2.3
List of the Electronic Configuration of Elements Z = 1 to 56 using the
advanced s, p, d and f notation
YOU MUST STUDY Parts 2.1 and 2.2
before studying section 2.3 onwards – The rules of how to assign
electrons in multi–electron atoms to the appropriate quantum levels
were explained in
section 2.2.
The list
below quotes the ground
state electron configurations i.e. the lowest available state
according to the
Aufbau principle
(previously described). The order of filling the electron levels is
listed below and also indicated on the diagram below.
Electron Box diagrams of
the outer electron arrangement and examples of the simple electron
notation (e.g. 2.8.1) are also included, with brief comments
in the end right hand column e.g. element symbol, group, series
etc.
The electrons–in–boxes notation for subshells: Boxes are
used to represent an individual orbital or set of orbitals in the
electrons are shown as arrows. The pairs up/down arrows represent a
full orbital with electrons of opposite spin and note how the
half–filled boxes/orbitals illustrate Hund's rule of maximum
multiplicity
Energy level filling order to Z = 56 is
1s 2s 2p 3s 3p 4s 3d
4p (for Z = 1 to 36) then 5s 4d 5p 6s 4f/5d varies (for Z = 37 to
56)
However, when writing out the
electron configuration you must write them out in order of
strict principal quantum with the accompanying s, p, d, f notation
order of writing out is: 1s 2s 2p 3s 3p 3d
4s 4p 4d 4f 5s 5p 5d 6s (up to Z = 58)
BUT the order of orbital filling is:
1s 2s 2p 3s 3p 4s 3d
4p 5s 4d 5p 6s (up to Z = 56)
So at Z = 21 Sc, you start to fill the 3d
orbitals (NOT 4p orbitals),
then at Z = 31 Ga you start to fill the 4p
orbitals, and this is all you need pre-university! I think?
Atomic
number Z and the element
name and chemical symbol |
Electron configuration
Electron arrangement
s, p, d & f notation with electron
number superscripts (plus some simplified electron arrangements) |
Electron spin box diagrams of
the outer
electron orbitals for the electron configuration of the atom representing the superscripted electrons
beyond
the inner noble gas core [He/Ne/Ar/Kr], the latter are not involved in chemical bonding
or reactions. |
Symbol,
group/series/block and Comments
Gp = Group! |
1
Hydrogen, H |
1s1 |
1s |
H, no
Group really, a bit unique! |
2
Helium, He |
1s2 = [He] |
1s
very stable, unreactive, filled shell |
He, Group
0/18 Noble Gas |
3
Lithium, Li |
1s22s1
(simple notation: 2.1) |
[He]2s 2p
empty sub-shell |
Li,
s–block, Gp1 Alkali Metal, v. reactive |
4
Beryllium, Be |
1s22s2
(2.2) |
[He]2s 2p
empty sub-shell |
Be,
s–block, Gp2 Alkaline Earth Metal, |
5 Boron, B |
1s22s22p1
(2.3) |
[He]2s 2p |
B,
p–block, Group 3/13 |
6
Carbon, C |
1s22s22p2
(2.4) |
[He]2s 2p |
C,
p–block, Group 4/14 |
7
Nitrogen, N |
1s22s22p3
(2.5) |
[He]2s 2p |
