Outcome 1- Periodic Table Flashcards
The Trends of Properties of elements Across the periodic table
Atomic Radius: Decreases (Increased force into centre due to increasing core charge)
Electronegativity: Increases (closer to Fluroine)
1st Ionization energy: Increases
Metallic/ non-metallic character: Decreases
Reactivity:
The Trends of Properties of elements down the Periodic table
Atomic Radius: Increases (Same core charge but increased amount of protons)
Electronegativity: Decreases
1st Ionization energy: Decreases
Metallic/ non-metallic character: Increases
Reactivity: Increases
Expections of Electron Configuration and why?
Chronium and copper The actual electron configurations are: Cr = [Ar] 4s1 3d5 Cu =[Ar] 4s1 3d10 in these two cases, a completely full or half full d sub-level is more stable than a partially filled d sub-level, so an electron from the 4s orbital is excited and rises to a 3d orbital.
What does electron configurations tell us on where the element is on the periodic table?
The Subshell tells us the period tells us the group number eg
1s2,2s2,2p5 = Period 2, Group 7 (2+5) equals Fluorine
How do transition metals differ to main group metals?
There are no transition elements in the first three periods because they require 4 orbitals. Transition metals are in the d subshell where as metals are in the s subshell and Metals in group 1 and 2 are more reactive.
What are the properties and reactivity of s-block, d-block and p-block metals?
S-block- Alkali metals- Very reactive, low density and melting points due to one outershell electron, are not found in elemental form.
d- block- Transition metals- They can form ions with different charge, use catalysts, coloured
p-block- Non metals and metal alloids-s. generally have low boiling points, are poor conductors, and do not lose electrons easily.
The FIrst ionisation energy of period 2
increases irregulary from Li to Ne
