1H | 2He | ||||||||||||||||
3Li | 4Be | 5B | 6C | 7N | 8O | 9F | 10Ne | ||||||||||
11Na | 12Mg | 13Al | 14Si | 15P | 16S | 17Cl | 18Ar | ||||||||||
19K | 20Ca | 21Sc | 22Ti | 23V | 24Cr | 25Mn | 26Fe | 27Co | 28Ni | 29Cu | 30Zn | 31Ga | 32Ge | 33As | 34Se | 35Br | 36Kr |
37Rb | 38Sr | 39Y | 40Zr | 41Nb | 42Mo | 43Tc | 44Ru | 45Rh | 46Pd | 47Ag | 48Cd | 49In | 50Sn | 51Sb | 52Te | 53I | 54Xe |
55Cs | 56Ba | 57- 71 |
72Hf | 73Ta | 74W | 75Re | 76Os | 77Ir | 78Pt | 79Au | 80Hg | 91Tl | 82Pb | 83Bi | 84Po | 85At | 86Rn |
87Fr | 88Ra | 89- 103 |
104Rf | 105Db | 106Sg | 107Bh | 108Hs | 109Mt | 110Uun | 111Uuu | 112Uub | 113Uut | 116Uuh | 118Uuo | |||
116 & 118 new in 1999. | |||||||||||||||||
Lanthanides | 57La | 58Ce | 59Pr | 60Nd | 61Pm | 62Sm | 63Eu | 64Gd | 65Tb | 66Dy | 67Ho | 68Er | 69Tm | 70Yb | 71Lu | ||
Actinides | 89Ac | 90Th | 91Pa | 92U | 93Np | 94Pu | 95Am | 96Cm | 97Bk | 98Cf | 99Es | 100Fm | 101Md | 102No | 103Lr |
Metals | Semimetals | Nonmetals | Z, atomic #Symbol |
Organizing
Mendele'ev | OK, you're too young to remember the Cold War, but a favorite Russian
phrase then was "We invented it first!"
Well, in the case of the Periodic Table of the Elements, they were right! Dmitri Mendele'ev was Professor of General Chemistry at University of St. Petersberg when he hit upon an organizing principle for the then known atoms. As they were listed in A (atomic weight) order, the cyclic nature of their chemistry suggested the kind of columnar organization above where the chemistry (reactions and properties) of atoms in a given column were all suspiciously similar despite great differences in their weights. Later we'll see why that has to be so, and I wouldn't want to spoil the surprise, now would I? So we'll content ourselves here with admiring the fact of such periodicity as a mnemonic to chemical prediction.
|
While Mendele'ev thought it a fine way to present the myriad of the
chemical elements to his students (and to you!), his Periodic Table turned
out to be central in the discovery of new elements. For example, the spot
now occupied by 31Ga, Gallium (after the Latin Gallia
name for France), was unknown at the time Mendele'ev organized the elements.
But by the trend in the properties of Boron, B, and Aluminum, Al, he
predicted the kind of chemistry that Eka-Aluminum, as he called it
in 1869. Ga was discovered via those hints only 6 years later by a French
chemist.
Notice that while he didn't discover any elements himself, Mendele'ev is immortalized in the table as the element mendeleevium, 101Md!
| |
The similarities of chemistry of elements in the same column has given rise
to common names for many of them. For example, those in the first column
(except hydrogen which excepts itself from many rules) are called the
Alkali Metals because these metals react strongly with
water to create highly alkaline (chemists would say "basic") solutions.
Our bodies use Na+ and K+ ions in our nerve cells
where their motions through cell membranes constitute the electrical
signals by which we think and sense our environment.
|
1H | Alkali Metals | 2He
3Li
| 4Be
|
| 5B
| 6C
| 7N
| 8O
| 9F
| 10Ne
| 11Na
| 12Mg
|
| 13Al
| 14Si
| 15P
| 16S
| 17Cl
| 18Ar
| 19K
| 20Ca
| 21Sc
| 22Ti
| 23V
| 24Cr
| 25Mn
| 26Fe
| 27Co
| 28Ni
| 29Cu
| 30Zn
| 31Ga
| 32Ge
| 33As
| 34Se
| 35Br
| 36Kr
| 37Rb
| 38Sr
| 39Y
| 40Zr
| 41Nb
| 42Mo
| 43Tc
| 44Ru
| 45Rh
| 46Pd
| 47Ag
| 48Cd
| 49In
| 50Sn
| 51Sb
| 52Te
| 53I
| 54Xe
| 55Cs
| 56Ba
| 57- | 71 72Hf
| 73Ta
| 74W
| 75Re
| 76Os
| 77Ir
| 78Pt
| 79Au
| 80Hg
| 91Tl
| 82Pb
| 83Bi
| 84Po
| 85At
| 86Rn
| 87Fr
| 88Ra
| 89- | 103 104Rf
| 105Db
| 106Sg
| 107Bh
| 108Hs
| 109Mt
| 110Uun
| 111Uuu
| 112Uub
|
|
| Lanthanides
| 57La
| 58Ce
| 59Pr
| 60Nd
| 61Pm
| 62Sm
| 63Eu
| 64Gd
| 65Tb
| 66Dy
| 67Ho
| 68Er
| 69Tm
| 70Yb
| 71Lu
|
| Actinides
| 89Ac
| 90Th
| 91Pa
| 92U
| 93Np
| 94Pu
| 95Am
| 96Cm
| 97Bk
| 98Cf
| 99Es
| 100Fm
| 101Md
| 102No
| 103Lr
|
| |
The second columnar elements also produce alkaline water solutions,
but they are far, far less reactive than the Alkali Metals. This second column
contains what are called the Alkaline Earths. We use
the representative alkaline earth element calcium as a construction element
in our own bones as do shellfish in their shells.