N,
p–block, Group 5/15 |
8
Oxygen, O |
1s22s22p4
(2.6) |
[He]2s 2p |
O,
p–block, Group 6/16 |
9
Fluorine, F |
1s22s22p5
(2.7) |
[He]2s 2p |
F,
p–block, Group 7/17 Halogen |
10 Neon, Ne |
1s22s22p6 = [Ne]
(2.8) |
[He]2s 2p
very stable, unreactive, filled outer shell |
Ne,
p–block, Group 0/18 Noble Gas |
11
Sodium, Na |
1s22s22p63s1
(2.8.1) |
[Ne]3s 3p
empty sub-shell |
Na, Gp1
Alkali Metal, v. reactive |
12
Magnesium, Mg |
1s22s22p63s2
(2.8.2) |
[Ne]3s 3p
empty sub-shell |
Mg,
s–block, Gp2 Alkaline Earth Metal, |
13
Aluminium, Al |
1s22s22p63s23p1
(2.8.3) |
[Ne]3s 3p |
Al,
p–block, Group 3/13 |
14
Silicon, Si |
1s22s22p63s23p2
(2.8.4) |
[Ne]3s 3p |
Si,
p–block, Group 4/14 |
15
Phosphorus, P |
1s22s22p63s23p3
(2.8.5) |
[Ne]3s 3p |
P,
p–block, Group 5/15 |
16 Sulfur, S |
1s22s22p63s23p4
(2.8.6) |
[Ne]3s 3p |
S,
p–block, Group 6/16 |
17
Chlorine, Cl |
1s22s22p63s23p5
(2.8.7) |
[Ne]3s 3p |
Cl,
p–block, Group 7/17 Halogen |
18
Argon, Ar |
1s22s22p63s23p6
= [Ar] (2.8.8) |
[Ne]3s 3p
very stable, unreactive, filled outer shell |
Ar,
p–block, Group 0/18 Noble Gas |
19
Potassium, K |
1s22s22p63s23p64s1
(2.8.8.1) |
[Ar]3d 4s 4p |
K,
s–block, Gp1 Alkali Metal, v. reactive |
20
Calcium, Ca |
1s22s22p63s23p64s2
(2.8.8.1) |
[Ar]3d 4s 4p |
Ca,
s–block, Gp2 Alkaline Earth Metal |
21
Scandium, Sc |
1s22s22p63s23p63d14s2 |
[Ar]3d 4s 4p |
Sc, 3d
block, not a true Transition Metal |
22
Titanium, Ti |
1s22s22p63s23p63d24s2 |
[Ar]3d 4s 4p |
Ti, 3d
block, a true Transition Metal |
23
Vanadium, V |
1s22s22p63s23p63d34s2 |
[Ar]3d 4s 4p |
V, 3d
block, a true Transition Metal |
24
Chromium, Cr |
1s22s22p63s23p63d54s1 |
[Ar]3d 4s 4p |
Cr, 3d
block, a true Transition Metal |
25
Manganese, Mn |
1s22s22p63s23p63d54s2 |
[Ar]3d 4s 4p |
Mn, 3d
block, a true Transition Metal |
26 Iron, Fe |
1s22s22p63s23p63d64s2 |
[Ar]3d 4s 4p |
Fe, 3d
block, a true Transition Metal |
27
Cobalt, Co |
1s22s22p63s23p63d74s2 |
[Ar]3d 4s 4p |
Co, 3d
block, a true Transition Metal |
28
Nickel, Ni |
1s22s22p63s23p63d84s2 |
[Ar]3d 4s 4p |
Ni, 3d
block, a true Transition Metal |
29
Copper, Cu |
1s22s22p63s23p63d104s1 |
[Ar]3d 4s 4p |
Cu, 3d
block, a true Transition Metal |
30 Zinc, Zn |
1s22s22p63s23p63d104s2 |
[Ar]3d 4s 4p |
Zn, 3d
block, not a true Transition Metal |
31
Gallium, Ga |
[Ar]3d104s24p1 |
[Ar]3d 4s 4p |
Ga,
p–block, Group 3/13 |
32
Germanium, Ge |
[Ar]3d104s24p2 |
[Ar]3d 4s 4p |
Ge,
p–block, Group 4/14 |
33
Arsenic, As |
[Ar]3d104s24p3 |
[Ar]3d 4s 4p |
As,
p–block, Group 5/15 |
34
Selenium, Se |
[Ar]3d104s24p4 |
[Ar]3d 4s 4p |
Se,
p–block, Group 6/16 |
35
Bromine, Br |
[Ar]3d104s24p5 |
[Ar]3d 4s 4p |
Br,
p–block, Group 7/17 Halogen |
36
Krypton, Kr |
[Ar]3d104s24p6
= [Kr] (2.8.18.8) |
[Ar]3d 4s 4p
very stable, filled outer shell |
Kr,
p–block, Group 0/18 Noble Gas |
37
Rubidium, Rb |
[Kr]5s1 |
[Kr]5s |
