The Simplified Periodic Table: Elements Ordered By Their Sub-Shell
Ben Alper
Cranfield University, Bedfordshire, MK43 0AL, ben_alper@live.com
Abstract: This article introduces a periodic table in which the elements are ordered by the energy level of their sub shells
and by the number of electrons in their outer shell. Such a layout is both representative of the structure of atoms and has
utility since it is easy to use. This article also introduces electron ’promotion’ which is a simple concept for characterising
the structure of elements which do not conform to the Aufbau principle.
Development of the periodic table
Dmitri Mendeleev created the forerunner of the traditional
periodic table 140 years ago in 1869. The elements were ordered
by atomic weight and arranged so that elements with similar
repeating properties were aligned in columns. Unlike other tables,
Mendeleev’s was able to predict the weight and properties of new
elements.
In 1919 Henry Moseley reordered some elements in order of
atomic charge rather than atomic weight: swapping Argon with
Potassium, and putting Cobalt before Nickel.
In 1945 during the Manhattan project, as Glenn Seaborg
synthesised new elements he noticed that the Actinide group had
different properties to the transition metals. He removed it and put
it in a separate block along with the Lanthanide group resulting in
the modern version of the traditional periodic table.
Quantum theory of electron sub shells
In 1923 Bohr proposed that the periodicity of the periodic table
could be explained if the electrons (or quanta) orbiting the nucleus
were ordered in shells. This was corrected to include sub shells by
Stoner & Summerfield in 1924, and was further corrected by Pauli
1925, Schrodinger in 1926 and finally Madelung in1936.
Despite the advances in understanding of atomic structure, the
periodic table was left unchanged, perhaps because no one could be
sure that the most recent change to the sub-shell structure would be
the last. Even now, there is uncertainty over whether experimental
evidence really proves the order of the sub shells. However there
have been no major changes to the consensus on sub-shell structure
in the last 70 years making sudden new developments less likely.
The order of electron sub shells
There are 4 types of sub shell known as s, p, d and f. S sub
shells contain up to 2 electrons; p sub shells contain up to 6
electrons; d sub shells contain up to 10 electrons and f sub shells
contain up to 14 electrons. Prefixing each sub shell type is the
number of the shell known as the ‘principle quantum number’ thus
the full name of a sub shell is written as e.g. ‘1s’.
The naming convention of the principle quantum number is an
artefact of the outdated Bohr model of the atom and can be
misleading since the higher sub shells in a Bohr shell overlap the
lower sub shells of the next shell, as shown in figure 2.
The table below shows the order in which the sub shells are
filled for the first 36 elements.
Element
Hydrogen
Helium
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
Sodium
Magnesium
Symbol
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
No
1
1
3
4
5
6
7
8
9
10
11
12
Electron Configuration
1s1
1s2
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p5
1s2 2s2 2p6
1s2 2s2 2p6 3s1
1s2 2s2 2p6 3s2
Aluminium
Silicon
Phosphorus
Sulfur
Chlorine
Argon
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
Al
Si
P
S
Cl
Ar
K
Ca
Sc
Ta
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
1s2 2s2 2p6 3s2 3p1
1s2 2s2 2p6 3s2 3p2
1s2 2s2 2p6 3s2 3p3
1s2 2s2 2p6 3s2 3p4
1s2 2s2 2p6 3s2 3p5
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p6 4s1
1s2 2s2 2p6 3s2 3p6 4s2
1s2 2s2 2p6 3s2 3p6 3d1 4s2
1s2 2s2 2p6 3s2 3p6 3d2 4s2
1s2 2s2 2p6 3s2 3p6 3d3 4s2
1s2 2s2 2p6 3s2 3p6 3d5 4s1
1s2 2s2 2p6 3s2 3p6 3d5 4s2
1s2 2s2 2p6 3s2 3p6 3d6 4s2
1s2 2s2 2p6 3s2 3p6 3d7 4s2
1s2 2s2 2p6 3s2 3p6 3d8 4s2
1s2 2s2 2p6 3s2 3p6 3d10 4s1
1s2 2s2 2p6 3s2 3p6 3d10 4s2
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p1
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p2
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p5
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
Table 1: The order in which electron shells are filled for the first
36 atoms.