|
1H | Alkaline Earths | 2He
3Li
| 4Be
|
| 5B
| 6C
| 7N
| 8O
| 9F
| 10Ne
| 11Na
| 12Mg
|
| 13Al
| 14Si
| 15P
| 16S
| 17Cl
| 18Ar
| 19K
| 20Ca
| 21Sc
| 22Ti
| 23V
| 24Cr
| 25Mn
| 26Fe
| 27Co
| 28Ni
| 29Cu
| 30Zn
| 31Ga
| 32Ge
| 33As
| 34Se
| 35Br
| 36Kr
| 37Rb
| 38Sr
| 39Y
| 40Zr
| 41Nb
| 42Mo
| 43Tc
| 44Ru
| 45Rh
| 46Pd
| 47Ag
| 48Cd
| 49In
| 50Sn
| 51Sb
| 52Te
| 53I
| 54Xe
| 55Cs
| 56Ba
| 57- | 71 72Hf
| 73Ta
| 74W
| 75Re
| 76Os
| 77Ir
| 78Pt
| 79Au
| 80Hg
| 91Tl
| 82Pb
| 83Bi
| 84Po
| 85At
| 86Rn
| 87Fr
| 88Ra
| 89- | 103 104Rf
| 105Db
| 106Sg
| 107Bh
| 108Hs
| 109Mt
| 110Uun
| 111Uuu
| 112Uub
|
|
| Lanthanides
| 57La
| 58Ce
| 59Pr
| 60Nd
| 61Pm
| 62Sm
| 63Eu
| 64Gd
| 65Tb
| 66Dy
| 67Ho
| 68Er
| 69Tm
| 70Yb
| 71Lu
|
| Actinides
| 89Ac
| 90Th
| 91Pa
| 92U
| 93Np
| 94Pu
| 95Am
| 96Cm
| 97Bk
| 98Cf
| 99Es
| 100Fm
| 101Md
| 102No
| 103Lr
|
| |
On the other side of the table from the highly reactive alkali metals lie
the terribly inert (unreactive) Noble Gases. Only in very
recent years has anyone persuaded any of these atoms to engage in any chemistry
at all! We chemists appreciate that these elements provide perfect inert
atmospheres in which to keep otherwise highly reactive chemicals. But the only
time we find any noble gas in our bodies is when we inhale a lungful of air,
which consists of about 1% Argon! Divers use Helium instead of Nitrogen in the
air they carry with them because it doesn't dissolve in their blood (as does
nitrogen) and bubble out in deadly bends when they ascend from
deep dives.
