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As you move down Group 17 (halogens) from top to bottom, the reactivity decreases. This is due to the increasing atomic size and electron shielding, making it more difficult for the outer electron to be gained by the lower elements in the group, thus decreasing their reactivity.
Halogens are group seven on the Periodic Table, this means they take electrons during bonding as opposed to giving them. Halogens are often used for cleaning and disinfecting, most notably in pools. They are also poisonous and were introduced into warfare in the first world war. Halogens are common in acids such as hydro-CHLORIC acid.
As we move down the group of halogens the number of shells increase (as the number of periods are increased). Thus the halogens become less reactive. Halogens react by gaining an electron to have a complete outer shell (as they have seven). As the number of shells increase, the magnetic force from the nucleus (of the protons to the electrons) decrease thus make them less likely to gain an electron from other molecules. So the ones nearer to the bottom (e.g. iodine) will be less reactive than the one nearer to the top (e.g. chlorine).
Reactivity in group 1 of elements increases as we go down the group (to francium) because in the alkali metals as we go down the group number of atomic shells increases so the elements with most shells will easily release their electrons in the outer most shell.
The highly reactive members of group 17 in the periodic table are fluorine, chlorine, bromine, iodine, and astatine. They are known as the halogens and readily react with other elements to form compounds. Their reactivity decreases going down the group.
the reactivity of halogens goes on decreasing as we go down the group, because of increasing in atomic size of the respective element.
Nope.
The reactivity increase down in the group.
The reactivity of Group 7 halogens decreases as you move down the column from fluorine to iodine. This is because atomic size increases down the group, leading to weaker intermolecular forces of attraction between atoms. As a result, it becomes harder for the halogens to gain an extra electron and they become less reactive.
Halogens have high reactivity because they have a strong tendency to gain an electron to achieve a stable electron configuration. This reactivity decreases as you move down the group from fluorine to iodine.
As it go down the group, the distance between the nucleus (+ve) and the last electron (-ve) becomes smaller No: BIGGER.Therefore the electrons are held in the atom very tightly more loosely by a strong weakening force from the nucleus.So, it is said as the reactivityDEcreases down the group of NON-metals which gain stronger their electrons andINcreases down the group of metals which loose those electrons.
Reactivity decreases. In other words, fluorine is the most reactive of the halogens while astatine is the lease reactive. This is because the ability to attract electrons(electronegativity) decreases as you go down the group.
The periodicity of nonmetals is that reactivity increases from left to right across a period, through group 17, the halogens. As you move down a group, reactivity decreases. Fluorine is the most reactive element.
As you move down Group 17 (halogens) from top to bottom, the reactivity decreases. This is due to the increasing atomic size and electron shielding, making it more difficult for the outer electron to be gained by the lower elements in the group, thus decreasing their reactivity.
In the periodic table, the reactivity of the halogens that are found in Group 17 decreases as you go down the column of elements in this group. The first element of the group is fluorine, and it has the highest reactivity. The other elements in this group are chlorine, bromine, iodine, and astatine.
The reactivity is increasing goinng down in the group.
As you go down Group 1 (alkali metals), reactivity increases due to the lower ionization energy, making it easier for these metals to lose their outermost electron. In contrast, Group 2 (alkaline earth metals) also shows an increase in reactivity down the group, but the trend is less pronounced compared to Group 1. This is because while ionization energy decreases, the presence of two outer electrons means that the reactivity is not solely dependent on losing one electron. Overall, both groups exhibit increasing reactivity down the group, but the rate of change is stronger in Group 1.