Halogens are the compounds found in group 17 of the periodic table. Group 7 elements form salts when they react with metals. Reaction with Halogens. They are all incredibly electronegative, meaning that they are very willing to take electrons from other atoms. In this article, we will explain the electronic configurations, ionization enthalpy, hydration enthalpy and atomic, ionic radii and other physical and chemical properties of the group one alkali metals. Reactivity of alkali metals and halogens Alkali Metals: •are placed in group 1, • can be cut with a knife. The alkali metals have the silver-like lustre, high ductility, and excellent conductivity of electricity and heat generally associated with metals. They are pretty much opposites. Alkali metals belong to the s-block elements occupying the leftmost side of the periodic table.Alkali metals readily lose electrons, making them count among the most reactive elements on earth. Properties of Alkali Metals. Shows both the reactions and properties of some chemical elements. 3. Alkali metals react with elements of the halogen group (Group 17 of the periodic table) to form halides. Use the periodic table to identify and explain the properties of chemical families, includong alkali metals, alkaline earth metals, halogens, noble gases, and transition metals. Furthermore, an alkali metal's valence electron is relatively far away from the nucleus, making it … The alkali metals are on the far left side of the periodic table, thus they have the lowest ionization energy. They have one outermost shell electron. Examples of halogens are Fluorine (F), Chlorine (Cl), Bromine (Br) and Iodine (I). Properties and uses of the halogens. Lithium is the lightest metallic element. Hydrogen shares some properties of alkali metals and halogen, yet it is neither. Examples of alkali metals: lithium (Li), sodium (Na), potassium (K), rubidium (Rb), ceasium (Cs), and francium (Fr). The term ‘halogen’ means 'salt former'. These hydrides have strong reducing properties. Halogens: •are placed in group 17, • react vigorously with metals. This can be explained by the fact that they all have one valence electron, thus they "want" to get rid of it. Alkali metals, particularly sodium, are important in commercial use and chemical synthesis. The interhalogens react like their component halides; halogen fluorides, for example, are stronger oxidizing agents than are halogen chlorides. The alkali metals have low melting points, ranging from a high of 179 °C (354 °F) for lithium to a low of 28.5 °C (83.3 °F) for cesium. The stability of the hydrides thus formed, reduces with the increase in the atomic numbers of alkali metals. Alkali metals have been studied since 1807, when Sir Humphry Davy explored the electrical properties of potassium and sodium. Terms in this set (5) Alkali Metals Except lithium iodide, all other halides are ionic in nature. 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