Rb,
s–block, Gp1 Alkali Metal, v. reactive |
38
Strontium, Sr |
[Kr]5s2 |
[Kr]5s |
Sr,
s–block, Gp2 Alkaline Earth Metal, |
39
Yttrium, Y |
[Kr]4d15s2 |
[Kr]4d 5s |
Y, 4d block, not
a true Transition Metal |
40
Zirconium, Zr |
[Kr]4d25s2 |
[Kr]4d 5s |
Zr, 4d
block, a true Transition Metal |
41
Niobium, Nb |
[Kr]4d45s1 |
[Kr]4d 5s |
Nb, 4d
block, a true Transition Metal |
42
Molybdenum, Mo |
[Kr]4d55s1 |
[Kr]4d 5s |
Mo, 4d
block, a true Transition Metal |
43
Technetium, Tc |
[Kr]4d55s2 |
[Kr]4d 5s |
Tc, 4d
block, a true Transition Metal |
44
Ruthenium, Ru |
[Kr]4d75s1 |
[Kr]4d 5s |
Ru, 4d
block, a true Transition Metal |
45
Rhodium, Rh |
[Kr]4d85s1 |
[Kr]4d 5s |
Rh, 4d
block, a true Transition Metal |
46
Palladium, Pd |
[Kr]4d10 |
[Kr]4d 5s |
Pd, 4d
block, a true Transition Metal |
47
Silver, Ag |
[Kr]4d105s1 |
[Kr]4d 5s 5p |
Ag, 4d
block, a true Transition Metal |
48
Cadmium, Cd |
[Kr]4d105s2 |
[Kr]4d 5s 5p |
Cd, 4d
block, not a true Transition Metal |
49
Indium, In |
[Kr]4d105s25p1 |
[Kr]4d 5s 5p |
In,
p–block, Group 3/13 |
50 Tin, Sn |
[Kr]4d105s25p2 |
[Kr]4d 5s 5p |
Sn,
p–block, Group 4/14 |
51
Antimony, Sb |
[Kr]4d105s25p3 |
[Kr]4d 5s 5p |
Sb,
p–block, Group 5/14 |
52
Tellurium, Te |
[Kr]4d105s25p4 |
[Kr]4d 5s 5p |
Te,
p–block, Group 6/16 |
53
Iodine, I |
[Kr]4d105s25p5 |
[Kr]4d 5s 5p |
I,
p–block, Group7/17 Halogen |
54
Xenon, Xe |
[Kr]4d105s25p6
= [Xe] |
[Kr]4d 5s 5p
very stable, filled outer shell |
Xe,
p–block, Group 0/8/18 Noble Gas |
55
Caesium, Cs |
[Xe]6s1 |
[Xe]6s |
Cs,
s–block, Gp1 Alkali Metal, v. reactive |
56
Barium, Ba |
[Xe]6s2 |
[Xe]6s |
Ba,
s–block, Gp2 Alkaline Earth Metal, |
57 Lanthanum, La |
[Xe]5d16s2 |
[Xe]5d 6s |
La, start of 5d–bock and Lanthanide Series |
58 Cerium, Ce |
[Xe]4f26s2 not 4f15d16s2 |
things get a bit less systematic in
the f blocks |
Ce, 1st of f–block in the Lanthanides Metals |
************************ |
**************************************** |
********************************************************* |
***************************************************** |
The electron spin box diagrams can be used to
show the full electronic structure e.g.

All based on the right-hand diagram
More 'quantum level quirks'!
A note on
two anomalies in the 3d block,
namely the transition metals chromium and copper:
Cr is [Ar]3d54s1
and not [Ar]3d44s2
and
Cu is[Ar]3d104s1
and not [Ar]3d94s2
because an inner half–filled or fully–filled 3d sub–shells seem to be a little
lower in energy level, and marginally more stable.
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2.4 Electron
configuration and the Periodic Table
Not all the elements
are shown but the position of s, p, d and f blocks are shown and
explained after the table
It is an element's electron
configuration that determines whether it is an s, p, d or f block
element.
