The chemical reactivity increases as we go down the group for metals and decreases in the case of non metals
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.
the reactivity of halogens goes on decreasing as we go down the group, because of increasing in atomic size of the respective element.
The reactivity of a non metal decreases as you move down a group. This is because the size of the atomic radius increases and when the distance to the nucleus increases, the force of attraction decreases. Electrons are not pulled as strongly to larger atoms, and so larger atoms are not as reactive.
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.
The reactivity increase down in the group.
As you go down group 7 (halogens), reactivity decreases. This is because as you move down the group, the outer electron shells of the halogens are further away from the nucleus, making it harder for them to gain an electron and react with other elements. Additionally, the atomic size increases which leads to weaker intermolecular forces between the atoms.
The reactivity is increasing goinng down in the group.
the reactivity increases as you go down 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.
The chemical reactivity increase down in 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.
The reactivity of a non metal decreases as you move down a group. This is because the size of the atomic radius increases and when the distance to the nucleus increases, the force of attraction decreases. Electrons are not pulled as strongly to larger atoms, and so larger atoms are not as reactive.
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.
Nope.
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.
Down a group, the atomic number generally increases, size increases, ionization energy decreases, reactivity increases.