Which of the following remains unchanged on moving down a group?
Which of the following remains unchanged on moving down a group?
The correct option is C Valance electrons
Valence electrons: Every group is distinguished by its valence electrons, which are the number of electrons in the elements' outermost shells that are the same within a group. As a result, the common oxidation states of elements in the same group are fixed.
Atomic size: As you move down the group, each period adds a new shell. The electron within the new shell improves shielding as well. As a result, the Z eff decreases, as does the nucleus's attractive force, so the size increases.
Density: As one moves down the group, both mass and volume increase. As a result, density is determined by the dominant factor. Typically, density increases as one moves down the group, implying that the effect of mass predominates.
Metallic character: Moving down the group, the nuclear force of attraction on outer electrons tends to decrease due to a decrease in Z eff, which is caused by the increase in shielding besides outer valence electrons. As a result, as one moves down the group, the oxidation potential tends to decrease and the metallic character increases.
Hence, the correct answer is valence electrons.
Valance electrons
Valence electrons: Every group is distinguished by its valence electrons, which are the number of electrons in the elements' outermost shells that are the same within a group. As a result, the common oxidation states of elements in the same group are fixed.
Atomic size: As you move down the group, each period adds a new shell. The electron within the new shell improves shielding as well. As a result, the Z eff decreases, as does the nucleus's attractive force, so the size increases.
Density: As one moves down the group, both mass and volume increase. As a result, density is determined by the dominant factor. Typically, density increases as one moves down the group, implying that the effect of mass predominates.
Metallic character: Moving down the group, the nuclear force of attraction on outer electrons tends to decrease due to a decrease in Z eff, which is caused by the increase in shielding besides outer valence electrons. As a result, as one moves down the group, the oxidation potential tends to decrease and the metallic character increases.
Hence, the correct answer is valence electrons.