Instead of 'simply' assigning an
element to its group or series because of its chemical properties e.g.
formula of similar compounds, we can now
assign an element's position in the periodic table using its electron
configuration.
An
s block element has one or two
outer electrons i.e. ... s1 or ... s2 e.g.
group 1 and group 2 metals (shown below)
A
p block element has 1-6 outer p
electrons beyond the s2 orbital i.e. ... s2p1
to s2p6 e.g. group 3/13 across to group 0/18
(shown below)
A
d block element has 1 to 10
electrons in the outermost set of d orbitals i.e. ...d1 to
...d10 e.g. 3d block of Sc to Zn, 4d block Y to Cd
(shown below)
Note that a
true transition element
has an ion with an incomplete d sub-shell (3d, 4d etc.)
An
f block element has 1 to 14
electrons in the outermost set of f orbitals i.e. ...f1 to
...f14 e.g. Ce to Lu (NOT shown below)
This partial periodic
table relates an element's electron configuration to the element's
position in the periodic table.
You can then see the
patterns between an atom's electron arrangement and the group, block or
series the element belongs to.
Pd |
s block |
3d/4d blocks of Transition Metals (Periods 4/5), the 1st/10th
are NOT true
transition elements, they have no partially filled d shell in an
ion. |
p block
elements |
Gp1 |
Gp2 |
Gp3/13 |
Gp4/14 |
Gp5/15 |
Gp6/16 |
Gp7/17 |
Gp0/8/18 |
1 |
1H 1s1
|
2He 1s2 |
2 |
3Li [He]2s1 |
4Be [He]2s2 |
The electronic structure of Elements
1 to 56, ZSymbol,
Z = atomic or proton
number = total electrons in neutral atom,
[He] = 1s2, [Ne] = 1s22s22p6,
[Ar] = 1s22s22p63s23p6, [Kr] = 1s22s22p63s23p63d104s24p6
Between Groups 2 and 3/13
are the d–blocks and f–blocks where the quantum energy level
rules permit their inclusion. Periods 4 and
5 have 18 elements each, including the
3d (Sc-Zn) and 4d
(Y-Cd) d blocks
of elements
respectively (Groups 3 to 12 – new notation). |
5B [He]2s22p1 |
6C [He]2s22p2 |
7N [He]2s22p3 |
8O [He]2s22p4 |
9F [He]2s22p5 |
10Ne [He]2s22p6 |
3 |
11Na [Ne]3s1 |
12Mg [Ne]3s2 |
13Al [Ne]3s23p1 |
14Si [Ne]3s23p2 |
15P [Ne]3s23p3 |
16S [Ne]3s23p4 |
17Cl [Ne]3s23p5 |
18Ar [Ne]3s23p6 |
4 |
19K [Ar]4s1 |
20Ca [Ar]4s2 |
21Sc [Ar] 3d14s2 |
22Ti [Ar] 3d24s2 |
23V [Ar] 3d34s2 |
24Cr [Ar] 3d54s1 |
25Mn [Ar] 3d54s2 |
26Fe [Ar] 3d64s2 |
27Co [Ar] 3d74s2 |
28Ni [Ar] 3d84s2 |
29Cu [Ar] 3d104s1 |
30Zn [Ar] 3d104s2 |
31Ga [Ar] 3d104s24p1 |
32Ge [Ar] 3d104s24p2 |
33As [Ar] 3d104s24p3 |
34Se [Ar] 3d104s24p4 |
35Br [Ar] 3d104s24p5 |
36Kr [Ar] 3d104s24p6 |
5 |
37Rb [Kr]5s1 |
38Sr [Kr]5s2 |
39Y [Kr] 4d15s2 |
40Zr [Kr] 4d25s2 |
41Nb [Kr] 4d45s1 |
42Mo [Kr] 4d55s1 |
43Tc [Kr] 4d55s2 |
44Ru [Kr] 4d75s1 |
45Rh [Kr] 4d85s1 |
46Pd [Kr] 4d10 |
47Ag [Kr] 4d105s1 |
48Cd [Kr] 4d105s2 |
49In [Kr] 4d105s25p1 |
50Sn [Kr] 4d105s25p2 |
51Sb [Kr] 4d105s25p3 |
52Te [Kr] 4d105s25p4 |
53I [Kr] 4d105s25p5 |
54Xe [Kr] 4d105s25p6 |
6 |
55Cs [Xe]6s1 |
56Ba [Xe]6s2 |
4f–block (14) and 5d–block
(10), total of 32 elements in period 6 including the Lanthanide Series of
Metals. |
81Tl [Xe] 4f145d106s26p1 |
82Pb [Xe]
4f145d106s26p2 |
83Bi [Xe] 4f145d106s26p3 |
84Po [Xe] 4f145d106s26p4 |
85At [Xe]
4f145d106s26p5 |
86Rn [Xe]
4f145d106s26p6 |
