Development of Periodic Table

1
Development of Periodic Table
Development of Periodic Table
J.W. Dobereiner (1829)
J.W. Dobereiner (1829)
Law of Triads
Law of Triads
Elements could be classified into groups of
three, or triads. Trends in physical properties
such as density, melting point, and atomic mass
were observed.
J.A.R. Newlands (1864)
J.A.R. Newlands (1864)
Law of Octaves
Law of Octaves
Arranged the 62 known elements into groups of
seven according to increasing atomic mass. He
proposed that an eighth element would then repeat
the properties of the first element in the
previous group.
Arranged the 62 known elements into groups of
seven according to increasing atomic mass. He
proposed that an eighth element would then repeat
the properties of the first element in the
previous group.
Lothar Meyer (1830 1895)
Lothar Meyer (1830 1895)
Invented periodic table independently of
Mendeleev
Invented periodic table independently of
Mendeleev
his work was not published until 1870 - one year
his work was not published until 1870 - one year
2
Dmitri Mendeleev
Dmitri Mendeleev

• Russian
• Invented periodic table
• Organized elements by properties
• Arranged elements by atomic mass
• Predicted existence of several unknown elements
• Element 101

• Russian
• Invented periodic table
• Organized elements by properties
• Arranged elements by atomic mass
• Predicted existence of several unknown elements
• Element 101

Dmitri Mendeleev
Dmitri Mendeleev
3
Modern Periodic Table

• Henry G.J. Moseley
• Determined the atomic numbers of elements from
  their X-ray spectra (1914)
• Arranged elements by increasing atomic number
• Killed in WW I at age 28
• (Battle of Gallipoli in Turkey)

1887 - 1915
4
Groups of Elements
1
18
2
13
14
15
16
17
Alkali metals
Oxygen family
1
16
Halogens
Alkaline earth metals
17
2
Noble gases
Nitrogen family
15
18
Dorin, Demmin, Gabel, Chemistry The Study of
Matter , 3rd Edition, 1990, page 367
5
Metals and Nonmetals
He 2
H 1
1
Li 3
C 6
N 7
O 8
F 9
Ne 10
B 5
Be 4
Nonmetals
2
Na 11
Al 13
Si 14
P 15
S 16
Cl 17
Ar 18
Mg 12
3
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
4
METALS
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
5
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
6

Fr 87
Ra 88
Rf 104
Db 105
Sg 106
Bh 107
Hs 108
Mt 109
7
W
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
La 57
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
Ac 89
6
Metals, Nonmetals, Metalloids
1
Nonmetals
2
3
4
Metals
5
6
7
Metalloids
Zumdahl, Zumdahl, DeCoste, World of Chemistry
2002, page 349
7
Properties of Metals, Nonmetals, and Metalloids
METALS
malleable, lustrous, ductile, good conductors of
heat and electricity
NONMETALS
gases or brittle solids at room temperature, poor
conductors of heat and electricity (insulators)
(Semi-metals)
METALLOIDS
dull, brittle, semi-conductors (used in computer
chips)
8
Orbitals Being Filled
1
8
Groups
2
1s
1s
3 4 5 6 7
1
2s
2p
2
3s
3p
3
4p
3d
Periods
4s
4
4d
5p
5s
5
5d
6p
La
6s
6
6d
Ac
7s
7
4f
Lanthanide series
5f
Actinide series
Zumdahl, Zumdahl, DeCoste, World of Chemistry
2002, page 345
9
Electron Filling in Periodic Table
s
s
p
1
2
d
3
4
5
6

