale peach
• Kr (Krypton): pale silver
• Xe (Xenon): pale, deep blue
Lanthanide SeriesActinide Series
• The lanthanide series can be found naturally on Earth.
• Only one element in the series is radioactive.
• Also called rare-earth metals or inner-transition elements.
• You might find some of these elements in superconductors, glass production, or lasers
• The actinide series is much different.
• They are all radioactive • Some are not found in
nature. • Some of the elements with
higher atomic numbers have only been made in labs.
ELEMENTS THAT EXIST AS ELEMENTS THAT EXIST AS DIATOMICDIATOMIC MOLECULESMOLECULES
ELEMENTS THAT EXIST AS ELEMENTS THAT EXIST AS DIATOMICDIATOMIC MOLECULESMOLECULES
Remember:
The “GENS”These elements exist as PAIRS when ALONE.
Hydrogen (H2)
Nitrogen (N2)
Oxygen (O2)
Halogens
(F2, Cl2, Br2, I2)
(P4 and S8)
Diatomic ElementsH2
N2 O2 F2
Cl2
Br2
I2
Tl At
S
Li
Na
K
Fr
Be
Mg
Ca
Ra
Sc
Ac
He
Ne
Ar
Kr
Rn
Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se
Rb Sr Y XeZr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Pb Bi Po
Al Si P
B C
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
S
Tl