Compare the elements of oxygen or halogen family
Answers
Answer:
Comparing the elements of Oxygen family are listed below:-
Explanation:
Elements belonging to group 16 of the periodic table are described by electron configurations in which six electrons occupy the outer shell. An atom with such an electron structure is thought to become a solid shell of eight electrons by adding two more, creating a double negative charge ion. This tendency to form negatively charged ions, typically for non-metallic elements, is quantified by the properties of electronegativity (assuming a partial negative charge present in a covalent combination) and electron affinity (the ability of a neutral atom around an electron to absorb, forming a negative ion). Both of these properties decrease in intensity as the atomic number and mass of the elements continue in column 16 of the periodic table. Oxygen, with the exception of fluorine, has the highest electronegativity and electron affinity of each element; the values of these properties then decrease significantly for the remaining members of the group to the extent that tellurium and polonium are for the most part considered to be metallic in nature, more likely to disappear than the electrons gain in forming the composition. As with all groups of tables, the lightest element - the element with the smallest atomic number - has too many or exaggerated properties. Due to its small atom size, small number of electrons under its shell and large number of protons in the nucleus, oxygen has properties very different from those of sulfur and the remaining chalcogenes due to the radius of the atom. These elements work in a reasonably predictable and present way.
Although polonium exhibits an oxidation state of -2 to form some binary MPo-type compounds (where M is a metal), heavier chalcogenes do not easily form a negative state, preferring positive states such as +2 and +4. All elements of the group except oxygen can claim positive oxidation states with the same predominant values, but the highest value, +6, is less strong for most beetles. Once this state is reached, there is a strong driving force for the atom to return to a lower state, usually in elemental form. This tendency makes compounds with Se (VI) and Te (VI) more oxidizing agents than compounds with S (VI). In contrast, sulfides, selenides and tellurides, where the oxidation state is -2, are strong reducing agents, easily oxidizing to free elements.
Neither sulfur nor selenium, let alone oxygen, form pure ionic compounds in the non-metallic atom. Tellurium and polonium form some relatively ionic compounds; Telurium (IV) sulfate, Te (SO4) 2, and polonium (II) sulfate, PoSO4, are examples. Another characteristic of Group 16 elements, which is similar to the trends usually reported in the columns of the Periodic Table, is the increasing strength of molecules of composition X (OH) n with increasing size of central atom X. There is no composition of HO-O-OH in which central oxygen oxidation state, i.e. the state to which it resists. The same sulfur compound HO-S-OH, although not known in its pure state, has some strong sources in the form of metal salts, sulfoxylates. The much larger hydroxylated sulfur compound, S (OH) 4 and S (OH) 6, also does not exist, not because of the resistance of sulfur to the positive oxidation state, but because of the high charge densities S (IV) and S. (VI) states (a large number of positive small-diameter charges), which rejects electropositive hydrogen atoms, and the bond associated with the covalent bonding of six oxygen atoms to sulfur, which promotes water loss
As the size of the chalcogen atom increases, the strength of the hydroxylated compounds increases: there may be an orthotelluric acid compound, Te (OH) 6.
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