why do group 7 elements become weaker oxidising agents as you go down the group?

Answer 1

because they are noble gases...gaseous elements

Answer 2

Oxidising agents mean they oxidise other atoms by accepting electrons.

Down the group, the size of atoms increase because group 7 elements have an increase in the number of electrons.

When number of electrons increase, the nuclear attraction between the positive nucleus and the outermost electrons is weaker. Thus, group 7 elements tend to lose electrons than gain electrons.

They are more inclined to be reducing agents than oxidising agents.

Answer 3

Weaker oxidising agents means they are not as ready to accept electrons in a redox reaction.

Reason being down the group they have larger orbitals with lower attraction from the protons at the central nucleus thus resulting in a lower affinity for electrons.

Answer 4

I believe this is because as you go down the group, there is a less effective nuclear charge on the electrons. the nucleus is positively charged and the effect on negatively charged electrons can be less felt as we move down the group with larger atoms and there is an increased electron repulsion due to the higher number of electrons down the group. Hence, it is more difficult for the atom to oxidise another atom e.g a group one or two atom by taking an electron.

Answer 5

The formation of hydrated ions happens much more easily at the top of the group than the bottom.
The reason is atomisation energy and electron affinity.
Atomisation energy is the energy required to produce one mole of
isolated gaseous atoms. With chlorine it is just the energy to break the Cl-Cl bonds. For a solid like bromine or a liquid like
iodine, it also includes the energy that is needed to convert them into gases.
Atomisation energy+electron affinity+hydration enthalpy=overall heat evolved, are more pronounced at the top[fluorine--chlorine] than at the bottom of the group.

Answer 6

is this a coarse work question by any chance!