Alkali metals (so Group 1) however do give away their electrons much more easily and so are considered to be more reactive. Lead and the metals ranking above lead on the activity series form salts when reacted with hydrochloric acid or sulphuric acid. losing their 2 outer electrons to form a 2+ ion with non-metals. As you go down group 1 from lithium to francium, the alkali metals. In group 7 atoms get bigger down the group. The overall trend, for the reactivity of Group 2 metals with water, is an increase down the group. This is because they all have 1 electron in their outer shell which is why they react in similar ways. That is why as you go up a group Chemical Reactivity increases because it is easier for elements to gain electrons when they have high electronegativity. Now on moving down the group , the size of atom increases due to addition of atomic shells due to this , the tendency of an atom to gain electron decreases down the group due to decrease in nuclear charge . As you go up group 7 (the halogens), again the elements get more reactive. Four metals F,G,H and J were each separately added to cold water , hot water and steam . Included in the group two elements are Beryllium(Be), Magnesium(Mg), Calcium(Ca), Strontium(Sr), and Barium(Ba). All group 1 metals have one electron in its outer shell. They are called s-block elements because their highest energy electrons appear in the s subshell. I was wondering if anyone knew what other things to write about. Why do the reactivity of the group 1 atoms increase as you go down the group, but the reactivity of group 7 decreases as you go down the group. The answer lies in understanding what the atoms are trying to do. As you know that non- metals have the ability of gaining electrons ,so the non metal which can easily gain electron is more reactive. Does the reactivity with chlorine increase or decrease down group 2? Why do group 2 metal melting points decrease down the group?.Atomic radius increases increasing distance from nucleus.Shielding increases as shell are added 20. The resource is set out as teachers' notes followed by the students' page which presents the task to be investigated. Thanks Based on this information, what group do you expect this element to be in? 2. increases down the group in the periodic table, or that hydrogen's reactivity is evidenced by its reaction with oxygen. In this classic experiment, from the Royal Society of Chemistry, students carry out a series of chemical reactions involving group 2 metals. Have bigger atoms.Each successive element in the next period down has an extra electron shell. Explain. 1. Are softer.3. The Group 2 metals become more reactive towards water as you go down the Group. Similarly, what happens to the reactivity of alkali metals as you go down the group? The reactivity series allows us to predict how metals will react. a gp the removal of electron require less energy .therefore reactivity increases. Metals react by losing electrons so larger atoms lose electrons more readily as the outer electrons are further from nucleus and less attracted. very slow at RTP, with a pH of around 10 as the Mg(OH)2 is only sparingly soluble. Chemical Reactivity  decrease as you go down  the group; For Non-Metals, the farther right-up in the table you go, the higher the electronegativity. Based on this information, what group do you expect this element to be in? 8. For a metal, alkali earth metals tend to have low melting points and low densities. Beryllium as a special case. Using the results they determine the order of reactivity in group 2. Usually, there is no need to store these elements in oil, unlike the group one elements. 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. Period - reactivity increases as you go from the left to the right across a period. Describe the reactivity trend in group 2 metals. Why do some metals form peroxides on heating in oxygen? Going down the group… Alkali Earth Metals – Group 2 Elements. Therefore, the reactivity series of metals can be used to predict the reactions between metals and water. As we move down the group of 1 A. and 2 A which are metals, the reactivity increases as we move down the group. There is an increase in the tendency to form the peroxide as you go down the Group. Have a higher density.. 4. Reaction Between Metals and Acids. The easier an electron escapes, the more reactive the metals … In chemistry, a reactivity series (or activity series) is an empirical, calculated, and structurally analytical progression of a series of metals, arranged by their "reactivity" from highest to lowest. Non-metal atoms gain electrons when they react with metals. For example, it is commonly asserted that the reactivity of group one metals (Na, K, etc.) It is used to summarize information about the reactions of metals with acids and water, single displacement reactions and the extraction of metals from their ores reaction of magnesium and water. When a halogen atom reacts, it gains one electron into their highest occupied energy level (outer shell) to form a singly negative charged ion. The Periodic Table. Progressing down group 2, the atomic radius increases due to the extra shell of electrons for each element.