7 |
87Fr [Rn]7s1 |
88Ra [Rn]7s2 |
5f–block and 6d–block
including the Actinide Series of Metals in period 7, see full table below |
113Nh [Rn]
5f146d107s27p1 |
114Fl [Rn]
5f146d107s27p2 |
115Mc [Rn]
5f146d107s27p3 |
116Lv [Rn]
5f146d107s27p4 |
117Ts [Rn]
5f146d107s27p5 |
118Og [Rn]
5f146d107s27p6 |
-
Note on Group numbers
-
Using 0 to denote the Group number of Noble Gases is very historic now
since compounds of xenon known exhibiting a valency of 8.
-
Because of the horizontal series
of elements e.g. like the Sc to Zn block (10 elements), Groups 3 to
0 can also be numbered as Groups 13 to 18 to fit in with the
actual number of vertical columns of elements and this is the modern trend
in periodic table notation.
-
This can make things confusing, but there
it is, classification is still in progress!
-
The atomic/proton
number, decides which element an atom is and the outer electron
structure decides which group/block/series the element belongs to and
ultimately its chemistry.
-
The positions of the s, p, d
and f blocks are also indicated Periodic Table above and arise from
the quantum rules
-
s block elements have an
outer shell of just 1 or 2 s electrons i.e. s1 or s2
configuration beyond an inner noble gas configuration (2 per period
from period 2 onwards), that is groups 1 and 2. Technically,
hydrogen and helium are in the s block, but bare little
chemical similarity with the group 1 and group 2 metals.
-
p block elements have an
outer electron configuration of s2p1 to s2p6
i.e. elements where the p sub-shell is being filled (6 per period
from period 2 onwards), that is groups 3/13 to 0/18.
-
d block elements eg the
3d (Sc-Zn) where the 3d
sub-shell is being filled and like wise for the 4d block (Y-Cd),10
elements per block per period from period 4 onwards, the first
horizontal blocks of metals which lie between the s block and p
block,
-
f blocks elements eg the
4f and 5f blocks where the f sub-shells start being filled (14
elements in each block per period from period 6 onwards).
-
The most stable
electron configurations
-
What is the electronic
basis of Groups of
elements? – their 'electronic classification'
-
For groups 1 to 2, and
'old' 3 to 0/'new' notation 13 to 18 (except He), all the elements
in the same vertical column have the same outer electron
configuration and therefore will be expected to have a very similar
chemistry.
-
For the d blocks of
Groups 3 to 12, using the 'new' group number notation, the vertical 'group'
connection of similar outer electron configuration is
consistent except for V/Nb, Fe/Ru, Co/Rh, Ni/Pd where the 3d/4s and
4d/5s pairs of levels are of very similar energy and small differences in outer
electron configuration occur.
-
What
is the electronic basis for the 'series of elements'? – their 'electronic classification'
-
The '1st
Transition Metals Series' from Sc to Zn, and other 'horizontal blocks' are sometimes called
a 'series' but they are better described as the '3d block' or '3d
series of elements' (and, 4d block, 4f block – filling of 4f
sub–shell etc.), but a horizontal row of elements, unlike the
vertical columns of the eight vertical groups.
