The table below is a summary of the key physical and atomic properties of the halogens. Data marked with question marks are either uncertain or are estimations partially based on periodic trends rather than observations. The halogens are located on the left of the noble gases on the periodic table. These five toxic, non-metallic elements make up Group 17 of the periodic table and consist of: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). The halogen elements are the six elements in Group 17 of the periodic table. Group 17 occupies the second column from the right in the periodic table and contains fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At), and tennessine (Ts). Astatine and tennessine are radioactive elements with very short half-lives and thus do not occur naturally.What are the major properties of the halogen elements?Halogen elements are very reactive. With sodium, they produce salts, of which table salt (sodium chloride, NaCl) is the most well known. Each halogen atom has seven valence electrons in its outermost electron shell. Therefore, when a halogen atom can receive an electron from an atom of a different element, the two atoms form a very stable compound, because the halogen atom’s outermost electron shell is then full.What are some uses of halogen elements?Chlorine is used to purify water. In addition, chlorine is part of table salt, sodium chloride, which is one of the most widely used chemical compounds. Fluorine is used in fluorides, which are added to water supplies to prevent tooth decay. Iodine is used as an antiseptic.Why are these elements called halogens?See full list on britannica.comProbably the most important generalization that can be made about the halogen elements is that they are all oxidizing agents; i.e., they raise the oxidation state, or oxidation number, of other elements—a property that used to be equated with combination with oxygen but that is now interpreted in terms of transfer of electrons from one atom to another. In oxidizing another element, a halogen is itself reduced; i.e., the oxidation number 0 of the free element is reduced to −1. The halogens can combine with other elements to form compounds known as halides—namely, fluorides, chlorides, bromides, iodides, and astatides. Many of the halides may be considered to be salts of the respective hydrogen halides, which are colourless gases at room temperature and atmospheric pressure and (except for hydrogen fluoride) form strong acids in aqueous solution. Indeed, the general term salt is derived from rock salt, or table salt (sodium chloride). The tendency of the halogen elements to form saltlike (i.e., highly ionic) compounds increases in the following order: astatine < iodine < bromine < chlorine < fluorine. Fluorides are usually more stable than the corresponding chlorides, bromides, or iodides. (Often astatine is omitted from general discussions of the halogens because less is known about it than about the other elements.)The oxidizing strength of the halogens increases in the same order—i.e., from astatine to fluorine. Therefore, of the halogen elements, elemental fluorine is prepared with the greatest difficulty and iodine with the least. As a class, the halogen elements are nonmetals, but astatine shows certain properties resembling those of the metals.Special offer for students! Check out our special academic rate and excel this spring semester!Learn MoreSee full list on britannica.comThe chemical behaviour of the halogen elements can be discussed most conveniently in terms of their position in the periodic table of the elements. In the periodic table the halogens make up Group 17 (according to the numbering system adopted by the International Union of Pure and Applied Chemistry), the group immediately preceding the noble gases. The halogen atoms carry seven valence electrons in their outermost electron shell. These seven outermost electrons are in two different kinds of orbitals, designated s (with two electrons) and p (with five). Potentially, a halogen atom could hold one more electron (in a p orbital), which would give the resulting halide ion the same arrangement (configuration) as that of the noble gas next to it in the periodic table. These electron configurations are exceptionally stable. This pronounced tendency of the halogens to acquire an additional electron renders them strong oxidizers.At room temperature and atmospheric pressure the halogen elements in their free states exist as diatomic molecules. In molecular fluorine (F2) the atoms are held together by a bond made from the union of a p orbital from each atom, with such a bond being classed as a sigma bond. It should be mentioned that the dissociation energy for fluorine (the energy necessary to break the F―F bond) is over 30 percent smaller than that of chlorine but is similar to that of iodine (I2). The weakness of the F―F single bond compared with chlorine can be ascribed to the small size of fluorine resulting in a decreased overlap of bonding orbitals and an increased repulsion of the nonbonding orbitals. In iodine, however, the p orbitals are more diffuse, which means the bond becomes weaker than in chlorine or bromine.See full list on britannica.comOct 10, 2020 · Learn about the six halogen elements: fluorine, chlorine, bromine, iodine, astatine, and tennessine. They are group 17 on the periodic table and have various properties, uses, and biological roles. · Learn about the properties, reactivity, and electronic configuration of the halogens, the most reactive nonmetals in group 17 of the periodic table. Find out how many valence electrons they have, where they are found on the table, and why they are called salt-producers. 