Please enable JavaScript.
Coggle requires JavaScript to display documents.
Periodic Trends (Nam. Jun Hee, Minh, Khanh, Kevin) - Coggle Diagram
Periodic Trends (Nam. Jun Hee, Minh, Khanh, Kevin)
Ionization
-
It increases from left to right (Period)
- Effective nuclear charge causes an increase in the attractive force holding electrons
It increases from top to bottom (Group)
- The outer electron is in a larger energy shell, and is therefore less attracted to the nucleus, and is easier to remove
Effective Nuclear Charge (ZEFF) : From left to right on the periodic table, and from bottom to top on the periodic table, ZEFF increases. They increase as electron shielding remains constant.This pulls the electron cloud closer to the nucleus, strengthening the nuclear attraction to the outer-most electrons, and thus, is more difficult to remove (requires more energy).
Why this happens: Zeff increases from top to bottom because while there is an addition of higher electron shells the increasing positive nucleus outweighs the effect.
Equation is as follows: zeff = Z-S where Z is atomic number and S is # of shielding electrons
-
Electron Affinity: The energy that is released or absorbed when a single electron is added to a neutral atom in the gaseous state.
Electron Affinity increases as you go across a period (left to right). This is because the effective nuclear charge increases and more electrons are attached to the atom.
It also increase as you go up a group (top to bottom). This is because the atom becomes smaller, and the valence shell is closer to the nucleus, which makes the electrons attracted to the atom.
Atomic Radius
As we go across the periodic table, the atomic radius decreases due to the increases of protons that makes the attraction force stronger. As we go down the periodic table, the atomic radius increases because the atom is bigger.
-
-
-
-
-
-
-
-
-