Periodicity Flashcards
Forces of attraction in metal
Electrostatic
Electron configuration of Ni +2
1s2 2s2 2p6 3s2 3p6 3d8
Name something that can react with acid E.g. HCl
Any alkali E.g. NaOH
Why is the melting point of magnesium is higher than that of sodium
Greater ionic charge
Smaller ion
More delocalised electrons
Stronger attraction between ions and delocalised electrons
General trend in ionisation energy across period 3
Increases
More protons but same shielding
What does an element have to have in order to be classed as p block element
Outer electrons are in p orbital
Why are Van Der waals weak in liquid non-metal
Particles are single atoms with electrons closer to nucleus
Cannot be easily polarised
Trend in atomic radius down group
Increases
Even though more protons
In electron configuration what happens after 4p6
5s2
(Same rules as 4s2)
What bonding is in a substance that does not conduct electricity when molten
Covalent
Describe in terms of electrons bonding in Na2S
Each sodium loses electron to form +1 charge then the sulfur gains the electrons from the sodium to form -2 charge
Trend in melting point across period 3
Increases sodium to aluminium
Metallic bonding
As we move across number of delocalised electrons per metal atom increases and radius decreases greater electrostatic forces of attraction.
Silicon increases
Macro molecular structure strong covalent bonds
Decreases after phosphorus
Van der waals which are weak
Why has highest melting point out of p s and cl + why
Sulfur
It is the largest molecule out of the 3 so has the most Van der waals
Observation when magnesium reacts with steam
White light
Trend in melting point down group 2 and why
Decreases
Metallic bonding
The radius of the metal ion increases but the number of delocalised electrons stays the same