With a small number of exceptions, the electron shells of each
element are filled in the same way as for the element before it, but
with an extra electron in the outermost sub shell. This is known as
the Aufbau principle. When a sub shell is filled, then the next
outermost shell begins to be filled, as shown in figure 1.
The order in which the sub shells are filled goes in order of the
energy level of the sub shell, rather than the shell number. For
example the 4s electron sub-shell is filled before the 3d sub-shell.
The order of sub-shell energy levels can be seen in figure 2. D
sub-shells have similar energy levels to the F sub-shell of the shell
below and there is in fact some overlapping of the 5f and 6d sub
shells. The number of elements with electron positions filled in an
unexpected order is 19 out of 120 elements. However, in general
the electrons positions are filled as expected, and the order in
which the sub-shells are filled are as follows: 1s, 2s, 2p, 3s, 3p, 4s,
3d, 4p, 5s, 4d, 5p, 6s, 5f, 5d, 6p, 7s, 5f, 6d, 7p, 8s.
From table 1, it can be seen that elements such as Chromium
and Copper do not follow the usual pattern of the Aufbau principle.
Their unusual configuration is highlighted in bold in table 1. The
change in order of the electrons can be described by ‘electron
promotion’ by which an element in a lower sub shell transfers to
higher sub shell as the lowest energy state for that element.
Figure 1: Filled electrons states for
a phosphorus atom
Elements ordered by their outer sub shell
In the ‘Quantum table of the elements’; shown in figure 5,
along the x axis, the elements are ordered by the energy levels of
their outer sub shell. The number of electrons in the outer sub shell
of each element are found down the y axis. The number of
electrons in the outer sub shell affects the properties of the
elements. Atoms with full outer sub shells are in a lower energy
state than atoms with partially filled sub shells. In order to reach
this lower energy state atoms are driven to bond with each other
through ionic or valence bonding. As an example of this, the
Noble gasses are un-reactive as they have full outer sub shells.
Figure 2: Energy levels of the sub shells.
Energy Level
6d Sub-Shell
1s
2s
2p
3s
3p
4s
3d
4p
5s
4d
5p
6s
4f
5d
6p
7s
5f
1
H
Li
B
Na
Al
K
Sc
Ga
Rb
Y
In
Cs
La
Lu
Ti
Fr
Ac
Lr
1
3
5
11
13
19
21
31
37
39
49
55
57
71
81
87
89
103 113 119
2
He
Be
C
Mg
Si
Ca
Ti
Ge
Sr
Zr
Sn
Ba
Ce
Hf
Pb
Ra
Th
Rf Uuq Ubn
2
4
6
12
14
20
22
32
38
40
50
56
58
72
82
88
90
104 114 120
Uut Uue
3
N
P
V
As
Nb
Sb
Pr
Ta
Bi
Pa
Db Uup
7
15
23
33
41
51
59
73
83
91
105 115
4
O
S
Cr
Se
Mo
Te
Nd
W
Po
U
Sg Uuh
8
16
24
34
42
52
60
74
84
92
106 116
5
F
Cl
Mn
Br
Tc
I
Pm Re
At
Np
Bh Uus
9
17
25
35
43
53
61
75
85
93
107 117
6
Ne
Ar
Fe
Kr
Ru
Xe
Sm Os
Rn
Pu
Hs Uuo
10
18
26
36
44
54
62
86
94
108 118
76
7
Co
Rh
Eu
Ir
27
45
63
77
8
Ni
Pd
Gd
Pt
Am Mt
95
109
Cm Ds
28
46
64
78
96
9
Cu
Ag
Tb
Au
Bk
Rg
29
47
65
79
97
111
10
Zn
Cd
Dv
Hg
Cf
Cn
30
48
66
80
98
112
11
Ho
67
99
12
Er
Fm
68
100
13
Tm
Md
69
101
14 Electrons in outer shell
Yb
No
70
102
110
Es
Figure 3: The Quantum table ordering elements by the energy levels of their sub shells.
