Module 3 Periodicity Flashcards
What is meant by periodicity?
The repeating trends in chemical and physical properties.
Define first ionisation energy.
The energy required to remove on electron from each atom in one mole of the gaseous element to form one mole of gaseous 1+ ions.
What are the factors affecting ionisation energy?
- Atomic radius
- Nuclear charge
- Electron shielding/screening
Why does first ionisation decrease between groups 2 and 3?
In group 3, the outermost electrons are in p orbital, whereas in group 2 they are in the s orbital meaning electrons are easier to remove.
Why does first ionisation energy increase between groups 5 and 6?
In group 5, the electrons in p orbital are single electrons and in group 6 the outermost electrons are spin paired with repulsion. Meaning electrons are easier to remove.
What are the properties of giant metallic lattices?
- High melting and boiling point
- Good electrical conductors
- Malleability
- Ductility
What is a ductile and malleable metal?
Ductile- the metal can be stretched.
Malleable- the metal can be shaped into different forms.
What is the structure, forces and bonding of the elements in period 2?
- Li and Be -> giant metallic, strong attraction between positive ions and delocalised electrons, metallic bonding.
- B and C -> giant covalent, strong forces between atoms, covalent.
- N, O, F and NE -> simple molecular, weak intermolecular forces between molecules, covalent bonding within molecules and intermolecular forces between molecules.
What are the structures, forces and bonding of the element in period 3?
- Na, Mg and Al-> giant metallic, strong attraction between positive ions and delocalised electrons and metallic bonding.
- Si -> giant covalent, strong forces between atoms and covalent.
- P, S, Cl and Ar -> simple molecular, weak intermolecular forces between molecules and covalent bonding within molecules and intermolecular forces between molecules.