7
W
f

W
10
Melting Points
He 0.126
He -269.7
H -259.2
Mg 650
1
1
Symbol Melting point oC
Li 180.5
C 4100
N -210.1
O -218.8
F -219.6
Ne -248.6
B 2027
Be 1283
2
2
3000 oC
2000 - 3000 oC
Na 98
Al 660
Si 1423
P 44.2
S 119
Cl -101
Ar -189.6
Mg 650
3
3
K 63.2
Ca 850
Sc 1423
Ti 1677
V 1917
Cr 1900
Mn 1244
Fe 1539
Co 1495
Ni 1455
Cu 1083
Zn 420
Ga 29.78
Ge 960
As 817
Se 217.4
Br -7.2
Kr -157.2
4
4
Rb 38.8
Sr 770
Y 1500
Zr 1852
Nb 2487
Mo 2610
Tc 2127
Ru 2427
Rh 1966
Pd 1550
Ag 961
Cd 321
In 156.2
Sn 231.9
Sb 630.5
Te 450
I 113.6
Xe -111.9
5
5
Cs 28.6
Ba 710
Hf 2222
Ta 2997
W 3380
Re 3180
Os 2727
Ir 2454
Pt 1769
Au 1063
Hg -38.9
Tl 303.6
Pb 327.4
Bi 271.3
Po 254
At
Rn -71
La 920
6
6
Ralph A. Burns, Fundamentals of Chemistry , 1999,
page 1999
11
Diatomic Molecules
Chlorine (Cl2) atomic radius 99 pm
Hydrogen (H2) atomic radius 37 pm
Distance between nuclei
Nucleus
Fluorine (F2) atomic radius 64 pm
Bromine (Br2) atomic radius 114 pm
Oxygen (O2) atomic radius 66 pm
Atomic radius
Iodine (I2) atomic radius 138 pm
Nitrogen (N2) atomic radius 71 pm
HOBrFINCl twins
H2 O2 Br2 F2 I2 N2 Cl2
12
Atomic Radii
IA IIA IIIA
IVA VA VIA VIIA
Li
Be
O
N
C
B
F
Na
Mg
Al
Si
P
Cl
S
K
Ca
Br
Se
As
Ge
Ga
Rb
Sr
In
Te
Sb
Sn
I
Cs
Ba
Pb
Tl
Bi
13
Periodic Trends in Atomic Radii
LeMay Jr, Beall, Robblee, Brower, Chemistry
Connections to Our Changing World , 1996, page 175
14
Relative Size of Atoms
Zumdahl, Zumdahl, DeCoste, World of Chemistry
2002, page 350
15
Trends in Atomic and Ionic Size
Metals
Nonmetals
Group 1
Group 17
Al3
Cations are smaller than parent atoms
Anions are larger than parent atoms
16
Energy
e
e
Li
Li

e
Lithium ion
Lithium atom
17
The Octet Rule and Common Ions
Oxygen atom O 1s22s22p4
Fluorine atom F 1s22s22p5
Sodium atom Na 1s22s22p63s1
Magnesium atom Mg 1s22s22p63s2
Neon atom Ne 1s22s22p6
Oxygen ion O2- 1s22s22p6
Fluorine ion F1- 1s22s22p6
Sodium ion Na1 1s22s22p6
Magnesium ion Mg2 1s22s22p6
18
Isoelectronic Species
Isoelectronic - all species have the same number
of electrons.
p 8 n 8 e 10
p 9 n 9 e 10
p 10 n 10 e 10
p 11 n 11 e 10
p 12 n 12 e 10
Oxygen ion O2- 1s22s22p6
Fluorine ion F1- 1s22s22p6
Sodium ion Na1 1s22s22p6
Magnesium ion Mg2 1s22s22p6
Neon atom Ne 1s22s22p6
Can you come up with another isoelectronic series
of five elements?
19
First Ionization Energies(kJ/mol)
s
p
H 1312.1
He 2372.5
Li 520.3
Be 899.5
B 800.7
C 1086.5
N 1402.4
O 1314.0
F 1681.1
Ne 2080.8
Na 495.9
Mg 737.8
Al 577.6
Si 786.5
P 1011.8
S 999.7
Cl 1251.2
Ar 1520.6
K 418.9
Ca 589.9
Ga 578.6
Ge 761.2
As 946.5
Se 940.7
Br 1142.7
Kr 1350.8
Rb 402.9
Sr 549.2
In 558.2
Sn 708.4
Sb 833.8
Te 869.0
I 1008.7
Xe 1170.3
Smoot, Price, Smith, Chemistry A Modern Course
1987, page 188
20
He

