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 reactivity
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 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.
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.
Nonmetal activity tends to decrease as one goes down Group 17 (halogens) because the atomic size increases along the group, leading to weaker attraction for electrons and thus decreasing reactivity. Additionally, the atomic number increases which leads to increasing electron shielding and decreasing effective nuclear charge, reducing the tendency to gain electrons.
the reactivity of halogens goes on decreasing as we go down the group, because of increasing in atomic size of the respective element.
Nope.
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 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.
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 increase down in the group.
Nonmetal activity tends to decrease as one goes down Group 17 (halogens) because the atomic size increases along the group, leading to weaker attraction for electrons and thus decreasing reactivity. Additionally, the atomic number increases which leads to increasing electron shielding and decreasing effective nuclear charge, reducing the tendency to gain electrons.
Reactivity tends to decrease as you go down a group in the periodic table. This is because as you move down a group, the valence electrons are further from the nucleus and are shielded by more inner electron shells, making it harder for the outer electrons to participate in chemical reactions.