Period - reactivity increases as you go from the left to the right across a period. Included in the group two elements are Beryllium(Be), Magnesium(Mg), Calcium(Ca), Strontium(Sr), and Barium(Ba). Have a higher density.. 4. Simply, as we go down the in the group 1 elements, electron shells increase, so the nucleus attraction decreases, making it easier for an electron to escape. Except for beryllium (2), the Group 2 elements are typical metals: (a) relatively soft, but harder than group 1 metals, shiny solids at room temperature and pressure that are good conductors of heat and electricity (b) Moderately-high melting point. Does the reactivity with chlorine increase or decrease down group 2? so the reactivity increases .as we go down in . Explain why the reactivity of group (VII) elements decreases down the group; 19. They are called s-block elements because their highest energy electrons appear in the s subshell. Properties: Soft metals that can be cut with a knife. In group 7 atoms get bigger down the group. Using the results they determine the order of reactivity in group 2. Reactivity: In chemistry, reactivity refers to how readily a substance undergoes a chemical reaction. The alkaline earth metals are less reactive than the alkali metals. Based on this information, what group do you expect this element to be in? (5 marks) I got one mark for stating that as you go down the group the reactivity with water increases. The answer to your question is quite simple.The alkali metals of group 1 grow larger in size downwards and since the effective nuclear charge remains the same as we go down group 1 the number of shells also increases and so it is easy to lose an electron and therefore as we move downwards the reactivity … I was wondering if anyone knew what other things to write about. This is because they all have 1 electron in their outer shell which is why they react in similar ways. This is why the solubility of Group 2 hydroxides increases while progressing down the group. 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. Why do group 2 metal melting points decrease down the group?.Atomic radius increases increasing distance from nucleus.Shielding increases as shell are added 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. 1. 3. The answer lies in understanding what the atoms are trying to do. Thanks Beryllium, magnesium and calcium don't form peroxides when heated in oxygen, but strontium and barium do. In the group 2 elements, the reactivity of the metals increase as you move down the group. There is an increase in the tendency to form the peroxide as you go down the Group. As you go down group 1 (the alkali metals) in the periodic table, the elements get more reactive. All group 1 metals have one electron in its outer shell. Doc Tang 10,794 views. very slow at RTP, with a pH of around 10 as the Mg(OH)2 is only sparingly soluble. Alkali metals (so Group 1) however do give away their electrons much more easily and so are considered to be more reactive. 8. 9. losing their 2 outer electrons to form a 2+ ion with non-metals. The Group 2 metals become more reactive towards water as you go down the Group. (c) have 2 valence electrons (2 electrons in the highest energy level) (d) are very reactive The overall trend, for the reactivity of Group 2 metals with water, is an increase down the group. Beryllium, magnesium and calcium don't form peroxides when heated in oxygen, but strontium and barium do. Low melting points in comparison with other metals. Describe the reactivity trend in group 2 metals. 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. 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. Lead and the metals ranking above lead on the activity series form salts when reacted with hydrochloric acid or sulphuric acid. 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 resource is set out as teachers' notes followed by the students' page which presents the task to be investigated. I get why it does in group 1, but I don't get why it does in group 7?? Explaining trends in reactivity. Have lower melting points and boiling points.. 2. what do group 2 metals react with water to form. 2. Group 1 - The Alkali Metals- Group Trends.. What are the Group Trends for the Alkali Metals? Is as follows: To remember how the reactivity of the alkali metals and halogens increases or decreases, put a pin in the middle of the periodic table and spin it anti-clockwise. Now let's look at $\ce{SO4^2-}$. due to ionization energy decreases . The reactivity of Group 7 elements decreases down the group. Why do some metals form peroxides on heating in oxygen? Summary of the trend in reactivity. Describe and explain the trend, down the group, in the reactivity of Group 2 elements with water. However, Group 7 react by gaining electrons. As you go up group 7 (the halogens), again the elements get more reactive. a gp the removal of electron require less energy .therefore reactivity increases. 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. 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. reaction of magnesium and water. 1.3.2 (b) Reactivity of Group 2 Elements. In this classic experiment, from the Royal Society of Chemistry, students carry out a series of chemical reactions involving group 2 metals. The reactivity of the alkali metals depends upon the loss of the outermost electron. Why do some metals form peroxides on heating in oxygen? Are softer.3. For example, it is commonly asserted that the reactivity of group one metals (Na, K, etc.) With the exception of magnesium, the alkaline earth metals have to be stored under oil, or they react with oxygen in the air. 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 . 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