Advantages of the Quantum table
The Quantum table is simpler and more elegant than the
traditional periodic table and other designs. This gives advantages
to students studying chemistry as it allows them to understand how
the position and properties of an element relate to its atomic
structure. The user can visualise the table as an atom with layers of
shells.
One can see directly by looking at the table, how many
electrons are in the outer shell of each element and how many it
needs to gain or loose to become stable. For example in the case of
a reaction between Oxygen and Hydrogen, it can be seen that
hydrogen needs to gain or loose 1 electron and that Oxygen needs
to gain two electrons. Since they are both non metals, the simplest
structure they could form would have two Hydrogen atoms sharing
their outer electrons with a single Oxygen atom, giving the same
number of electrons as Neon, with 10 electrons. When lithium
reacts with oxygen it forms Li2O or Li2O2. Respectively these
have the same number of electrons as Neon (10) and Magnesium
(12) which has a full ‘s’ type shell.
The table also eases the introduction of students to quantum
effects.
In terms of visual cohesiveness, the table’s continuous
progression includes the Lanthanide and Actinide groups. The
table has the same width as the traditional table: 18 elements; and
similar depth: 14 elements compared with 9 elements and a gap.
Problems with the traditional table
Figure 4: Sub shells represented in each row of the traditional
periodic table.
The left column of figure 4 indicates the sub shells that are
filled as the atomic number increases. More than one electron shell
is represented in each row. By merging the sub shells together the
traditional periodic table reduces the clarity of the data it presents.
In addition the 4f and 5f sub shells occur in two different rows, as
do the 5d and 6d sub shells, adding further complexity.
Use in identifying ‘electron promotion’
Elements such as Copper, Silver and Gold have an unusual
arrangements of electrons, thus Silver has 10 electrons in its outer
shell rather than 9. This is because an electron that would normally
be in a lower sub shell is found instead in the outer sub shell. The
Quantum table shown in figure 5 identifies elements with electron
promotion and shows the types of electron promotion so that the
user is aware of the atomic structure of these elements.
Other versions of the periodic table that include sub shells
Hundreds of other types of periodic table have been published
or have reached the popular media, however these are all variations
on a small number of themes. Most relevant to this article is the
left step periodic table, the first version of which was first
published by Janet in 1928 and more recent versions of which have
been popularised by Valery Tsimmerman. This table orders the
elements by sub shell, yet groups the sub shells together as in the
traditional periodic table, eliminating the benefit. These tables also
tend to be very long and thin, making them difficult to follow.
Secondly there are many tables designed as spirals and circles
to mimic the shape of atoms, one for example, is popularised by
Eric Sterri. However these are difficult to use since the atoms are
not aligned in order of their atomic number.
Use of the table
Any predictions that can be made about the properties of
elements by their position on the traditional table can be made with
the quantum table.
Periodicity with regards to atomic radii, ionisation energy,
electron affinity, metallic character, electronegativity and atomic
emissions all hold true.
For example Noble gasses all have full p type outer sub shells.
Magnetic materials are all have a 3d type outer sub shell; highly
reactive chemicals such as Lithium, Sodium, Potassium and
Caesium all have ‘s’ type outer sub shells with 1 electron, i.e. in
they are the same row. Calcium, Strontium and Barium all have ‘s’
type outer shells with 2 electrons; Sulphur, Selenium and
Tellurium all have ‘p’ type outer shells with 4 electrons; Chlorine,
Bromine and Iodine all have ‘p’ type outer shells with 5 electrons;
Copper, Silver and Gold all have ‘d’ type outer sub shells with 9
electrons. The Noble metals all have ‘d’ type outer shells with
between 6 and 9 electrons in the outer sub shell. Catalysts with
similar properties such as Nickel, Palladium and Platinum also all
have ‘d’ type outer sub shells but with 8 electrons.
