The chemical equation is: Zn + H 2 SO 4 → ZnSO 4 + H 2. A particular functional group will almost always display its characteristic chemical behavior when it is present in a compound. Group 2 Elements are called Alkali Earth Metals. Calcium, strontium, and barium react with water and form corrosive hydroxides. Precipitate relates to today’s lab because we will have to observe and compare the chemical reactions of different elements. 2) The atomic radii also increases. Group 2 reactions Reactions with water. The reaction of Group II Elements with Oxygen. 3.1.2 (d, e) Reaction of Group 2 Oxides with Water and Group 2 compounds as Bases. Single Displacement Reactions Between Metals. Mg (s) + H 2O ( g) MgO (s) + H 2 (g) The other group 2 metals will react with cold water with increasing vigour down the group to form hydroxides. 1. Salts of beryllium are toxic, and water-soluble or acid-soluble salts of barium are toxic. For grade B they consider the aluminium sulphate Camelford water poisoning in Cornwall and write ionic equations. This experiment indicates the relative reactivity of elements within the group. Page 1 of 1. Introduction . Explaining trends in reactivity. Note that group II metals form mostly ionic compounds because the electronegativities are significantly lower than elements such as oxygen and chlorine. The reactivity of Group 7 elements decreases down the group. Rep:? The reactivity increases down the groups: in fact, Beryllium and Magnesium are stable in water and air due to the presence of a thin oxide layer formed by reaction with the air which prevents reaction with the water. Metals in Group 2 of the Periodic Table are less reactive than those in Group 1. 2. When a halogen atom reacts, it gains one electron into their highest occupied energy level (outer shell) to form a singly negative charged ion. Note that all ions are aqueous and … What to do . \[ Be_{(s)} + H_2O_{(g)} \rightarrow BeO_{(s)} + H_{2(g)} … Welcome to 2.6 Group 2, The Alkaline Earth Metals. To find the trend of reactions of metals with oxygen is almost impossible. The reactions of the Group 2 metals with air rather than oxygen is complicated by the fact that they all react with nitrogen to produce nitrides. Rusting is an oxidation reaction. Group 2 reactions Reactivity of group 2 metals increases down the group Mg will also react slowly with oxygen without a flame. Melting points and boiling points decrease down the group due to weaker forces of attraction between atoms. They are called s-block elements because their highest energy electrons appear in the s subshell. It cannot be said that by moving down the group these metals burn more vigorously. A precipitate is a solid form that is a result of a chemical reaction. GO: GO with the Game Plan Reactivity increases down group 2, this is due to 3 things: 1) The electron shielding increases as you go down the group. Beryllium has the highest electronegativity in Group II and, as you might predict, it forms the chloride with most covalent character. (b) Relative Reactivities of the Group 2 elements Mg → Ba shown by their redox reactions with: (i) Oxygen (ii) Water (iii) Dilute acids {Reactions with acids will be limited to those producing a salt and Hydrogen.} Beryllium as a special case. Thanks 1) Write an eqn for it, M + 2H2O -----> M(OH)2 + H2 It is metal(II) hydroxide, the 2 should be a subscript. Fill two test-tubes a quarter full with dilute hydrochloric acid. (5 marks) I got one mark for stating that as you go down the group the reactivity with water increases. in their outer shell. The reactivity of Group 2 metals . Progressing down group 2, the atomic radius increases due to the extra shell of electrons for each element. A more reactive metal will displace a less reactive metal from a compound. What is a precipitate and how does it relate to today's lab? Are precipitates soluble in water? The Mg would burn with a bright white flame. In the group 2 elements, the reactivity of the metals increase as you move down the group. The Reactivity of Group 2 Metals. For grade C students write symbol equations. I was wondering if anyone knew what other things to write about. Here, zinc sulfate and H 2 gas are formed as products. Use caution when handling these metals. There is an additional reason for the lack of reactivity of beryllium compared with the rest of the Group. Non-metal atoms gain electrons when they react with metals. The solubility of the hydroxides increases down the group. Going down the group, the first ionisation energy decreases. Beryllium reacts with steam at high temperatures (typically around 700°C or more) to give white beryllium oxide and hydrogen. Reactivity of group 2 metals increases down the group Magnesium burns in steam to produce magnesium oxide and hydrogen. Each metal is naturally occurring and quite reactive. Go to first unread Skip to page: cheekymokeyxxx Badges: 0. Period 7. Jose & Lindsay Sanchez Reactivity of Group 2 Metal Atoms Pre-lab: 1. Chemical Reactivity decrease as you go left to right of the periodic