A | B | C | D | E | F | G | H | CH | I | J | K | L | M | N | O | P | Q | R | S | T | U | V | W | X | Y | Z | 0 | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9
| Group 12 in the periodic table | |||||||||
|---|---|---|---|---|---|---|---|---|---|
| |||||||||
| ↓ Period | |||||||||
| 4 |  30 Transition metal | ||||||||
| 5 |  48 Transition metal | ||||||||
| 6 |  80 Transition metal | ||||||||
| 7 | Copernicium (Cn) 112 transition metal | ||||||||
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Legend
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Group 12, by modern IUPAC numbering,[1] is a group of chemical elements in the periodic table. It includes zinc (Zn), cadmium (Cd), mercury (Hg),[2][3][4] and copernicium (Cn).[5] Formerly this group was named IIB (pronounced as "group two B", as the "II" is a Roman numeral) by CAS and old IUPAC system.[note 1]
The three group 12 elements that occur naturally are zinc, cadmium and mercury. They are all widely used in electric and electronic applications, as well as in various alloys. The first two members of the group share similar properties as they are solid metals under standard conditions. Mercury is the only metal that is known to be a liquid at room temperature – as copernicium's boiling point has not yet been measured accurately enough,[note 2] it is not yet known whether it is a liquid or a gas under standard conditions. While zinc is very important in the biochemistry of living organisms, cadmium and mercury are both highly toxic. As copernicium does not occur in nature, it has to be synthesized in the laboratory.
Physical and atomic properties
Like other groups of the periodic table, the members of group 12 show patterns in its electron configuration, especially the outermost shells, which result in trends in their chemical behavior:
| Z | Element | No. of electrons/shell |
|---|---|---|
| 30 | zinc | 2, 8, 18, 2 |
| 48 | cadmium | 2, 8, 18, 18, 2 |
| 80 | mercury | 2, 8, 18, 32, 18, 2 |
| 112 | copernicium | 2, 8, 18, 32, 32, 18, 2 (predicted) |
The group 12 elements are all soft, diamagnetic, divalent metals. They have the lowest melting points among all transition metals.[8] Zinc is bluish-white and lustrous,[9] though most common commercial grades of the metal have a dull finish.[10] Zinc is also referred to in nonscientific contexts as spelter.[11] Cadmium is soft, malleable, ductile, and with a bluish-white color. Mercury is a liquid, heavy, silvery-white metal. It is the only common liquid metal at ordinary temperatures, and as compared to other metals, it is a poor conductor of heat, but a fair conductor of electricity.[12]
The table below is a summary of the key physical properties of the group 12 elements. The data for copernicium is based on relativistic density-functional theory simulations.[13]
| Name | Zinc | Cadmium | Mercury | Copernicium |
|---|---|---|---|---|
| Melting point | 693 K (420 °C) | 594 K (321 °C) | 234 K (−39 °C) | 283±11 K[13] (10 °C) |
| Boiling point | 1180 K (907 °C) | 1040 K (767 °C) | 630 K (357 °C) | 340±10 K[13] (60 °C) |
| Density | 7.14 g·cm−3 | 8.65 g·cm−3 | 13.534 g·cm−3 | 14.0 g·cm−3 [13] |
| Appearance | silvery bluish-gray | silver-gray | silvery | ? |
| Atomic radius | 135 pm | 155 pm | 150 pm | ? 147 pm |
Zinc is somewhat less dense than iron and has a hexagonal crystal structure.[14] The metal is hard and brittle at most temperatures but becomes malleable between 100 and 150 °C (212 and 302 °F).[9][10] Above 210 °C (410 °F), the metal becomes brittle again and can be pulverized by beating.[15] Zinc is a fair conductor of electricity.[9] For a metal, zinc has relatively low melting (419.5 °C, 787.1 °F) and boiling points (907 °C, 1,665 °F).[8] Cadmium is similar in many respects to zinc but forms complex compounds.[16] Unlike other metals, cadmium is resistant to corrosion and as a result it is used as a protective layer when deposited on other metals. As a bulk metal, cadmium is insoluble in water and is not flammable; however, in its powdered form it may burn and release toxic fumes.