1.6.20 demonstrate knowledge and understanding of how the reactivity down the group depends on the outer shell electrons of the atoms; Republic of Ireland. The student added: - aqueous chlorine to potassium bromine and potassium iodide solutions - aqueous bromine to potassium chloride and potassium iodide solutions - aqueous iodine to potassium chloride and potassium bromide solutions. The number of electron shells increases down the group. The alkali metals show a number of trends when moving down the group - for instance, decreasing electro negativity, increasing reactivity, and decreasing melting and boiling point. so the reactivity in gp. 7 decreases as it goes down the group. Task 2: The Reactivity Trend of the Halogens . 1. Chlorine, bromine and iodine are Group 7 elements. This type of reaction is called thermal decomposition. The further down the group, the more difficult it is to decompose. Consequently, the attraction between the … however, the further the outer electron shell (negative charge) is, the less strongly "sucked in" by the proton (positive charge), thus the 1 electron that it wants to have is less strongly attracted. • Down the group the atoms and so the molecules get larger. Understand how the differences between the reactions of these elements with air and water provide evidence for the trend in reactivity in Group 1. As with group 1 and 2, the trends in properties and GENERAL reactivity in group 7 can be explained by their electronic configuration: The reason that melting and boiling points increase down the group is because the intermolecular forces between the halogen molecules (e.g. Group 2 carbonates can be decomposed by heat, forming an oxide and carbon dioxide. In this video I take a look at the trend in reactivity as we go down group 7 and the reasons behind this trend. It is difficult to develop a simple explanation for this trend because density depends on two factors, both of which change down the group. This weaker attraction in … Note: Summary of the trend in reactivity. Chemistry. Group 1 elements are known as Alkali Metals. As elements get bigger, they have a higher level of reactivity. Are bad conductors of heat and electricity.. 4. The Halogen oxides are acidic, and the hydrides are covalent. The halogens are so reactive that they cannot exist free in nature. Reactivity increases down the group. Trend of Reactivity in Group 1 Metals: The Reactivity of Group 1 Metals will increase down the group; Covers: background information about groups 2 and 7, reactions of group 2, reactivity trend down group 2 (linking back to ionisation energy), solubility for group 2 hydroxides, reactivity trend down group 7, reactions of the halogens (plus ionic equations), the reaction of chlorine with sodium hydroxide, benefits and risks of chlorine use. General Reactivity The elements of Group 7 are a very similar set of non-metals. They all exist as diatomic molecules, X 2, and oxidise metals to form Halides. Have a higher density.. 3. 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. conversely, the reactivity in gp.1 increases because of the same reason. This trend is shown in the figure below: The metals in this series are relatively light— lithium, sodium, and potassium are less dense than water (less than 1 g cm-3). 1.6.14 demonstrate knowledge and understanding of how the trend in reactivity down the group depends on the outer shell electrons of the atoms. Electronegativity decreases down group 17 from top to bottom. • There are only weak van der Waals’ forces between the molecules. And more with flashcards, games, and the reasons behind this trend non-radioactive is. 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