Periodicty Flashcards
What happens are you go across the period in terms of atomic radius
The atomic radius decreases as the number of protons increases
And the atoms have similar shielding
What happens as you go down a group in terms of atomic radius
Increases as the number of shells increases therefore more shielding
What happens as you go across the period in terms of Ionisation energy (Ei)
Increases as the nuclear charge increases
the number of shells decrease and the shielding is similar
What happens as you go down the group in terms of Ionisation energy (Ei)
Decreases as the number of shells increases therefore the shielding also increases
The nuclear charge decreases therefore weaker force of attraction between the positive nucleus and outer electrons
Harder to attract a pair of electrons
What block is group 1 and 2 in
S block
What block is the transition metals in
D block
What block is the radioactive elements in
F block
What blocks is the group 3 to 0 in
P block
What metals in period 3 have a high melting point and boiling point
Sodium
Magnesium
Aluminium
Explain why the given metals have a high mp and bp
Strong metallic bonding
The bigger the sea of delocalised electrons and positive ions the stronger the force
More energy required to break the bonds
What are the simple covalent molecules structures in period 3
Sulphur s8
Phosphorus p4
Chlorine Cl2
Why do these simple covalent structure have weak mp and bp
Weak vdw forces
Little energy is required to break the bonds
What is the macromolecular structure in period 3
Silicon
Why does silicon have a high mp and bp
Macromolecular structure
Strong covalent bonds
Lots of energy is required to break the bonds
Why does S8 have a higher mp and bp than p4
As sulphur has more electrons therefore it has stronger vdw than phosphorus meaning more energy to break the bonds
