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Draw the Electron Configuration for a Neutral Atom of Manganese

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Doc Brown's Advanced Level Chemistry - Inorganic Chemistry - Periodic Table Revision Notes

Part 2 Electronic structure, spectroscopy & ionisation energies,

e lectron configurations of the elements for Z = 1 to 58

Section 2.3 Electron configurations for elements of atomic number Z = 1 to 56

Parts 2.1 to 2.2 should be read and studied first !

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Part 2.3 uses the rules on assigning electron arrangements, and how the quantum level notation is written out, and using boxes to represent orbitals, as well as the usual written orbital notation, is given for elements Z = 1 to 56.

e.g. 26 Iron, Fe

1s22s22p63s23p63d64s2

[Ar]3d4s4p

Part 2.4 The relationship between electron configuration and the Periodic Table and uses the electron configurations to show how the Periodic Table arises, i.e. an element's position in the Periodic Table and hence its chemistry, is primarily determined by the arrangement of its outer valency electrons.

Part 2.5 shows how to work out the electron configuration of ions, (positive cations or negative anions formed by the loss or gain of valence electrons) and relating electron arrangements to the oxidation states exhibited by selected elements.

See also on other pages part ...

2.1 The electronic basis of the modern Periodic Table

2.2 The electronic structure of atoms (including s p d f subshells/orbitals/notation)

2.6 Spectroscopy and the hydrogen spectrum

2.7 Evidence of quantum levels from ionisation energies

2.8 Emission and absorption spectra of elements

 2.3 List of the Electronic Configuration of Elements 1 to 56 using the advanced 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 at Z = 20 Ca, and NOT 4p orbitals),

then at Z = 31 Ga you start to fill the 4p orbitals, and this is all you need pre-university!

