Periodicity - 3
No description yet. This curated deck is ready for daily study.
Card preview (12)
How are elements arranged in the periodic table
Arranged in order of increasing atomic number
Define periodicity
The repeating trends in chemical and physical properties
Define first ionisation energy
The energy required to remove one electron from each atom in one mole of the gaseous element to form one mole of gaseous 1+ ions
Write an equation for the first ionisation energy of a metal (X)
X (g) —-> X+ (g) + e-
What three factors affect ionisation energy
Atomic radius Nuclear charge Electron shielding
What happens to the ionisation energy down a group and why
Ionisation energy decreases Shielding increases, so weaker forces of attraction Atomic radius increases, so distance between valence electron and nucleus increase, so weaker attraction Increase of protons outweighed
What is a ductile metal
The metal can be stretched
Why does first ionisation energy decrease between group 2 to 3
In group 3 the outermost electrons are in the p orbitals, where as in group 2 they are in the s orbital, so the electrons are easier to remove
Why does first ionisation energy decrease between group 5 to 6
Group 5 electrons in p-orbital are single electrons and in the group 6 the outermost electrons are spin paired, with some repulsion, therefore the electrons are slightly easier to remove
What happens to ionisation energy between the end of one period and the start of the next.
Decreases because there is an increase in atomic radius and an increase in electron shielding
What are the properties of giant metallic lattices
Heigh melting/boiling point Good electrical conductors Malleability Ductility
What is a malleable metal
The metal can be shaped into different forms