Group 17 elements - the halogens

The non-metallic elements exist as stable diatomic molecules F2, CI2, Bt2 and I2. 

They are volatile elements fluorine and chlorine are gases at room temperature, whereas bromine and iodine are a liquid and volatile solid respectively. Solid iodine sublimes when warmed. 

They are coloured the colours of the elements are shown in Table 12.7. 

Halogens combine directly with most metals to form ionic solids  

Some iodides have covalent character, however, because of the high polarizability of the iodide ion. 

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Why are the Group 17 elements, the halogens, the most reactive of the nonmetal elements ... 

Most metals react with the Group 17 elements, the halogens, to form either ionic or covalent compounds. For example. Group 1 metals react with halogens to form ionic compounds with the formula MX, where M is the metal and X is the halogen. Examples of this type of synthesis reaction include the reactions of sodium with chlorine and potassium with iodine. 

A family of elements is a numbered group from the periodic table, sometimes carrying a distinctive name. For example, group 17 is the halogen family. 

The first column of the periodic table, Group 1, contains elements that are soft, shiny solids. These alkali metals include lithium, sodium, potassium, mbidium, and cesium. At the other end of the table, fluorine, chlorine, bromine, iodine, and astatine appear in the next-to-last column. These are the halogens, or Group 17 elements. These four elements exist as diatomic molecules, so their formulas have the form X2 A sample of chlorine appears in Figure EV. Each alkali metal combines with any of the halogens in a 1 1 ratio to form a white crystalline solid. The general formula of these compounds s, AX, where A represents the alkali metal and X represents the halogen A X = N a C 1, LiBr, CsBr, KI, etc.). 

Halogens, the elements in Group 17 of the periodic table, have the largest electron affinities of all the elements, so halogen atoms (a n readily accept electrons to produce halide anions (a a. This allows halogens to react with many metals to form binary compounds, called halides, which contain metal cations and halide anions. Examples include NaCl (chloride anion), Cap2 (fluoride anion), AgBr (bromide anion), and KI (iodide anion). 

The halogens, the elements from Group 17 of the periodic table, provide an introduction to intermolecular forces. These elements exist as diatomic molecules F2, CI2, Bf2, and I2. The bonding patterns of the four halogens are identical. Each molecule contains two atoms held together by a single covalent bond that can be described by end-on overlap of valence p orbitals. 

Halogens The elements—fluorine, chlorine, bromine, iodine, and astatine—that make up Group 17 of the periodic table. 

A Only nitrogen, oxygen and the halogen (Group 17) elements. They are electronegative non-metals. 

The standard reduction potentials for the main species formed by the Group 17 elements in aqueous solution are given in Tables 6.16 and 6.17, for pH values 0 and 14, respectively. Irrespective of the pH of the solution, the halogen elements range from the extremely powerful F2 (which has the potential to oxidize water to dioxygen), through the powerful oxidants Cl2 and Br2, to 12, which is a relatively weak oxidant. 

In this section, the polyatomic cations of group 17 elements (halogen and interhalogen cations and polycations), cations and polycations of group 16 elements (O, S, Se, and... 

The BCNOs, along with the halogens of Group 17 and the noble gases of Group 18, are part of the periodic tables p block. The p block is named after the fact that electrons involved in chemical reactions in these elements come from the p orbital. 

The halogens are all poisonous nonmetals, but they are so reactive that they are rarely found alone in nature. Why do they pair up with other elements so easily and often The clue, once again, is in their periodic table position. As Group 17 elements, their valence electron shell has seven electrons—only one electron away from being a full or complete shell. Many elements have an electron they can spare or at least share to fill a halogens outer shell. Halogens have... 

Halogens The elements found in Group 17 of the periodic table. 

Halogens (group 17 elements) have an irritating odor. Unlike the metallic bonds between alkali metals, London forces between halogen molecules increase in strength further down the periodic table. 

Consequently all the halogens occur as halides. All these elements belong to the same group 17 of the periodic table which is indicated by the observed gradation in properties of these elements as is expected from their electronic configuration (Table). 

National Laboratory, in Upton, New York. Those experiments show that astatine is chemically similar to the other halogens above it in Group 17 of the periodic table. As chemists would expect, it acts more like a metal than iodine, the element just above it in the table. One of the few properties that have been determined for astatine is its melting point, found to be 576°F (302°C). Its boiling point is estimated to be about 639°F (337°C). 

CAS 7782-41-4. F. Nonmetallic halogen elementin group 17 of the periodic table. An 9, aw 18.99840, valence of 1, no other stable isotopes, the most electronegative element and most powerful oxidizing agent known. 

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