EL - periodicity Flashcards
(12 cards)
melting point along period 3, general trend
increases up to the maximum at group 4 then decreases
first three elements of period 3 - melting point
Generally increases because they are metals they have metallic bonding and a positive charge. As you go along these first three metals the charge increases and so more electrons delocalise, this means that more energy is required to break the metallic bond
silicon m.p.
Highest m.p. of period 3
Giant covalent structure so lots of strong covalent bonds to overcome
phosphorus m.p.
Simple molecular structure
Weaker intermolecular forces
M.p. decreases rapidly
sulfur m.p.
Slight increase in m.p.
Slightly larger simple molecular
Larger IM forces
Chlorine m.p.
Diatomic
Decrease in m.p.
Smaller simple molecular
Smaller IM forces
Argon m.p.
Decrease in m.p.
Only exists as individual atoms
Smaller IM forces
ionisation energy
amount of energy needed to remove one mole of an electron from one mole of an atom in gaseous state
ionisation energy across a period
General increase
It becomes harder to lose an electron
Electronegativity across a period
Increases
Atomic radius across a period
Decreases
The nuclear charge increases due to more protons in the nucleus, creating a stronger attraction between the positive nucleus and the outer electron, pulling the atom in
Density across a period
Increases to max density in group 3 then decreasing
The initial increase being because of the smaller atomic radius is more significant than the atomic mass