For elements with ‘p’ type outer sub shells, the properties
change for larger atoms. For example semiconductors all have ‘p’
type outer shells but the number of electrons in the outer shell is
higher for higher level p shells. The relative conductivity gradually
increases with larger atoms, even with the same number of
electrons in the ‘p’ type outer shell.
In general, to find an element with a similar property to another
one, it is best to examine elements with an outer shell of the same
type and a similar number of electrons in the outer shell.
Electron Promotion
As discussed above, electrons do not always fill the electron
shells exactly as would be expected. In some elements a gap
appears in an inner shell, and the electron that would normally fill
this space is found in the outer shell.
There are 2 categories of electron promotion; firstly an electron
can jump from a lower shell into the outer shell of this element;
this occurs for the elements: Cr, Cu, Nb, Mo, Ru, Rh, Ag, Pt, Pd,
Au, Uun and Uub. In the case of Pd, this happens to 2 electrons.
In the second category of electron promotion an electron can jump
from the outer shell of this element into a higher shell; this occurs
in the cases of Gd, Ac, Th, Pa, U, Np and Cm.
Details of Electron promotion
Examining ‘electron promotion’ in greater detail, one can see
that there are four different types of electron promotion: an electron
promoted from an ‘s’ type sub shell; two electrons promoted from
an ‘s’ type sub shell; an electron promoted from an ‘s’ type sub
shell that jumps over an ‘f’ type shell into the outer d shell and an
electron promoted from an ‘f’ type sub shell:
Promoted 's': an electron from the highest 's' sub shell jumps up to
the outer sub shell: Cr, Cu have [Ar] 4s1 3d(N+1) and
Nb, Mo, Ru, Rh and Ag have [Kr] 5s1 4d(N+1)
Double promoted 's': 2 electrons from the highest 's' sub shell
jump up to the outer sub shell:
Pd has [Kr] 5s0 4d(N+2)
Jumping promoted 's': an electron from the highest 's' sub shell
jump up to the outer sub shell and jumps over an 'f' shell to get
there:
Pt and Au have [Xe] 6s1 4f14 5d(N+1) and
Uun and Uub have [Rn] 7s1 5f14 6d(N+1)
Promoted 'f': electron from outer 'f' sub shell jumps up to outer
sub shell:
Gd has [Ba] 4f(N-1) 5d1 and
Ac, Th, Pa, U, Np and Cm have [Ra] 5f(N-1) 6d.
Where 'N' is the number of electrons in the outer shell.
Acknowledgement. The author would like to acknowledge
helpful discussions with Rajeeve Dattani and encouragement from
Professor Jeremy Ramsden.