[17] Mercury has an exceptionally low melting temperature for a d-block metal. A complete explanation of this fact requires a deep excursion into quantum physics, but it can be summarized as follows: mercury has a unique electronic configuration where electrons fill up all the available 1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d, 4f, 5s, 5p, 5d and 6s subshells. As such configuration strongly resists removal of an electron, mercury behaves similarly to noble gas elements, which form weak bonds and thus easily melting solids. The stability of the 6s shell is due to the presence of a filled 4f shell. An f shell poorly screens the nuclear charge that increases the attractive Coulomb interaction of the 6s shell and the nucleus (see lanthanide contraction). The absence of a filled inner f shell is the reason for the somewhat higher melting temperature of cadmium and zinc, although both these metals still melt easily and, in addition, have unusually low boiling points. Gold has atoms with one less 6s electron than mercury. Those electrons are more easily removed and are shared between the gold atoms forming relatively strong metallic bonds.[18][19]
Zinc, cadmium and mercury form a large range of alloys. Among the zinc containing ones, brass is an alloy of zinc and copper. Other metals long known to form binary alloys with zinc are aluminium, antimony, bismuth, gold, iron, lead, mercury, silver, tin, magnesium, cobalt, nickel, tellurium and sodium.[11] While neither zinc nor zirconium are ferromagnetic, their alloy ZrZn
2 exhibits ferromagnetism below 35 K.[9] Cadmium is used in many kinds of solder and bearing alloys, due to a low coefficient of friction and fatigue resistance.[20] It is also found in some of the lowest-melting alloys, such as Wood's metal.[21] Because it is a liquid, mercury dissolves other metals and the alloys that are formed are called amalgams. For example, such amalgams are known with gold, zinc, sodium, and many other metals. Because iron is an exception, iron flasks have been traditionally used to trade mercury. Other metals that do not form amalgams with mercury include tantalum, tungsten and platinum. Sodium amalgam is a common reducing agent in organic synthesis, and is also used in high-pressure sodium lamps. Mercury readily combines with aluminium to form a mercury-aluminium amalgam when the two pure metals come into contact. Since the amalgam reacts with air to give aluminium oxide, small amounts of mercury corrode aluminium. For this reason, mercury is not allowed aboard an aircraft under most circumstances because of the risk of it forming an amalgam with exposed aluminium parts in the aircraft.[22]
Chemistry
Most of the chemistry has been observed only for the first three members of the group 12. The chemistry of copernicium is not well established and therefore the rest of the section deals only with zinc, cadmium and mercury.
Periodic trends
All elements in this group are metals. The similarity of the metallic radii of cadmium and mercury is an effect of the lanthanide contraction. So, the trend in this group is unlike the trend in group 2, the alkaline earths, where metallic radius increases smoothly from top to bottom of the group. All three metals have relatively low melting and boiling points, indicating that the metallic bond is relatively weak, with relatively little overlap between the valence band and the conduction band.[23] Thus, zinc is close to the boundary between metallic and metalloid elements, which is usually placed between gallium and germanium, though gallium participates in semi-conductors such as gallium arsenide.
Zinc and cadmium are electropositive while mercury is not.[23] As a result, zinc and cadmium metal are good reducing agents. The elements of group 12 have an oxidation state of +2 in which the ions have the rather stable d10 electronic configuration, with a full sub-shell. However, mercury can easily be reduced to the +1 oxidation state; usually, as in the ion Hg2+
2, two mercury(I) ions come together to form a metal-metal bond and a diamagnetic species.[24] Cadmium can also form species such as 4− in which the metal's oxidation state is +1. Just as with mercury, the formation of a metal-metal bond results in a diamagnetic compound in which there are no unpaired electrons; thus, making the species very reactive. Zinc(I) is known mostly in the gas phase, in such compounds as linear Zn2Cl2, analogous to calomel. In the solid phase, the rather exotic compound decamethyldizincocene (Cp*Zn–ZnCp*) is known.