|
1H | Noble Gases | 2He
3Li
| 4Be
|
| 5B
| 6C
| 7N
| 8O
| 9F
| 10Ne
| 11Na
| 12Mg
|
| 13Al
| 14Si
| 15P
| 16S
| 17Cl
| 18Ar
| 19K
| 20Ca
| 21Sc
| 22Ti
| 23V
| 24Cr
| 25Mn
| 26Fe
| 27Co
| 28Ni
| 29Cu
| 30Zn
| 31Ga
| 32Ge
| 33As
| 34Se
| 35Br
| 36Kr
| 37Rb
| 38Sr
| 39Y
| 40Zr
| 41Nb
| 42Mo
| 43Tc
| 44Ru
| 45Rh
| 46Pd
| 47Ag
| 48Cd
| 49In
| 50Sn
| 51Sb
| 52Te
| 53I
| 54Xe
| 55Cs
| 56Ba
| 57- | 71 72Hf
| 73Ta
| 74W
| 75Re
| 76Os
| 77Ir
| 78Pt
| 79Au
| 80Hg
| 91Tl
| 82Pb
| 83Bi
| 84Po
| 85At
| 86Rn
| 87Fr
| 88Ra
| 89- | 103 104Rf
| 105Db
| 106Sg
| 107Bh
| 108Hs
| 109Mt
| 110Uun
| 111Uuu
| 112Uub
|
|
| Lanthanides
| 57La
| 58Ce
| 59Pr
| 60Nd
| 61Pm
| 62Sm
| 63Eu
| 64Gd
| 65Tb
| 66Dy
| 67Ho
| 68Er
| 69Tm
| 70Yb
| 71Lu
|
| Actinides
| 89Ac
| 90Th
| 91Pa
| 92U
| 93Np
| 94Pu
| 95Am
| 96Cm
| 97Bk
| 98Cf
| 99Es
| 100Fm
| 101Md
| 102No
| 103Lr
|
| |
Moving left a column from the noble gases brings us to the
Halogens which begin as gaseous fluorine, progress
through liquid bromine, and conclude with solid iodine (and astatine, but
nobody much wants to deal with that highly radioactive element). Indeed,
melting and boiling points of the elements follow that trend in general;
the higher values are found further down the table. Halogens are very
corrosive elements; nevertheless our bodies contain them as well. After all,
our nerves may pass electric current but they are not electrically charged
as they would be if their only ions were Na+ and K+.
Each of those ions is balanced by an equivalent number of negative ions,
the most prevalent of which would be Cl- anions. As a general rule,
even ionic compounds are found in an electrically neutral state with as many
positive charges from their "cations" as there are negative ones from their
"anions."
|
1H | Halogens | 2He
3Li
| 4Be
|
| 5B
| 6C
| 7N
| 8O
| 9F
| 10Ne
| 11Na
| 12Mg
|
| 13Al
| 14Si
| 15P
| 16S
| 17Cl
| 18Ar
| 19K
| 20Ca
| 21Sc
| 22Ti
| 23V
| 24Cr
| 25Mn
| 26Fe
| 27Co
| 28Ni
| 29Cu
| 30Zn
| 31Ga
| 32Ge
| 33As
| 34Se
| 35Br
| 36Kr
| 37Rb
| 38Sr
| 39Y
| 40Zr
| 41Nb
| 42Mo
| 43Tc
| 44Ru
| 45Rh
| 46Pd
| 47Ag
| 48Cd
| 49In
| 50Sn
| 51Sb
| 52Te
| 53I
| 54Xe
| 55Cs
| 56Ba
| 57- | 71 72Hf
| 73Ta
| 74W
| 75Re
| 76Os
| 77Ir
| 78Pt
| 79Au
| 80Hg
| 91Tl
| 82Pb
| 83Bi
| 84Po
| 85At
| 86Rn
| 87Fr
| 88Ra
| 89- | 103 104Rf
| 105Db
| 106Sg
| 107Bh
| 108Hs
| 109Mt
| 110Uun
| 111Uuu
| 112Uub
|
|
| Lanthanides
| 57La
| 58Ce
| 59Pr
| 60Nd
| 61Pm
| 62Sm
| 63Eu
| 64Gd
| 65Tb
| 66Dy
| 67Ho
| 68Er
| 69Tm
| 70Yb
| 71Lu
|
| Actinides
| 89Ac
| 90Th
| 91Pa
| 92U
| 93Np
| 94Pu
| 95Am
| 96Cm
| 97Bk
| 98Cf
| 99Es
| 100Fm
| 101Md
| 102No
| 103Lr
|
| |
There are three other groupings of sufficient interest to memorize, but
they aren't columns. One is the Lanthanides which, strictly speaking,
is the run of elements from 57La (lanthanum) through
70Yb (ytterbium) as the second to the last row above.
71Lu (lutecium) is tacked onto the end of that
row because it should occupy the cell between 54Ba (barium) and
72Hf (hafnium) but it can't simply because we've stuck a
sign there, 57-71, to indicate that's where the lanthanides should
really go!
The same thing is true of the Actinides which are the last row from 89Ac (actinium) through 102No (nobelium) but 103Lr (lawrencium) sits at the end because the sign 89-103 occupies its rightful place. We encounter the lanthanides whenever we watch TV since some of them are components of the glowing phosphors in the tube by which we see images. The actinides are mainly artificial elements whose nuclei are so unstable that they are highly radioactive...so much so that none beyond 92U are found in Nature.
| |
The last collection of elements to think about are the Transition
Metals which lie in the row from 21Sc (scandium) through
30Zn (zinc) and the three rows beneath them. They contain
not only elements critical to our technology from the
Bronze Age (29Cu, copper) forward but also
the iron, 26Fe, our bodies need to carry oxygen in our red blood
cells!
And the REST of the table? So important we discuss them individually! But you needn't wait; there's a history of all the elements at the Los Alamos National Laboratory. (Try not to sell any secrets you find there to foreign powers.) |