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The elements of group VI are: oxygen, sulfur, selenium, tellurium and polonium. The oxygen and sulfur are nonmetals, the metalloids selenium and tellurium are semiconductors, while polonium is a metal. The main features are:

• all are solid at room temperature, except the oxygen and gaseous
• their atoms have six outer electrons, two on a type s orbital, and four out of orbit type p;
• have all the oxidation state of -2 when they bind to the less electronegative. When they bind to electronegative elements are the oxidation states +4 and +6, with the exception of oxygen, this being the second element after elttronegatività fluoride, has a positive oxidation state only when bound to fluorine (and in this case states can take +1 or +2);
• have two pairs of paired electrons, and thus can form two dative bonds with the role of donors; exception of oxygen, which, given its high electronegativity, it does not behave donor, acceptor, but, as an acceptor and can form a single dative bond;
• hydrogen forming compounds which are present in an atom and two hydrogen atoms of the element.

The elements of Group VI A, the group also Ext 16, are called chalcogens, the name has generally been derived from the Greek words chalcos "mineral" and-gen "formation", then the generator of minerals. The compounds, including sulfides, tellurides and the selenuri are also known as chalcogenides.

Oxygen was discovered in 1774 by Joseph Priestley, was known from ancient sulfur, selenium was discovered in 1818 by Jons Jacob Berzelius, tellurium in 1783 by von Mueller Reichestein, and polonium in 1898 by Pierre and Marie Curie.

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Sixth Seventh group

Group 7 of the periodic table consists of elements :
manganese (25)
technetium (43)
rhenium (75)
Bohrium (107)
these elements are classed in Group 7 because they all have 7 electrons in the valence shell.
Manganese is a metal, is the ' chemical element in the periodic table that has the symbol Mn and atomic number 25. Technetium
's chemical element of atomic number 43. Its symbol is Tc.

Rhenium 's chemical element of atomic number 75. Its symbol is The King

Bohr 's chemical element in the periodic table of elements, that has the symbol Bh and atomic number as the 107.

At room temperature, these elements are all solid, the color red for the atomic numbers indicates that the element is synthetic and not found in nature.

Halogens.

The halogens are a group of highly reactive elements, these tend to acquire an electron to achieve a stable electronic configuration. Fluoride is a colorless, highly reactive gas that is able to attack even the glass. Chlorine is a gas instead of the characteristic yellow-green pools. Bromine is a red volatile liquid scent irritant. Iodine is a dark purple solid that sublimates easily, leaving brown spots in the point where it is placed. These elements are strong oxidants are corrosive and in some cases respond to simple contact with a reducing agent.

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Periodic properties of elements in the periodic table

the early nineteenth century, scientists began to tidy up the increasing amount of information they had available. In 1869, these efforts culminated in the 'development of what today is called the periodic law, which states that certain physical and chemical properties to express themselves at regular intervals when the elements are arranged in order of increasing atomic number.
Frequency In chemistry, Law which states that the chemical and physical properties of the elements recur in a systematic way for atomic numbers increasing. In the periodic table the elements are distributed according to the external electronic configuration. In particular, see the table in vertical position (for groups), we find elements that have the same number of electrons nell'orbitale outside, and for this reason they have similar physical and chemical characteristics. Instead of moving in a horizontal direction, ie by reading the table for periods, we find that electrons in atoms present nell'orbitale outer rise, continuously, from 1 to 8. When a period is completed, it will start a new one, so that the configurations external electronic, and with it the chemical properties of elements change periodically repeating line by line (ie, period by period). Adjacent elements within a period, therefore, have an electronic structure that varies regularly through it and therefore are characterized by a parallel change of ownership. The most important periodic properties: atomic radius, ionization, electron affinity and electronegativity. More precisely, the atomic radius increases moving in the periodic table from top to bottom, ie in individual groups and decreases from left to right, ie in each period. The first ionization energy, the affinity Electronic el'elettronegatività increase from left to right in the periodic table, but decrease from top to bottom.