3 days ago · Vertical columns on the periodictable are known as groups, and these groupings contain elements that share similar chemical properties. Group17, located toward the right side of the table, represents a highly reactive family of nonmetals that are uniquely important in chemistry and everyday life. Read about group17 elements, their configuration, physical and chemical properties, their uses, and group17periodictable. The halogens are located on the left of the noble gases on the periodic table. These five toxic, non-metallic elements make up Group 17 of the periodic table and consist of: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). The halogen elements are the six elements in Group 17 of the periodic table. Group 17 occupies the second column from the right in the periodic table and contains fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At), and tennessine (Ts). Astatine and tennessine are radioactive elements with very short half-lives and thus do not occur naturally.What are the major properties of the halogen elements?Halogen elements are very reactive. With sodium, they produce salts, of which table salt (sodium chloride, NaCl) is the most well known. Each halogen atom has seven valence electrons in its outermost electron shell. Therefore, when a halogen atom can receive an electron from an atom of a different element, the two atoms form a very stable compound, because the halogen atom’s outermost electron shell is then full.What are some uses of halogen elements?Chlorine is used to purify water. In addition, chlorine is part of table salt, sodium chloride, which is one of the most widely used chemical compounds. Fluorine is used in fluorides, which are added to water supplies to prevent tooth decay. Iodine is used as an antiseptic.Why are these elements called halogens?See full list on britannica.comProbably the most important generalization that can be made about the halogen elements is that they are all oxidizing agents; i.e., they raise the oxidation state, or oxidation number, of other elements—a property that used to be equated with combination with oxygen but that is now interpreted in terms of transfer of electrons from one atom to another. In oxidizing another element, a halogen is itself reduced; i.e., the oxidation number 0 of the free element is reduced to −1. The halogens can combine with other elements to form compounds known as halides—namely, fluorides, chlorides, bromides, iodides, and astatides. Many of the halides may be considered to be salts of the respective hydrogen halides, which are colourless gases at room temperature and atmospheric pressure and (except for hydrogen fluoride) form strong acids in aqueous solution. Indeed, the general term salt is derived from rock salt, or table salt (sodium chloride). The tendency of the halogen elements to form saltlike (i.e., highly ionic) compounds increases in the following order: astatine < iodine < bromine < chlorine < fluorine. Fluorides are usually more stable than the corresponding chlorides, bromides, or iodides. (Often astatine is omitted from general discussions of the halogens because less is known about it than about the other elements.)The oxidizing strength of the halogens increases in the same order—i.e., from astatine to fluorine. Therefore, of the halogen elements, elemental fluorine is prepared with the greatest difficulty and iodine with the least. As a class, the halogen elements are nonmetals, but astatine shows certain properties resembling those of the metals.Special offer for students! Check out our special academic rate and excel this spring semester!Learn MoreSee full list on britannica.comThe chemical behaviour of the halogen elements can be discussed most conveniently in terms of their position in the periodic table of the elements. In the periodic table the halogens make up Group 17 (according to the numbering system adopted by the International Union of Pure and Applied Chemistry), the group immediately preceding the noble gases. The halogen atoms carry seven valence electrons in their outermost electron shell. These seven outermost electrons are in two different kinds of orbitals, designated s (with two electrons) and p (with five). Potentially, a halogen atom could hold one more electron (in a p orbital), which would give the resulting halide ion the same arrangement (configuration) as that of the noble gas next to it in the periodic table. These electron configurations are exceptionally stable. This pronounced tendency of the halogens to acquire an additional electron renders them strong oxidizers.At room temperature and atmospheric pressure the halogen elements in their free states exist as diatomic molecules. In molecular fluorine (F2) the atoms are held together by a bond made from the union of a p orbital from each atom, with such a bond being classed as a sigma bond. It should be mentioned that the dissociation energy for fluorine (the energy necessary to break the F―F bond) is over 30 percent smaller than that of chlorine but is similar to that of iodine (I2). The weakness of the F―F single bond compared with chlorine can be ascribed to the small size of fluorine resulting in a decreased overlap of bonding orbitals and an increased repulsion of the nonbonding orbitals. In iodine, however, the p orbitals are more diffuse, which means the bond becomes weaker than in chlorine or bromine.See full list on britannica.comOct 10, 2020 · Learn about the six halogen elements: fluorine, chlorine, bromine, iodine, astatine, and tennessine. They are group 17 on the periodic table and have various properties, uses, and biological roles. · Learn about the properties, reactivity, and electronic configuration of the halogens, the most reactive nonmetals in group 17 of the periodic table. Find out how many valence electrons they have, where they are found on the table, and why they are called salt-producers. 3 days ago · Vertical columns on the periodictable are known as groups, and these groupings contain elements that share similar chemical properties. Group17, located toward the right side of the table, represents a highly reactive family of nonmetals that are uniquely important in chemistry and everyday life. Read about group17 elements, their configuration, physical and chemical properties, their uses, and group17periodictable. · Learn about the properties, reactivity, and electronic configuration of the halogens, the most reactive nonmetals in group 17 of the periodic table. Find out how many valence electrons they have, where they are found on the table, and why they are called salt-producers. 3 days ago · Vertical columns on the periodictable are known as groups, and these groupings contain elements that share similar chemical properties. Group17, located toward the right side of the table, represents a highly reactive family of nonmetals that are uniquely important in chemistry and everyday life. Read about group17 elements, their configuration, physical and chemical properties, their uses, and group17periodictable. · Learn about the six halogen elements: fluorine, chlorine, bromine, iodine, astatine, and tennessine. They are group 17 on the periodic table and have various properties, uses, and biological roles.
