Topic 13- Introduction to periodicity Flashcards
Trend in first ionisation across period 3 and why
First ionisation energy increases
Sheilding and atomic radius remains the same
More protons= Increased nuclear charge
Greater attraction between nucleus and outermost electron
Why is the second ionisation energy greater than 1st for aluminium
Closer to the nucleus
Positive ion
3s orbital rather than 3p
Trend in atomic radius
More protons- increased nuclear charge
Sheilding is the same
Highest energy electron more strongly attracted
Atomic radius decreases
Define the term periodicity
A trend/ pattern of repeating properties
Each period 3 element and type of bonding
Sodium- Metallic
Magnesium- Metallic
Aluminium- Metallic
Silicon- Giant covalent/ macromolecular
Phosphorus- Simple covalent
Sulfur- Simple covalent
Chlorine- Simple covalent
Argon- Simple covalent