It includes Lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs) and francium (Fr). They are known as s Block Elements as their last electron lies in the s-orbital. Table of Data for Group 1 Elements. Group 1: Properties of Alkali Metals This page discusses the trends in some atomic and physical properties of the Group 1 elements - lithium, sodium, potassium, rubidium and cesium. Group 1 elements are very reactive. The elements in group 1 are called the alkali metals.. Group 1 is on the left-hand side of the periodic table. Group 1 elements are known as Alkali Metals. Sections below cover the trends in atomic radius, first ionization energy, electronegativity, melting and boiling points, and density. The elements in group 1 are called the alkali metals. Chemical properties of Alkali Metals; Uses of Alkali Metals; Group 1 elements are known as Alkali Metals. The table below gives the name, atomic number, electronic configuration of the atom, the first and second ionisation energy, melting point, density and electronegativity, of the Group 1 elements (alkali metals). In chemistry, a group (also known as a family) is a column of elements in the periodic table of the chemical elements.There are 18 numbered groups in the periodic table; the f-block columns (between groups 3 and 4) are not numbered. and chemical properties. This group lies in the s block of the periodic table. chemical reactivity increasing down the group. You'll find more specific groups, like transition metals, rare earths, alkali metals, alkaline earth, halogens, and noble gasses. This means that the alkali metals all have similar chemical properties . The group 1 elements are all soft, reactive metals with low melting points. The alkali metals share similar physical. Hydrogen The Element H 2 is small and nonpolar so the H atoms can only attract each other Chemical properties of the group 1 elements Atoms of group 1 elements all have one electron in their outer shell. atomic and physical properties of the group 1 elements This page explores the trends in some atomic and physical properties of the Group 1 elements - lithium, sodium, potassium, rubidium and caesium. Progressing down group 1, the atomic radius increases due to the extra shell of electrons for each element. There are multiple ways of grouping the elements, but they are commonly divided into metals, semimetals (metalloids), and nonmetals. They are called s-block elements because their highest energy electrons appear in the s subshell. In this lesson we will learn what types of compounds the group forms, how these compounds are formed, and what these compounds are used for. Group 1 Elements Carefully inspect this data to find trends, or patterns, in the properties of group 1 elements. 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