Figure 5: The Quantum table of the elements, colour version
C
12.01
Ar
39.95
ARGON
18
NEON
20.18
Ne
10
Cl
35.45
CHLORINE
17
F
19.00
FLUORINE
9
S
32.07
SULPHUR
16
O
16.00
OXYGEN
8
PHOSPHORUS
30.97
NITROGEN
15
P
14.01
Si
28.09
SILICON
14
Mg
24.31)
MAGNESIUM
12
Al
ALUMINIUM
SODIUM
13
26.98
3p
Na
11
22.99
3s
N
7
CALCIUM
5
BORON
B
10.81
Element Name
Atomic Number
Symbol
Synthetic
Relative atomic mass
Promoted ‘f’
Gd has [Ba] 4f(N-1) 5d1
Ac, Th, Pa, U, Np & Cm have [Ra] 5f(N-1) 6d1
Jumping promoted ‘s’
Pt & Au have [Xe] 6s1 4f14 5d(N+1)
Rg & Cn have [Rn] 7s1 5f14 6d(N+1)
Double promoted ‘s’
Pd has [Kr] 5s0 4d(N+2)
40.08
Ca
20
POTASSIUM
K
39.10
4s
19
Promoted ‘s’
Cr, Cu have [Ar] 4s1 3d(N+1)
Nb, Mo, Ru, Rh & Ag have [Kr] 5s1 4d(N+1)
Fe Naturally Occurring
f
S
S
S
S
B
BORON
CARBON
6
5
10.81
2p
Elements with electron promotion
Be
9.01
BERYLLIUM
4
HELIUM
4.00
He
2
Li
LITHIUM
H
HYDROGEN
3
6.94
2s
Electrons in outer shell
14
13
12
11
10
9
8
7
6
5
4
3
2
1
1
1.01
1s
47.87
50.94
54.94
55.85
87.62
74.92
78.96
79.90
83.80
91.22
Mo
127.6
45
S
102.91
RUTHENIUM
S
101.07
Ru
44
TECHNETIUM
43
121.76
127.60
Te
52
ANTIMONY
Sb
51
TIN
I
126.90
131.29
Actinide
Lanthanide
137.33
Not yet discovered
BARIUM
Ba
56
CAESIUM
Cs
132.91
6s
55
Nobel Gases
Non-metals
Semimetals
Alkali metals and
Alkali earth metals
Transition metals
Poor metals
XENON
Xe
54
IODINE
53
Hydrogen
Cd
CADMIUM
112.41
SILVER
48
ZINC
65.4
S
107.87
Ag
47
Zn
30
COPPER
Cu
S
63.55
PALLADIUM
29
NICKEL
S
S
106.42
Pd
46
Ni
58.69
RHODIUM
28
116.71
Sn
50
INDIUM
In
49
114.82
5p
MOYBDENIUM TELLURIUM
S
95.94
NIOBIUM
42
S
92.91
Nb
41
ZIRCONIUM
Zr
40
YITRIUM
Y
39
88.91
4d
COBALT
KRYPTON
Kr
36
BROMINE
Br
35
SELENIUM
Se
34
ARSENIC
As
33
GERMANIUM STRONTIUM
Sr
38
RUBIDIUM
Rb
37
85.47
5s
Rh
58.93
72.64
Ge
32
GALLIUM
Ga
31
69.72
4p
Co
27
IRON
Fe
26
MANGANESE
Mn
25
CHROMIUM
S
52.00)
Cr
24
VANADIUM
V
23
TITANIUM
Ti
22
SCANDIUM
Sc
21
44.96
3d
140.91
180.95
Ta
73
144.24
(145)
150.36
183.84
186.21
76
190.23
RHENIUM
Re
75
TUNGSTEN
W
74
207.20
208.96
(209)
(210)
86
(222)
ASTATINE
At
85
POLONIUM
Po
84
BISMUTH
Bi
83
LEAD
Pb
82
THALLIUM
Ti
81
204.38
6p
151.96
158.93
162.50
164.93
167.26
168.93
173.04
YITERBIUM
Yb
70
THULIUM
Tm
69
ERBIUM
Er
68
HOLMIUM
Ho
67