-
What is the overall
electronic basis for blocks of
elements across the whole of the periodic table?
-
The s–block
consists of Groups 1 and 2 where the only outer electrons are in an s
sub–energy level orbital (no outer p electrons, 2 per period).
-
The p–block
corresponds to Groups 3 to 0 (old notation) or Groups 13 to 18 (new
notation) where the three p sub–energy level orbitals are being
filled (6 per period).
-
Starting with
period 4, where the first of the d sub–shells is low enough in energy
to be filled, there are ten elements 'inserted' between groups 2 and
3, the so–called d blocks of ten elements (the 1st block, the
3d block Sc–Zn is on Period 4).
-
Therefore Sc to Zn form
the head elements of Groups 3 to 12 using the 'new' group number
notation.
-
Similarly on period 5 there is a 4d block
where the 4d sub–shell level is filled.
-
So 10 d block elements per
period are now permitted\under the quantum number rules.
-
Starting with
cerium (Z=58, period 6), see in full table below, there is a further
insertion of fourteen elements where the seven f–orbital sub–shell is
being filled after the first of the d–block metals and similarly with
thorium (Z=90) in period 7 and these are known as the f blocks
(14 per period where permitted).
-
The
full Periodic Table is shown below without the
electron configurations, but including the old/new group number
notation.
Pd |
s–block
metals |
3d to 6d blocks including the Transition Metals
For Periods 4
to 7, note that the 1st (d1) and 10th (d10)
block metals are NOT true transition elements, the d2 to d9
elements are true transition metals |
p–block
metals and non-metals |
Gp1 |
Gp2 |
Gp3/13 |
Gp4/14 |
Gp5/15 |
Gp6/16 |
Gp7/17 |
Gp0/18 |
1 |
1H Note: (i) H does not readily
fit into any group, (ii) He not strictly a 'p' element but does
belong in Gp
0/18
|
2He |
2 |
3Li |
4Be |
Full IUPAC modern Periodic Table of Elements
ZSymbol, z = atomic or proton
number |
5B |
6C |
7N |
8O |
9F |
10Ne |
3 |
11Na |
12Mg |
*Gp3 |
*Gp4 |
*Gp5 |
*Gp6 |
*Gp7 |
*Gp8 |
*Gp9 |
*Gp10 |
*Gp11 |
*Gp12 |
13Al |
14Si |
15P |
16S |
17Cl |
18Ar |
4 |
19K |
20Ca |
21Sc |
22Ti |
23V |
24Cr |
25Mn |
26Fe |
27Co |
28Ni |
29Cu |
30Zn |
31Ga |
32Ge |
33As |
34Se |
35Br |
36Kr |
5 |
37Rb |
38Sr |
39Y |
40Zr |
41Nb |
42Mo |
43Tc |
44Ru |
45Rh |
46Pd |
47Ag |
48Cd |
49In |
50Sn |
51Sb |
52Te |
53I |
54Xe |
6 |
55Cs |
56Ba |
*57-71 |
72Hf |
73Ta |
74W |
75Re |
76Os |
77Ir |
78Pt |
79Au |
80Hg |
81Tl |
82Pb |
83Bi |
84Po |
85At |
86Rn |
7 |
87Fr |
88Ra |
*89-103 |
104Rf |
105Db |
106Sg |
107Bh |
108Hs |
109Mt |
110Ds |
111Rg |
112Cn |
113Nh |
114Fl |
115Mc |
116Lv |
117Ts |
118Og |
Group
1 Alkali Metals
Group 2 Alkaline Earth Metals
Group 7/17 Halogens
Group 0/18 Noble Gases
Take note of the four
points on the right |
|
*57La |
58Ce |
59Pr |
60Nd |
61Pm |
62Sm |
63Eu |
64Gd |
65Tb |
66Dy |
67Ho |
68Er |
69Tm |
70Yb |
71Lu |
|
*89Ac |
90Th |
91Pa |
92U |
93Np |
94Pu |
95Am |
96Cm |
97Bk |
98Cf |
99Es |
100Fm |
101Md |
102No |
103Lr |
*Horizontal insert in Period 6 of
Lanthanide
Metal Series (Lanthanides/Lanthanoids block) Z=57 to 71
includes 4f–block
series (elements 58–71). Element 57 is the start of the 5d
block, interrupted by the 14 4f block elements and then
continues with elements 72-80.
