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sophie zhang

on 14 October 2013

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DATE: OCT 7 2013
CREATED BY: Sophie Lucy Bessie
TEAM: Bessie Lucy Sophie
Atomic numbers increases as we go across a period (from left to right). Atomic numbers increases as we go across a period (from left to right).
Ionization energy and electron affinity share the same trend on this new periodic table. They increase as one goes from top to bottom and from right to left.
An example for electron affinity would be Chlorine, which releases 349 kJ/mol of energy when becoming Cl-.
For example, the ionization energy for helium is 2370 kJ/mol, which means it takes up that much energy to take one electron away from the helium atom.
The reactivity decreases as it goes from top to bottom and also from left to right.
For example, the atomic radius of Lithium is smaller than that of Boron as you go from left to right.
The last element in each group that contains 5 elements are all noble gases, plus helium.
Easy to understand
Small adjustment of the current periodic table
Is colour coded
It shows the electron configuration and energy sublevels of elements, therefore making it easier to draw energy level diagrams and writing out electron configuration.
Shows all the trends that are in the current periodic table e.g. trend of atomic radii, electronegativity, ionization energy and electron affinity
It even includes 2 extra elements than the old periodic table; Unbilinium(Ubn) with the atomic number of 120, and Ununennium (Uue) with the atomic number 119

In this periodic table, the atomic radii increases as it going from left to right as well as when it goes from top to bottom.
Each group going vertically down represents one energy sub-level.
There are two exceptions that don’t follow the electron filling pattern, which are La and Lu, and Ac and Lr.
The energy level of the electron configuration and the group number corresponds with each other; by increasing simultaneously.
For example Hydrogen and Helium are in the same group and represent the 1s orbital.
All you have to do is switch their places when you are doing the electron configuration.
Electronegativity is the energy needed for an atom to attract electrons in order to form an ionic bond.
The groups that only contain 2 elements (excluding the first group) are metals.
The unknown elements are listed in the second last column.
As one goes down a group, the reactivity level of elements decreases.
Electronegativity increases from right to left as well as from top to bottom.
For example Sodium and Chloride forms an ionic bond, that is because Chlorine's electronegativity is stronger than Sodium's, therefore Chlorine takes an electron from Sodium, creating an ionic bond.
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