Periodicity Flashcards
What group are He and H placed in?
He - Group 0
H - No Group
Blocks of Periodic Table
Draw it Out
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Electronic Configuration?
Diagrams
Sulfur Oxide?
SO3
Structure of Sulfur Oxide
Molecular covalent
Al2O3 Structure?
Ionic (Mostly)
pH of Na2O?
12-14
pH of MgO?
8-9
pH of Al2O3?
7
pH of SiO2?
7
What happens when Na reacts with Water?
Na reacts vigorously with water to give Hydrogen and Hydroxide
2Na(s) + 2H2O(l) –> 2NaOH(aq) + H2 (g)
Strongly Alkaline
How does the reactivity of Period 3 work?
Reactivity of period 3 towards water decreases from Na to Si, and then increases from P to Cl
How does NaCl react in Water?
Dissolves to form neutral solution
How does MgCl2 react in Water?
Dissolves to form acidic solution
Na Reaction with H2O
Reacts vigorously to form NaOH and H2
Mg Reaction with H2O?
Reacts with steam to form Magnesium Hydroxide and Hydrogen
Cl Reaction with H2O?
Dissolves in Water and some reacts to from an acidic solution
Why is the melting point of P4O10 higher than that of SO2?
P4O10 is a molecule containing 4P’s and 10 O’s. As it is a bigger molecule and has more electrons than SO2 it will have larger London forces between molecules and a higher melting point.
why do giant covalent networks have high melting and boiling point|?
They have very high melting points and boiling points . This is because large amounts of energy are needed to overcome their strong covalent bonds to make them melt or boil.
Sodium Oxide + Water
Sodium Hydroxide
Sulphur Dioxide + Water
H2SO3
Phosphorus Oxide + Water?
P4O10 + 6H2O –> 4H3PO4(G)
First Ionisation Energy?
The energy required to remove one mole of electrons from one mole of gaseous atoms
Atomic Radius
The atomic radius is the distance between the nucleus and the outermost electron of an atom
The atomic radius decreases from left to right across a period (rightwards
Electronegativity rules?
EN will increase as you go right across period
En will Decrease as you go down
Why does Atomic Radius decrease along the second period?
As you go across a period, electrons are added to the same shell, alongside an increase in nuclear charge
Therefore, electrons are equidistant from the nucleus but pulled more strongly. This decreases the distance between the nucleus and electrons (atomic radius)