*Horizontal insert
in Period 7 of the Actinide Series of Metals (Actinides/Actinoids
block) Z=89–103
including the 5f–block
series (elements 90–103). Element 57 is the start of the 5d
block, interrupted by the 15 5f block elements and continues
with elements 72-80. |
-
Using 0 to
denote the Group number of the Noble Gases is historic i.e. when its valency was
considered zero since no compounds were known. However, from
1961 stable compounds of
xenon have been synthesised exhibiting up to the maximum possible expected valency of 8
e.g. in XeO4.
-
* 21Sc to 30Zn can be considered
as the top elements in the vertical Groups 3 to 12 (marked
as Gp3 -12.
-
*Therefore
Groups 3–7 and 0 can also be numbered as
Groups 13 to 18 (marked as
*13,
*14,
*15,
*16,
*17 and
*18) to fit in with the maximum number of vertical columns of elements
in periods 4 and 5 (18 elements per period).
-
I'm afraid
this can make things confusing, but there
it is, classification is still in progress and the notation Group 1 to 18
seems due to become universal.
-
Elements up to Z = 118 have
now been synthesised, if only a few atoms have been identified !
|
Notes:
The Noble Gases
have been referred to as Group 0 because they were believed not to
form compounds with other elements.
However, since 1961, many
compounds of xenon have been prepared including xenon(VIII) oxide,
XeO4, thus attaining the expected maximum possible
oxidation state based on the number of electrons in the outer shell, so Group 18 seems most appropriate to use these days
for advanced level chemistry courses.
The d block
elements are sometimes referred in terms of their vertical columns as
Groups 3 to 12, and the subsequent p–block group columns as Groups
13 to 18.
The s p d
f blocks are shown in the Periodic Table above.
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2.5
Electronic configuration of ions and oxidation states
How do you work out the
electron arrangement of ions? How do you work out the electron
configuration of ions?
In what order to you
remove electrons for positive ions? In what order do you add electrons
for negative ions?
SPECTROSCOPY, the
HYDROGEN SPECTRUM and IONISATION ENERGY PATTERNS
are now on a separate page
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and sub-indexes OR
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keywords and phrases: revision study notes for AQA Edexcel OCR Salters advanced
A level chemistry on how to use the rules on assigning electron
arrangements, and how the electron configuration notation is written out,
how to use
boxes to represent orbitals of electrons, how to explain the relationship between electron
configuration and the position of an element in the Periodic Table, using electron configurations to
show how the Periodic Table is worked out, explaining an element's position in the
Periodic Table and the electronic origin of the element's chemistry, which
is due to the
arrangement of its outer valency electrons. How to work out the electron
configuration of positive and negative ions from the electron configuration
of the element and explaining maximum and minimum oxidation sates from
the electron configuration of an element. How to work out the
electron configurations of the elements
Alphabetical order of the elements of the
periodic table symbol name atomic number: electron configuration of
Ac Actinium 89,
electron configuration of Al Aluminium 13,
electron configuration of Sb Antimony 51, electron configuration of Ar Argon 18,
electron configuration of As Arsenic 33, electron configuration of At Astatine 85,
electron configuration of Ba Barium 56, electron configuration of Be Beryllium 4,
electron configuration of Bi Bismuth 83, electron configuration of B Boron 5,
electron configuration of Br Bromine 35, electron configuration of Cd Cadmium 48,
electron configuration of Cs Caesium 55, electron configuration of Ca Calcium 20,
electron configuration of C Carbon 6, electron configuration of Ce Cerium 58, electron configuration of Cl Chlorine 17, electron configuration
of Cr Chromium 24, electron configuration of Co Cobalt 27, electron
configuration of Cu Copper 29,