DYSPROSIUM
Dv
66
TERBIUM
Tb
65
GADOLINIUM
f
157.25
Gd
64
EUROPIUM
Eu
63
SAMARIUM
192.22
MERCURY
Hg
200.59
GOLD
80
S
196.97
Au
79
PLATINUM
S
195.08
Pt
78
IRIDIUM
Ir
77
OSMIUM
RADON
Sm Os Rn
62
PROMETHIUM
61
NEODYMIUM
Nd
60
PRASEODYMIUM TANTALUM
Pr
59
Hf
178.49
HAFNIUM
72
CERIUM
140.12
LUTETIUM
Lu
71
174.97
5d
Ce
58
LANTHANUM
La
57
138.91
4f
(226)
RADIUM
Ra
88
FRANCIUM
Fr
(223)
7s
87
Quantum Table of the Elements
f
f
f
(237)
(244)
(243)
(247)
(238)
(252)
(257)
(258)
(259)
NOBELIUM
102
MENDELEVIUM
101
FERMIUM
100
EINSTEINIUM
99
(293)
(261)
114
(298)
(262)
(266)
(299)
116
(302)
UNUNPENTIUM
115
(264)
(277)
(268)
S
(281)
111
S
(272)
DARMSTADTIUM
110
MEITNERIUM
109
HASSIUM
108
BOHRIUM
107
112
(285)
(310)
(314)
UNUNOCTIUM
118
UNUNSEPTIUM
117
SEABORGIUM UNUNHEXIUM
106
DUBNIUM
105
RUTH’FORDIUM UNUNQUADIUM
104
CALIFORNIUM COPERNICIUM
98
113
(316)
(238)
UNBINILIUM
120
UNUNENNIUM
119
7p Shell
LAWRENCIUM UNUNTRIUM
103
(262)
6d
BERKELIUM ROENTGENIUM
97
f
(247)
CURIUM
96
AMERICIUM
95
PLUTONIUM
94
NEPTUNIUM
93
URANIUM
f
238.03
U
92
PROTACTINIUM
Pa
231.04
THORIUM
91
f
232.04
Th
90
ACTINIUM
Ac
89
(238)
5f
Figure 6: The Quantum table of the elements, black and white version
C
12.01
Ar
39.95
ARGON
18
NEON
20.18
Ne
10
Cl
35.45
CHLORINE
17
F
19.00
FLUORINE
9
S
32.07
SULPHUR
16
O
16.00
OXYGEN
8
PHOSPHORUS
30.97
NITROGEN
15
P
14.01
Si
28.09
SILICON
14
Mg
24.31)
MAGNESIUM
12
Al
ALUMINIUM
SODIUM
13
26.98
3p
Na
11
22.99
3s
N
7
CALCIUM
5
BORON
B
10.81
Element Name
Atomic Number
Symbol
Synthetic
Relative atomic mass
Promoted ‘f’
Gd has [Ba] 4f(N-1) 5d1
Ac, Th, Pa, U, Np & Cm have [Ra] 5f(N-1) 6d1
Jumping promoted ‘s’
Pt & Au have [Xe] 6s1 4f14 5d(N+1)
Rg & Cn have [Rn] 7s1 5f14 6d(N+1)
Double promoted ‘s’
Pd has [Kr] 5s0 4d(N+2)
40.08
Ca
20
POTASSIUM
K
39.10
4s
19
Promoted ‘s’
Cr, Cu have [Ar] 4s1 3d(N+1)
Nb, Mo, Ru, Rh & Ag have [Kr] 5s1 4d(N+1)
Fe Naturally Occurring
f
S
S
S
S
B
BORON
CARBON
6
5
10.81
2p
Elements with electron promotion
Be
9.01
BERYLLIUM
4
HELIUM
4.00
He
2
Li
LITHIUM
H
HYDROGEN
3
6.94
2s
Electrons in outer shell
14
13
12
11
10
9
8
7
6
5
4
3
2
1
1
1.01
1s
47.87
50.94
54.94
55.85
87.62
74.92
78.96
79.90
83.80
91.22
Mo
127.6
45
S
102.91
RUTHENIUM
S
101.07
Ru
44
TECHNETIUM
43
121.76
127.60
