Topic 13- Introduction to periodicity Flashcards

1
Q

Trend in first ionisation across period 3 and why

A

First ionisation energy increases
Sheilding and atomic radius remains the same
More protons= Increased nuclear charge
Greater attraction between nucleus and outermost electron

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2
Q

Why is the second ionisation energy greater than 1st for aluminium

A

Closer to the nucleus
Positive ion
3s orbital rather than 3p

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3
Q

Trend in atomic radius

A

More protons- increased nuclear charge
Sheilding is the same
Highest energy electron more strongly attracted
Atomic radius decreases

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4
Q

Define the term periodicity

A

A trend/ pattern of repeating properties

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5
Q

Each period 3 element and type of bonding

A

Sodium- Metallic
Magnesium- Metallic
Aluminium- Metallic
Silicon- Giant covalent/ macromolecular
Phosphorus- Simple covalent
Sulfur- Simple covalent
Chlorine- Simple covalent
Argon- Simple covalent

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