electron configuration of Dy Dysprosium 66, electron configuration of Er Erbium 68,
electron configuration of Eu Europium 63, electron configuration of F Fluorine 9,
electron configuration of Fr Francium 87, electron configuration of Gd Gadolinium 64,
electron configuration of Ga Gallium 31, electron configuration of Ge Germanium 32,
electron configuration of Au Gold 79, electron configuration of Hf Hafnium 72,
electron configuration of He Helium 2, electron configuration of Ho Holmium 67,
electron configuration of H Hydrogen 1, electron configuration of In Indium 49,
electron configuration of I Iodine 53, electron configuration of Ir Iridium 77,
electron configuration of Fe Iron 26, electron configuration of Kr Krypton 36,
electron configuration of La Lanthanum 57, electron configuration of Pb Lead 82,
electron configuration of Li Lithium 3, electron configuration of Lu Lutetium 71,
electron configuration of Mg Magnesium 12,
electron configuration of Mn Manganese 25,
electron configuration of Hg
Mercury 80, electron configuration of Mo Molybdenum 42, electron
configuration of Nd Neodymium 60, electron configuration of Ne Neon 10,
electron configuration of Ni Nickel 28, electron configuration of Nb Niobium 41,
electron configuration of N Nitrogen 7, electron configuration of Os Osmium 76,
electron configuration of O Oxygen 8, electron configuration of Pd Palladium 46,
electron configuration of P Phosphorus 15, electron configuration of Pt Platinum 78,
electron configuration of Po Polonium 84, electron configuration of K Potassium 19,
electron configuration of Pr Praseodymium 59, electron configuration of Pm Promethium 61,
electron configuration of Pa Protactinium 91, electron configuration of Ra Radium 88,
electron configuration of Rn Radon 86, electron configuration of Re Rhenium 75,
electron configuration of Rh Rhodium 45, electron configuration of Rb Rubidium 37,
electron configuration of Ru Ruthenium 44, electron configuration of Sm Samarium 62,
electron configuration of Sc Scandium 21, electron configuration of Se Selenium 34,
electron configuration of Si Silicon 14, electron configuration of Ag Silver 47,
electron configuration of Na Sodium 11, electron configuration of Sr Strontium 38,
electron configuration of S Sulfur 16, electron configuration of Ta Tantalum 73,
electron configuration of Tc Technetium 43, electron configuration of Te Tellurium 52,
electron configuration of Tb Terbium 65, electron configuration of Tl Thallium 81,
electron configuration of Th Thorium 90, electron configuration of Tm Thulium 69,
electron configuration of Sn Tin 50, electron configuration of Ti Titanium 22,
electron configuration of W Tungsten 74, electron configuration of U Uranium 92,
electron configuration of V Vanadium 23, electron configuration of Xe Xenon 54,
electron configuration of Yb Ytterbium 70, electron configuration of Y Yttrium 39,
electron configuration of Zn Zinc 30, electron configuration of Zr Zirconium 40,
electron configuration of Np Neptunium 93,
electron configuration of
Pu Plutonium 94, electron configuration of
Am Americium 95, electron configuration of
Cm Curium 96, electron configuration of
Bk
Berkelium 97, electron configuration of
Cf Californium 98, electron configuration of
Es Einsteinium 99, electron configuration of
Fm Fermium 100, electron configuration of
Md Mendelevium 101, electron configuration of
No Nobelium 102, electron configuration of
Lr Lawrencium 103, electron configuration of
Rf Rutherfordium 104, electron configuration of
Db Dubnium 105, electron configuration of
Sg Seaborgium 106, electron configuration of
Bh Bohrium 107, electron configuration of
Hs Hassium 108, electron configuration of
Mt Meitnerium 109, electron configuration of
Ds Darmstadtium
110, electron configuration of
Rg Roentgenium 111, electron configuration of
Cn Copernicium 112, electron configuration of
Nh Nihonium 113, electron configuration of
Fl Flerovium 114, electron configuration of
Mc Moscovium 115, electron configuration of
Lv Livermorium 116, electron configuration of
Ts Tennessine 117, electron configuration of
Og Oganesson 118
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