Does Zeff increase down the group?
Going down a group, distance and shielding increase. Effective Nuclear Charge (Zeff) remains constant. Going down a group, distance and shielding increase. Effective Nuclear Charge (Zeff) remains constant.
What factors affect effective nuclear charge?
Effective Nuclear Charge (Zeff) According to Coulomb’s law, the attraction of an electron to a nucleus depends only on three factors: the charge of the nucleus (+Z), the charge of the electron (-1), and the distance between the two (r).
What happens to Z effective down the group?
The periodic table tendency for effective nuclear charge: Increase across a period (due to increasing nuclear charge with no accompanying increase in shielding effect). Decrease down a group (although nuclear charge increases down a group, shielding effect more than counters its effect).
Why does Zeff increase going down a group?
A higher effective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius. Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital.
Why does shielding effect increase down a group?
The decrease in the force of attraction between the nucleus and valence electrons is called the screening effect. – Down the group the number of inner shells increases, therefore, the shielding effect also increases in the group.
Why is Zeff constant down a group?
In general, atomic radius decreases across a period and increases down a group. Across a period, effective nuclear charge increases as electron shielding remains constant. Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital.
Why does effective nuclear charge increase from left to right?
The atomic size generally decreases across a period. This is because within a period the outer electrons are in the same valence shell and the effective nuclear charge increases as the atomic number increases resulting in the increased attraction of electrons to the nucleus.
Why does Zeff increase going down?
The effective nuclear charge, Zeff, increases down a group which draws electrons closer towards the nucleus, decreasing atomic radius.