![]() ![]() Fluorine is mixed with lithium iodide Can fluorine displace iodine from lithium iodide? Why? Write the word equation.Describe the chemical test for chlorine.Give two uses for chlorine and one use for iodine.Why can chlorine displace bromine from sodium bromide?.What happens in a displacement reaction?.What is the trend in reactivity for halogens when going down the group?.What is the name of the product formed in this reaction? Write the word equation. What is formed when halogens react with metals?.Describe what fluorine, chlorine, bromine and iodine look like at room temperature.In which group of the periodic table are the halogens found?.If a damp, blue litmus paper is placed in chlorine gas, it first turns red then bleaches white. Chlorine is used as a disinfectant in swimming pools and in bleaches. UsesĪll halogens can be used in disinfectants and bleaches because they kill microorganisms like bacteria and remove colour from materials. However, bromine cannot displace chlorine from sodium chloride because it is less reactive. For example, chlorine displaces bromine from sodium bromide in solution because chlorine is more reactive than bromine.Ĭhlorine + sodium bromide à sodium chloride + bromine The order of the reactivity of halogens can be shown using displacement reactions where a more reactive element takes the place of a less reactive element in a salt. Reactivity of group 7 non-metals decreases as you go down the group. The halogens become less likely to react in chemical reactions when going down the group. A more reactive halogen can displace a less reactive halogen from a solution of. They frequently form halides when they react with metals and nonmetals. The halogens form covalent compounds by sharing electrons with other non-metals. Most halogens react with metals to form salts called metal halides, for example:Ĭhlorine + magnesium -> magnesium chloride In nature, halogens are extremely reactive. ![]() Bromine is a brown liquid that evaporates easily. ![]() At room temperature, fluorine is a pale yellow gas and chlorine a green gas. When going down group 7 melting points, boiling points and densities of the halogens increase. In addition, all halogens are poisonous and corrosive which means they burn through metals and living tissue like skin. They are non-metals which makes them poor conductors of heat and electricity. They share some similar properties (= features) and show a pattern in the way their properties change throughout the group.Īll halogens exist as diatomic molecules where two atoms are held together by a chemical bond. In summary, the trend in reactivity of group 7 elements is that it decreases down the group due to the increasing atomic size, which reduces the attraction between the outermost electrons and the positively charged nucleus, making it harder for them to react with other atoms.Elements in group 7 of the periodic table are called the halogens. this is because atomic shielding increases going down the group, meaning out electron is further away from nucleus. Therefore, the reactivity of halogens decreases as we move down the group. What is the trend in reactivity going down group 7 -going down group 7, reactivity decreases. Conversely, as the atomic size decreases, the outermost electrons are more tightly bound to the nucleus, making it harder for them to react with other atoms. This larger atomic radius means that the outermost electrons are further away from the positively charged nucleus and are therefore less strongly attracted to it.Īs a result, the outermost electrons in the larger halogen atoms are more easily attracted to another atom's positively charged nucleus, allowing for more readily occurring chemical reactions. ![]() As we move down the group, the number of occupied electron shells increases, which leads to an increase in the atomic radius. This trend can be explained by the increasing atomic size down the group. The reactivity of these elements decreases down the group. Group 7 elements, also known as halogens, include fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). ![]()
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