Te
52
ANTIMONY
Sb
51
TIN
I
126.90
131.29
Actinide
Lanthanide
137.33
Not yet discovered
BARIUM
Ba
56
CAESIUM
Cs
132.91
6s
55
Nobel Gases
Non-metals
Semimetals
Alkali metals and
Alkali earth metals
Transition metals
Poor metals
XENON
Xe
54
IODINE
53
Hydrogen
Cd
CADMIUM
112.41
SILVER
48
ZINC
65.4
S
107.87
Ag
47
Zn
30
COPPER
Cu
S
63.55
PALLADIUM
29
NICKEL
S
S
106.42
Pd
46
Ni
58.69
RHODIUM
28
116.71
Sn
50
INDIUM
In
49
114.82
5p
MOYBDENIUM TELLURIUM
S
95.94
NIOBIUM
42
S
92.91
Nb
41
ZIRCONIUM
Zr
40
YITRIUM
Y
39
88.91
4d
COBALT
KRYPTON
Kr
36
BROMINE
Br
35
SELENIUM
Se
34
ARSENIC
As
33
GERMANIUM STRONTIUM
Sr
38
RUBIDIUM
Rb
37
85.47
5s
Rh
58.93
72.64
Ge
32
GALLIUM
Ga
31
69.72
4p
Co
27
IRON
Fe
26
MANGANESE
Mn
25
CHROMIUM
S
52.00)
Cr
24
VANADIUM
V
23
TITANIUM
Ti
22
SCANDIUM
Sc
21
44.96
3d
140.91
180.95
Ta
73
144.24
(145)
150.36
183.84
186.21
76
190.23
RHENIUM
Re
75
TUNGSTEN
W
74
151.96
158.93
162.50
164.93
167.26
168.93
173.04
YITERBIUM
Yb
70
THULIUM
Tm
69
ERBIUM
Er
68
HOLMIUM
Ho
67
DYSPROSIUM
Dv
66
TERBIUM
Tb
65
GADOLINIUM
f
157.25
Gd
64
EUROPIUM
Eu
63
SAMARIUM
192.22
MERCURY
Hg
200.59
GOLD
80
S
196.97
Au
79
PLATINUM
S
195.08
Pt
78
IRIDIUM
Ir
77
OSMIUM
Sm Os
62
PROMETHIUM
61
NEODYMIUM
Nd
60
PRASEODYMIUM TANTALUM
Pr
59
Hf
178.49
HAFNIUM
72
CERIUM
140.12
LUTETIUM
Lu
71
174.97
5d
Ce
58
LANTHANUM
La
57
138.91
4f
207.20
208.96
(209)
(210)
(222)
RADON
Rn
86
ASTATINE
At
85
POLONIUM
Po
84
BISMUTH
Bi
83
LEAD
Pb
82
THALLIUM
Ti
81
204.38
6p
(226)
RADIUM
Ra
88
FRANCIUM
Fr
(223)
7s
87
Quantum Table of the Elements
f
f
f
(237)
(244)
(243)
(247)
(238)
(252)
(257)
(258)
(259)
NOBELIUM
102
MENDELEVIUM
101
FERMIUM
100
EINSTEINIUM
99
(293)
(261)
114
(298)
(262)
(266)
(299)
116
(302)
UNUNPENTIUM
115
(264)
(277)
(268)
S
(281)
111
S
(272)
DARMSTADTIUM
110
MEITNERIUM
109
HASSIUM
108
BOHRIUM
107
112
(285)
(310)
(314)
UNUNOCTIUM
118
UNUNSEPTIUM
117
SEABORGIUM UNUNHEXIUM
106
DUBNIUM
105
RUTH’FORDIUM UNUNQUADIUM
104
CALIFORNIUM COPERNICIUM
98
113
(316)
(238)
UNBINILIUM
120
UNUNENNIUM
119
7p Shell
LAWRENCIUM UNUNTRIUM
103
(262)
6d
BERKELIUM ROENTGENIUM
97
f
(247)
CURIUM
96
AMERICIUM
95
PLUTONIUM
94
NEPTUNIUM
93
URANIUM
f
238.03
U
92
PROTACTINIUM
Pa
231.04
THORIUM
91
f
232.04
Th
90
ACTINIUM
Ac
89
(238)
5f