They are the electrons involved in chemical bonds with other elements. x Compounds are white or colourless. Every element in the first column (group one) has one electron in its outer shell. Groups 3-12 are termed d-block elements. x Remember that the reactivity increases as you move down Group 2 (see ionisation energies) Physical properties: x All light metals. PubChem is working with IUPAC to help make information about the elements and the periodic table machine-readable. Group 2 Group 2 elements: Redox eactions: The Group 2 elements: x These are also called the alkaline earth metals as their hydroxides are alkaline. • Define allotropes and provide examples. Elements in Group 2 are called alkaline earth metals which is most similar about the alkaline earth metals. Usually, there is no need to store these elements in oil, unlike the group one elements. Included in the group two elements are Beryllium(Be), Magnesium(Mg), Calcium(Ca), Strontium(Sr), and Barium(Ba). The noble gasses have complete valence electron shells, so they act differently. Those outer electrons are also called valence electrons. The alkaline earth metals are six chemical elements in group 2 of the periodic table. For a metal, alkali earth metals tend to have low melting points and low densities. Group 2 contains soft, silver metals that are less metallic in character than the Group 1 elements. The elements in this group are also known as the chalcogens or the ore-forming elements because many elements can be extracted from the sulphide or oxide ores. They are transition metals because they have electrons in their d sublevels. Groups 3-11 are termed transition elements. Finally, IUPAC assigns collective names (lanthanoids and actinoids) and group numbering (1 to 18) and has investigated the membership of the group 3 elements. x They have reasonably high melting and boiling points. Group 2 elements generally react to form compounds in which the group 2 element has an oxidation state of +2, beryllium will also do this but it has a tendency to form covalent rather than ionic compounds. The group 16 elements of modern periodic table consist of 5 elements oxygen, sulphur, selenium, tellurium and polonium. elements in the same group are similar to each other; A section of the periodic table showing metals and non-metals. Seven valence electrons, so elements from this group typically exhibit a -1 oxidation state; Noble Gases . The group 2 elements are called the alkaline earth metals. The group number is an identifier used to describe the column of the standard periodic table in which the element appears. Introduction. Compare this with the coloured compounds of most transition metals. The transition metals are in groups 3 - 12. 186 Chapter 7 The Elements Section 7.2 Properties of p-Block Elements Objectives • Describe and compare properties of p-block elements. Groups 1-2 termed s-block elements. Unlike other groups, noble gasses are unreactive and have very low electronegativity or electron affinity. Although many characteristics are common throughout the group, the heavier metals such as Ca, Sr, Ba, and Ra are almost as reactive as the Group 1 Alkali Metals.All the elements in Group 2 have two electrons in their valence shells, giving them an oxidation state of +2. The elements in each group have the same number of electrons in the outer orbital. • Explain the importance to organisms of selected p-block elements. Groups 1-2 (except hydrogen) and 13-18 are termed main group elements. Alkali Earth Metals – Group 2 Elements. (3) Both group 1 and group 2 elements produce white ionic compounds. - The Group 2A elements are called alkaline earth metals. - The Group 1A elements are called alkali metals. - The nonmetals of Group 7A are called halogens. 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