Classification
The elements in group 12 are usually considered to be d-block elements, but not transition elements as the d-shell is full. Some authors classify these elements as main-group elements because the valence electrons are in ns2 orbitals. Nevertheless, they share many characteristics with the neighboring group 11 elements on the periodic table, which are almost universally considered to be transition elements. For example, zinc shares many characteristics with the neighboring transition metal, copper. Zinc complexes merit inclusion in the Irving-Williams series as zinc forms many complexes with the same stoichiometry as complexes of copper(II), albeit with smaller stability constants.[25] There is little similarity between cadmium and silver as compounds of silver(II) are rare and those that do exist are very strong oxidizing agents. Likewise the common oxidation state for gold is +3, which precludes there being much common chemistry between mercury and gold, though there are similarities between mercury(I) and gold(I) such as the formation of linear dicyano complexes, −. According to IUPAC's definition of transition metal as an element whose atom has an incomplete d sub-shell, or which can give rise to cations with an incomplete d sub-shell,[26] zinc and cadmium are not transition metals, while mercury is. This is because only mercury is known to have a compound where its oxidation state is higher than +2, in mercury(IV) fluoride (though its existence is disputed, as later experiments trying to confirm its synthesis could not find evidence of HgF4).[27][28] However, this classification is based on one highly atypical compound seen at non-equilibrium conditions and is at odds to mercury's more typical chemistry, and Jensen has suggested that it would be better to regard mercury as not being a transition metal.[29]
Relationship with the alkaline earth metals
Although group 12 lies in the d-block of the modern 18-column periodic table, the d electrons of zinc, cadmium, and (almost always) mercury behave as core electrons and do not take part in bonding. This behavior is similar to that of the main-group elements, but is in stark contrast to that of the neighboring group 11 elements (copper, silver, and gold), which also have filled d-subshells in their ground-state electron configuration but behave chemically as transition metals. For example, the bonding in chromium(II) sulfide (CrS) involves mainly the 3d electrons; that in iron(II) sulfide (FeS) involves both the 3d and 4s electrons; but that of zinc sulfide (ZnS) involves only the 4s electrons and the 3d electrons behave as core electrons. Indeed, useful comparison can be made between their properties and the first two members of group 2, beryllium and magnesium, and in earlier short-form periodic table layouts, this relationship is illustrated more clearly. For instance, zinc and cadmium are similar to beryllium and magnesium in their atomic radii, ionic radii, electronegativities, and also in the structure of their binary compounds and their ability to form complex ions with many nitrogen and oxygen ligands, such as complex hydrides and amines. However, beryllium and magnesium are small atoms, unlike the heavier alkaline earth metals and like the group 12 elements (which have a greater nuclear charge but the same number of valence electrons), and the periodic trends down group 2 from beryllium to radium (similar to that of the alkali metals) are not as smooth when going down from beryllium to mercury (which is more similar to that of the p-block main groups) due to the d-block and lanthanide contractions. It is also the d-block and lanthanide contractions that give mercury many of its distinctive properties.[29]
| Name | Beryllium | Magnesium | Calcium | Strontium | Barium | Radium |
|---|---|---|---|---|---|---|
| Valence electron configuration | 2s2 | 3s2 | 4s2 | 5s2 | 6s2 | 7s2 |
| Core electron configuration | [He] | [Ne] | [Ar] | [Kr] | [Xe] | [Rn] |
| Oxidation states[note 3] | +2, +1 | +2, +1 | +2, +1 | +2, +1 | +2 | +2 |
| Melting point | 1560 K (1287 °C) | 923 K (650 °C) | 1115 K (842 °C) | 1050 K (777 °C) | 1000 K (727 °C) | 973 K (700 °C) |
| Boiling point | 2742 K (2469 °C) | 1363 K (1090 °C) | 1757 K (1484 °C) | 1655 K (1382 °C) | 2170 K (1897 °C) | 2010 K (1737 °C) |
| Appearance | white-gray metallic | shiny gray metallic | dull silver-gray | silvery white metallic | silvery gray | silvery white metallic |
| Density | 1.85 g·cm−3 | 1.738 g·cm−3 | 1.55 g·cm−3 | 2.64 g·cm−3 | 3.51 g·cm−3 | 5.5 g·cm−3 |
| Pauling electronegativity | 1.57 | 1.31 | 1.00 | 0.95 | 0.89 | 0.9 |
| Atomic radius | 105 pm | 150 pm | 180 pm | 200 pm | 215 pm | 215 pm |
| Crystal ionic radius | 59 pm | 86 pm | 114 pm | 132 pm | 149 pm | 162 pm |
| Flame test color | white[29] | brilliant white[30] | brick-red[30] | crimson[30] | apple green[30] | crimson red[note 4] |
| Organometallic chemistry | good | good | poor | very poor | very poor | extremely poor |
| Hydroxide | amphoteric | basic | basic | strongly basic | strongly basic | strongly basic |
| Oxide | amphoteric | strongly basic | strongly basic | strongly basic | strongly basic | strongly basic |
| Name | Beryllium | Magnesium | Zinc | Cadmium | Mercury | Copernicium |
| Valence electron configuration | 2s2 | 3s2 | 4s2 | 5s2 | 6s2 | ? 7s2 |