• Helium (He) has
• a greater IE than H
• same shielding
• greater nuclear charge

n
H
First Ionization energy
Atomic number
21
He

• Li has
• lower IE than H
• more shielding
• Further away outweighs greater nuclear charge

n
H
First Ionization energy
Li
Atomic number
22
He

• Be has higher IE than Li
• same shielding
• greater nuclear charge

n
H
First Ionization energy
Be
Li
Atomic number
23
He

• B has lower IE than Be
• same shielding
• greater nuclear charge
• p-orbitals available

n
H
First Ionization energy
Be
B
Li
Atomic number
24
He
n
H
C
First Ionization energy
Be
B
Li
Atomic number
25
He
n
N
H
C
First Ionization energy
Be
B
Li
Atomic number
26
He
n
N

• Breaks the pattern because removing an electron
  gets to 1/2 filled p orbital

H
O
C
First Ionization energy
Be
B
Li
Atomic number
27
He
n
F
N
H
O
C
First Ionization energy
Be
B
Li
Atomic number
28
He
Ne
n
F
N

• Ne has a lower IE than He
• Both are full energy levels,
• Ne has more shielding
• Greater distance

H
O
C
First Ionization energy
Be
B
Li
Atomic number
29
n

• Na has a lower IE than Li
• Both are s1
• Na has more shielding
• Greater distance

First Ionization energy
Atomic number
30
First Ionization energy
Atomic number
31
Factors Affecting Ionization Energy
Nuclear Charge
The larger the nuclear charge, the greater the
ionization energy.
Shielding effect
The greater the shielding effect, the less the
ionization energy.
Radius
The greater the distance between the nucleus and
the outer electrons of an atom, the less the
ionization energy.
Sublevel
An electron from a full or half-full sublevel
requires additional energy to be removed.
Smoot, Price, Smith, Chemistry A Modern Course
1987, page 189
32
Electron Affinity

• The energy change associated with adding an
  electron to a gaseous atom.
• Easiest to add to group 17.
• Gets them to full energy level.
• Increase from left to right atoms become smaller,
  with greater nuclear charge.
• Decrease as we go down a group.

33
Ionic Size

• Cations form by losing electrons.
• Cations are smaller that the atom they come from.
  
• Metals form cations.
• Cations of representative elements have noble gas
  configuration.

34
Ionic size

• Anions form by gaining electrons.
• Anions are bigger that the atom they come from.
• Nonmetals form anions.
• Anions of representative elements have noble gas
  configuration.

35
Formation of Cation
sodium atom Na
e-
e-
e-
e-
e-
loss of one valence electron
e-
11p
e-
e-
e-
e-
e-
e-
36
Formation of Anion
chlorine atom Cl
gain of one valence electron
e-
e-
e-
e-
e-
e-
e-
e-
17p
e-
e-
e-
e-
e-
e-
e-
e-
e-
e-
37
Formation of Ionic Bond
38
Electron Filling in Periodic Table
metallic character increases
nonmetallic character increases
metallic character increases
nonmetallic character increases
39
Chemical Bonding

• Ionic
• Metal (cation) with non-metal (anion)
• Transfer of electron(s)
• Strong bondhigh melting point
• Covalent
• Non-metal with non-metal
• Sharing of electron(s)
• Non-polar (equal distribution of electrons)
• Polar (uneven electron distribution)
• Weak bondslow melting points
• Single, double and triple bonds
• Metallic (nuclei in a sea of shared electrons)

40
Element Brochure
Research any element you choose and make an
informational brochure to tell about your
element. Creativity may be needed. Technology
assignment (Publisher brochure) Minimum of three
references (one textbook and one internet site)
Title, author, year published and URL Not ALL
writing or not ALL bullets in brochure Use
graphics and pictures to add visual appeal
captions with pictures Front Name of
element, picture/graphic, your name, class hour
Back References, graphic Inside flap facts
melting point, atomic number, Bohr model, etc
Opened brochure (three sectionsinteresting
facts, history, uses)
Brochure should look neat. Writing should be 12
point font. Use only 1 or 2 fonts in entire
brochure.
41
http//education.jlab.org/jsat/powerpoint/chembond
.ppt
http//www.unit5.org/christjs/A4 Periodic
Table_files/frame.htm