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solubility of group 2 nitrates
solubility of group 2 sulphates explanation
uses of group 2 metals and their compounds
group 3 elements pdf
ph of group 2 hydroxides
uses of group 2 elements
group 2 elements properties
uses of group 2 compounds in agriculture
GROUP 2 ELEMENTS - Beryllium to Barium. Introduction. Group I (alkali metals) and Group 2 (alkaline earths) are known as s-block elements because their valence (bonding) electrons are in s orbitals. TRENDS IN PHYSICAL PROPERTIES. Atomic Radius. Increases down each group electrons in shells further from the
Appearance. The Group 2 elements are all metals with a shiny, silvery-white colour. General Reactivity. The alkaline earth metals are high in the reactivity series of metals, but not as high as the alkali metals of Group 1. Occurrence and Extraction. These elements are all found in the Earth's crust, but not in the elemental form
Ionisation Energy. Decreases down the group atomic size increases. Values for Group I are low because the electron has just gone into a new level and is shielded by filled inner levels. This makes them reactive. Group II elements have higher values than their Group I equivalents due to the increased nuclear charge.
CHAPTER 11: Group II. 11.1 Physical Properties of Group II Elements. 11.2 Reactions of Group II Elements. 11.3 Group II Oxides, Hydroxides and Carbonates. 11.4 Thermal Decomposition. 11.5 Uses of Group II Compounds. Learning outcomes: (a) describe the reactions of the elements with oxygen, water and dilute acids.
Alkali Metals. The group 1A elements with their ns1 valence electron configurations are very active metals. They lose their valence electrons very readily. They have low ionization energies and react with nonmetals to form ionic solids. 2Na. (s). + Cl. 2(g). > 2NaCl. (s). The expected trend in reducing ability,. Cs>Rb>K>Na>
•Small size and high charge density in Be2+. •Be is the only group 2 element that does not form a stable complex with [EDTA]4-. •Beryllium compounds tend to be covalent. •Beryllium occurs in the silicate mineral beryl Be3Al2[Si6O18], and emerald and aquamarine. X-ray Window.
The reaction gives an ionic product. If you apply oxidation numbers, you can see what has been oxidised and reduced: Calcium +. Oxygen. > Calcium oxide. 2Ca(s). +. O2(g). >. 2CaO(s). Element. 2Ca(s). +. O2(g). > 2CaO(s). Change in Ox No. Redox. Up. Down. Ca. 0. +2. 2. Ox. O. 0. - 2. 2. Red. Reaction with water.
Group 2. The physical properties of the elements. Elements of group 2 exist as solids at room temperature due to the strength of metallic bonding. The delocalised electrons in the structures give each element a silvery sheen and causes them to be good electrical conductors. They differ from other metals of the periodic table
Oxides of the s-block elements-review of group one (alkali). • Li behaves “normally". • The alkali metals will also react with oxygen to give relatively simple ionic solids,. However, when they are heated in (dry) air or an excess of O. 2. (g), the main products vary depending on the metal. ~ The alkalis are unusual in this regard
The Group 2 elements react with water to form hydroxides with the general formula M(OH)2 and hydrogen gas. The further you move down the group the more vigorous the reaction with water. Calcium, strontium and barium react with cold water and the reactivity increases from calcium to barium. In each case the metal
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