table; Chemical Reactivity increases as you go down the group; This happens because as you go down a group, it is easier for electrons to be taken or given away, resulting in high Chemical Reactivity. The overall trend, for the reactivity of Group 2 metals with water, is an increase down the group. As a whole, metals when burns with the oxygen form a simple metal oxide. Functional groups are atoms or small groups of atoms (two to four) that exhibit a characteristic reactivity when treated with certain reagents. The Group 2 metals become more reactive towards water as you go down the Group. The outer electrons are easier to remove as they are further from the nucleus and there is more shielding resulting in a lower nuclear attraction. They react magnesium and calcium with dilute acid in order to determine how reactive the metals are. Chemical reactivity with halogens of Group 1 and Group 2 elements : The elements belonging to group 1 are called alkali metals. Reactions . Thus, the reactions between metals and some acids can be predicted with the help of the reactivity series. Redox reactions . Mg ribbon will often have a thin layer of magnesium oxide on it formed by reaction with oxygen. Each alkaline earth metal has two valence electrons. Reactivity increases down the group. These hydroxides have a typical pH of 10-12. (a) Reaction rate (reactivity) increases down group 2 from top to bottom (b) First ionisation energy decreases down group 2 from top to bottom (d) Magnesium is the second element from the top in Group 2 and does not react with hydrogen but does react with water slowly. Hardness increases as you descend down the group. Therefore there is a greater attraction between the nucleus and electrons in magnesium than there is in calcium. The order of reactivity in group 2 is barium, strontium, calcium, and magnesium. Announcements Applying to uni? Non-Metals: Reactivity decreases as you go down the group. Note that the hydroxides and sulphates show opposite trends in solubility. Reactions of group 2 metals Watch. They constitute the six elements namely, lithium(Li), sodium(Na), potassium(K), rubidium(Rb), cesium(Cs) and francium(Fr). This is an AS Chemistry lesson on the group 2 metal compounds and their reactivity and solubility at grades C to A. This is because the smaller the atom the closer the outer electrons are to the nucleus. Beryllium, interestingly, does not react with water. 3. Summary of the trend in reactivity. #1 Report Thread starter 8 years ago #1 I have to know by heart the visual change that occurs when of Magnesium, Calcium, Strontium and Barium salts react with the following things.. 1. 2. Explaining the trend in reactivity. - they all have one electron. Group 2 elements share common characteristics. Reactivity increases as you go down the group. Functional Group Reactions. These metals are silver and soft, much like the alkali metals of Group 1. Basically, the more electron shielding an atom has the less attracted it's outermost … ** The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, = higher reactivity. Find your group chat here >> start new discussion reply. This is an experiment that students can carry out for themselves. In each case, you will get a mixture of the metal oxide and the metal nitride. Describe and explain the trend, down the group, in the reactivity of Group 2 elements with water. Group 2 oxides react with water to form a solution of metal hydroxides. These metals also react with water, though not as vigorously. Beryllium is reluctant to burn unless in the form of powder or dust. The reactivity series allows us to predict how metals will react. ** The farther right and up you go on the periodic table, the higher the electronegativity, = harder exchange of electron. 2.6 Group 2, The Alkaline Earth Metals notes. sulphates and carbonates of Group 2 elements as you go down the Group. Group 2 hydroxides dissolve in water to form alkaline solutions. Such reaction is: $$MgO_{(s)} + H_{2}O_{(l)} \rightarrow Mg(OH)_{2(aq)}$$ Group 2 hydroxides. Explaining reactivity The Group 1 elements have similar properties because of the electronic structure of their atoms. 2.4, 2.5, 2.6 Assessed Homework Task (mark scheme) 2.4, 2.5, 2.6 Test (mark scheme) More Exam Questions on 2.4 Redox Reactions, 2.5 Group 7, The Halogens and 2.6 Group 2, The Alkaline Earth Metals (mark scheme) 2.6 Exercise 1 - trends in group 2 . This page discusses the reactions of the Group 2 elements (beryllium, magnesium, calcium, strontium and barium) with water, using these reactions to describe the trend in reactivity in Group 2. Into one test-tube drop a small piece of magnesium. 2Mg + O2 2MgO This needs to be cleaned off by emery paper before doing reactions with Mg ribbon. The reaction between zinc and sulphuric acid is an example of such a reaction. The alkaline earth metals undergo reactions similar to … Category: Chemistry. Beryllium. The experiment can easily be expanded by reacting the same metals with water. 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