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