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 Gp really, a bit unique!
2 Helium, He 1s2= [He] 1s very stable, unreactive, filled shell He, Gp 0/18 Noble Gas,
3 Lithium, Li 1s22s1 (simple notation: 2.1) [He]2s2p empty sub-shell Li, s�block, Gp1 Alkali Metal, v. reactive
4 Beryllium, Be 1s22s2 (2.2) [He]2s2p empty sub-shell Be, s�block, Gp2 Alkaline Earth Metal,
5 Boron, B 1s22s22p1 (2.3) [He]2s2p B, p�block, Gp3/13
6 Carbon, C 1s22s22p2 (2.4) [He]2s2p C, p�block, Gp4/14,
7 Nitrogen, N 1s22s22p3 (2.5) [He]2s2p N, p�block, Gp5/15,
8 Oxygen, O 1s22s22p4 (2.6) [He]2s2p O, p�block, Gp6/16,
9 Fluorine, F 1s22s22p5 (2.7) [He]2s2p F, p�block, Gp7/17 Halogen,
10 Neon, Ne 1s22s22p6= [Ne] (2.8) [He]2s2p very stable, unreactive, filled shells Ne, p�block, Gp 0/18 Noble Gas,
11 Sodium, Na 1s22s22p63s1 (2.8.1) [Ne]3s3p empty sub-shell Na, Gp1 Alkali Metal, v. reactive
12 Magnesium, Mg 1s22s22p63s2 (2.8.2) [Ne]3s3p empty sub-shell Mg, s�block, Gp2 Alkaline Earth Metal,
13 Aluminium, Al 1s22s22p63s23p1 (2.8.3) [Ne]3s3p Al, p�block, Gp3/13,
14 Silicon, Si 1s22s22p63s23p2 (2.8.4) [Ne]3s3p Si, p�block, Gp4/14,
15 Phosphorus, P 1s22s22p63s23p3 (2.8.5) [Ne]3s3p P, p�block, Gp5/15,
16 Sulfur, S 1s22s22p63s23p4 (2.8.6) [Ne]3s3p S, p�block, Gp6/16,
17 Chlorine, Cl 1s22s22p63s23p5 (2.8.7) [Ne]3s3p Cl, p�block, Gp7/17 Halogen,
18 Argon, Ar 1s22s22p63s23p6 = [Ar] (2.8.8) [Ne]3s3p very stable, unreactive, filled shells Ar, p�block, Gp 0/18 Noble Gas,
19 Potassium, K 1s22s22p63s23p64s1 (2.8.8.1) [Ar]3d4s4p K, s�block, Gp1 Alkali Metal, v. reactive
20 Calcium, Ca 1s22s22p63s23p64s2 (2.8.8.1) [Ar]3d4s4p Ca, s�block, Gp2 Alkaline Earth Metal,
21 Scandium, Sc 1s22s22p63s23p63d14s2 [Ar]3d4s4p Sc, 3d block, not true Transition Metal
22 Titanium, Ti 1s22s22p63s23p63d24s2 [Ar]3d4s4p Ti, 3d block, a true Transition Metal
23 Vanadium, V 1s22s22p63s23p63d34s2 [Ar]3d4s4p V, 3d block, a true Transition Metal
24 Chromium, Cr 1s22s22p63s23p63d54s1 [Ar]3d4s4p Cr, 3d block, a true Transition Metal
25 Manganese, Mn 1s22s22p63s23p63d54s2 [Ar]3d4s4p Mn, 3d block, a true Transition Metal
26 Iron, Fe 1s22s22p63s23p63d64s2 [Ar]3d4s4p Fe, 3d block, a true Transition Metal
27 Cobalt, Co 1s22s22p63s23p63d74s2 [Ar]3d4s4p Co, 3d block, a true Transition Metal
28 Nickel, Ni 1s22s22p63s23p63d84s2 [Ar]3d4s4p Ni, 3d block, a true Transition Metal
29 Copper, Cu 1s22s22p63s23p63d104s1 [Ar]3d4s4p Cu, 3d block, a true Transition Metal
30 Zinc, Zn 1s22s22p63s23p63d104s2 [Ar]3d4s4p Zn, 3d block, not true Transition Metal
31 Gallium, Ga [Ar]3d104s24p1 [Ar]3d4s4p Ga, p�block, Gp3/13,
32 Germanium, Ge [Ar]3d104s24p2 [Ar]3d4s4p Ge, p�block, Gp4/14,
33 Arsenic, As [Ar]3d104s24p3 [Ar]3d4s4p As, p�block, Gp5/15,
34 Selenium, Se [Ar]3d104s24p4 [Ar]3d4s4p Se, p�block, Gp6/16,
35 Bromine, Br [Ar]3d104s24p5 [Ar]3d4s4p Br, p�block, Gp7/17 Halogen,
36 Krypton, Kr [Ar]3d104s24p6 = [Kr] (2.8.18.8) [Ar]3d4s4p very stable, filled shells Kr, p�block, Gp 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]4d5s Y, 4d block, not true Transition Metal
40 Zirconium, Zr [Kr]4d25s2 [Kr]4d5s Zr, 4d block, a true Transition Metal
41 Niobium, Nb [Kr]4d45s1 [Kr]4d5s Nb, 4d block, a true Transition Metal
42 Molybdenum, Mo [Kr]4d55s1 [Kr]4d5s Mo, 4d block, a true Transition Metal
43 Technetium, Tc [Kr]4d55s2 [Kr]4d5s Tc, 4d block, a true Transition Metal
44 Ruthenium, Ru [Kr]4d75s1 [Kr]4d5s Ru, 4d block, a true Transition Metal
45 Rhodium, Rh [Kr]4d85s1 [Kr]4d5s Rh, 4d block, a true Transition Metal
46 Palladium, Pd [Kr]4d10 [Kr]4d5s Pd, 4d block, a true Transition Metal
47 Silver, Ag [Kr]4d105s1 [Kr]4d5s5p Ag, 4d block, a true Transition Metal
48 Cadmium, Cd [Kr]4d105s2 [Kr]4d5s5p Cd, 4d block, not true Transition Metal
49 Indium, In [Kr]4d105s25p1 [Kr]4d5s5p In, p�block, Gp3/13,
50 Tin, Sn [Kr]4d105s25p2 [Kr]4d5s5p Sn, p�block, Gp4/14,
51 Antimony, Sb [Kr]4d105s25p3 [Kr]4d5s5p Sb, p�block, Gp5/14,
52 Tellurium, Te [Kr]4d105s25p4 [Kr]4d5s5p Te, p�block, Gp6/16,
53 Iodine, I [Kr]4d105s25p5 [Kr]4d5s5p I, p�block, Gp7/17 Halogen,
54 Xenon, Xe [Kr]4d105s25p6 = [Xe] [Kr]4d5s5p very stable, filled shells Xe, p�block, Gp 0/18 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]5d6s 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.

electron spin box diagram for carbon electron spin box diagram for neon electron spin box diagram for silicon

electron spin box diagram for argon electron spin box diagram for calcium electron spin box diagram for vanadium

electron spin box diagram for the elements s p d f orbital quantum levels

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]3d54s 1 and not [Ar]3d44s2

and Cu is[Ar]3d104s 1 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 Gp0/18
1

1 H 1s1

2 He 1s2
2 3 Li [He]2s 1 4 Be [He]2s2 The e lectronic structure of Elements 1 to 56, ZSymbol, Z = atomic or proton number = total electrons in neutral atom, [He] = 1s2, [Ne] = 1s22s22p6, [Ar] = 1s22s22p63s23p6, [Kr] = 1s22s22p63s23p63d104s24p 6

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).

5 B [He]2s22p1 6 C [He]2s22p2 7 N [He]2s22p3 8 O [He]2s22p4 9 F [He]2s22p5 10 Ne [He]2s22p6
3 11 Na [Ne]3s1 12 Mg [Ne]3s2 13 Al [Ne]3s23p1 14 Si [Ne]3s23p2 15 P [Ne]3s23p3 16 S [Ne]3s23p4 17 Cl [Ne]3s23p5 18 Ar [Ne]3s23p6
4 19 K [Ar]4s1 20 Ca [Ar]4s2 21 Sc [Ar] 3d14s2 22 Ti [Ar] 3d24s2 23 V [Ar] 3d34s2 24 Cr [Ar] 3d54s1 25 Mn [Ar] 3d54s2 26 Fe [Ar] 3d64s2 27 Co [Ar] 3d74s2 28 Ni [Ar] 3d84s2 29 Cu [Ar] 3d104s1 30 Zn [Ar] 3d104s2 31 Ga [Ar] 3d104s24p1 32 Ge [Ar] 3d104s24p2 33 As [Ar] 3d104s24p3 34 Se [Ar] 3d104s24p4 35 Br [Ar] 3d104s24p5 36 Kr [Ar] 3d104s24p6
5 37 Rb [Kr]5s 1 38 Sr [Kr]5s2 39 Y [Kr] 4d15s 2 40 Zr [Kr] 4d25s2 41 Nb [Kr] 4d45s1 42 Mo [Kr] 4d55s1 43 Tc [Kr] 4d55s2 44 Ru [Kr] 4d75s1 45 Rh [Kr] 4d85s1 46 Pd [Kr] 4d10 47 Ag [Kr] 4d105s1 48 Cd [Kr] 4d105s2 49 In [Kr] 4d105s25p1 50 Sn [Kr] 4d105s25p2 51 Sb [Kr] 4d105s25p3 52 Te [Kr] 4d105s25p4 53 I [Kr] 4d105s25p5 54 Xe [Kr] 4d105s25p6
6 55 Cs [Xe]6s 1 56 Ba [Xe]6s 2 4f�block (14) and 5d�block (10), total of 32 elements in period 6 including the Lanthanide Series of Metals. 81 Tl [Xe] 4f145d106s26p1 82 Pb [Xe] 4f145d106s26p2 83 Bi [Xe] 4f145d106s26p3 84 Po [Xe] 4f145d106s26p4 85 At [Xe] 4f145d106s26p 5 86 Rn [Xe] 4f145d106s26p 6
7 87 Fr [Rn]7s1 88 Ra [Rn]7s 2 5f�block and 6d�block including the Actinide Series of Metals in period 7, see full table below 113 Nh [Rn] 5f146d107s27p1 114 Fl [Rn] 5f146d107s27p2 115 Mc [Rn] 5f146d107s27p3 116 Lv [Rn] 5f146d107s27p4 117 Ts [Rn] 5f146d107s27p5 118 Og [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

    • When the outer s and p quantum levels (and any completely filled inner orbital quantum levels eg 3d or 4f) you get a particularly stable element with minimal chemical reactivity ie you get a Noble Gas element [simple electron notation in ()]

      • Z = 2, helium, 1s2= [He] (2)

      • Z = 10, neon, 1s22s22p6= [Ne] (2.8)

      • Z = 18, argon, 1s22s22p63s23p6 = [Ar] (2.8.8)

      • Z = 36, krypton, [Ar]3d104s24p6 = [Kr] (2.8.18.8)

      • Z = 54, xenon, [Kr]4d105s25p6 = [Xe]

      • Z = 86, radon, [Xe]5d106s26p6 =[Rn]

  • 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.

      • This gives the electronic basis for Mendeleev's brilliant conception of the periodic table, ie laying out all the elements in order of 'atomic weight' and lining them up to give vertical columns of chemically and physically similar elements.

    • 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.

      • Never�the�less these pairs of elements show strong similarities as part of the justification for denoting the Transition Metals plus Groups 4 to 0 as Groups 3 to 18.

  • 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.

      • Why is 'block' better than 'series'?

        • The reference to the electronic structure is very important, the word series is a bit vague!

        • Technically, scandium (Sc, Z = 21) and zinc (Zn, Z = 30), are NOT true transition metals BUT they are true 3d block elements!

          • See Detailed Advanced Level Transition Metal Notes

  • 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).

      • Technically, the same applies to hydrogen and helium in period 1.

    • 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 Z Symbol, 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) 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) 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.

  1. 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.

  2. * 21Sc to 30Zn can be considered as the top elements in the vertical Groups 3 to 12 (marked as Gp3 -12.

  3. * 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).

  4. 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.

  5. Elements up to Z = 118 have now been synthesised, if only a few atoms have been identified !

  • Notes:

    1. 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, so Group 18 seems most appropriate to use these days for advanced level courses.

    2. The d block elements are sometimes referred in terms of vertical columns as Groups 3 to 12, and the subsequent p�block group columns as Groups 13 to 18.

      • Whether this will become standard at pre�university level, I don't know? but I think its a bit confusing for school level chemistry below pre�university courses like UK GCSE or US grades 6�10.

  • 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?

  • The electron configuration of ions :

    • Beware in quoting the configurations for simple ions where, although the order of removal is basically the reverse of the order for filling the energy levels, there is one important exception you should know.

      • For d/transition blocks/series the 4s electrons are 'removed' before the 3d electrons and similarly the 5s electrons are 'removed' before the 4d electrons.

    • Positive ions (cations) are formed by electron loss and the order of removal is the reverse of the order the full electron configuration is written out e.g.

      • sodium atom Na = 1s22s22p63s1 , sodium ion Na+ = 1s22s22p6  = [Ne]

      • calcium atom is Ca = 1s22s22p63s23p64s2, calcium ion Ca2+ = 1s22s22p63s23p6 = [Ar]

      • iron atom Fe =  [Ar]3d64s2, iron(II) ion Fe2+ = [Ar]3d6 , and iron(III) ion Fe3+ = [Ar]3d5

      • germanium atom Ge = [Ar]3d104s24p2, germanium(II) ion Ge2+ = [Ar]3d104s2 , germanium(IV) ion Ge4+ = [Ar]3d10

    • Negative ions (anions) are formed by electron gain and the filling order rule is continued e.g.

      • chlorine Cl = [Ne]3s23p5, chloride ion Cl� = [Ne]3s23p6 = [Ar]

      • oxygen: O = [He]2s22p4, oxide ion O2� = [He]2s22p6 = [Ne]

      • phosphorus: P = [Ne]3s23p3, phosphide ion P3� = [Ne]3s23p3 = [Ar]

      • Note the maximum negative oxidation state is governed by the number of electrons needed to complete a noble gas structure in the covalent or ionic bonding situation.

  • Oxidation state and electronic structure :

    • For more details see notes on oxidation state and redox reactions .

    • The maximum oxidation state is often, but not always, limited by an inner full noble gas structure with or without a full d/f sub�shell.

    • The maximum oxidation state from Group 1 Alkali Metals (+1) to Group 0/18 Noble Gases (+8) is numerically equal to the number of outer electrons, i.e. those beyond an inner noble gas core or inner noble gas plus a full d/f sub�shell e.g.

      • The maximum oxidation states for Groups 1 to 0 in old notation (now s-block Groups 1-2 and p-block 13-18)

      • Group 1 , outer electron configuration s 1 , eg sodium is +1 in sodium chloride NaCl

      • Group 2 , outer electron configuration s 2 , eg magnesium is +2 in magnesium oxide MgO

      • Group 3 (13) , outer electron configuration s2p 1 , eg aluminium is +3 in aluminium fluoride AlF3

      • Group 4 (14) , outer electron configuration s2p 2 , eg silicon is +4 in silicon dioxide SiO2

      • Group 5 (15) , outer electron configuration s2p 3 , eg phosphorus is +5 in the phosphate(V) ion PO4 3�

      • Group 6 (16) , outer electron configuration s2p 4 , eg sulfur is +6 in sulfur trioxide SO3

      • Group 7 (17) , outer electron configuration s2p 5 , eg chlorine is +7 in the chlorate(VII) ion ClO4 �

      • Group 0 (18) , outer electron configuration s2p 6 (except He , just s 2 ), eg xenon is +8 in xenon(VIII) oxide XeO4

        • The maximum oxidation state pattern for the d blocks is a bit more complicated and the trend goes through a maximum e.g.

          • the maximum observed oxidation states for the 3d block and transition metal series :

          • Sc (+3), Ti (+4), V (+5), Cr (+6), Mn (+7), Fe (+3, maybe +6?), Co (+3), Ni (+3), Cu (+3), Zn (+2)

          • The maximum oxidation state from scandium to manganese (Sc-Mn) equates to the presence of 4 to 7 3d and 4s electrons beyond the inner noble gas core of [Ar], the 'theoretical' ion would have a 3d0 structure.

    • Atoms or ions with the same electron configuration are referred to as isoelectronic eg

      • Na+, Mg2+, Al3+ and Ne are all 1s22s22p6 and you might say the three ions are isoelectronic with neon.

      • N3-, O2- and F- are also all isoelectronic with neon.

      • Zn2+ and  Ge4+ are both [Ar]3d10

SPECTROSCOPY, the HYDROGEN SPECTRUM and IONISATION ENERGY PATTERNS

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