Chapter 7 periodicity Flashcards
In which directions on the periodic table does ionisation energy increase
To the right and up
In which directions on the periodic table does electron affinity increase?
To the right and up
In which directions on the periodic table does atomic radius increase?
To the left and down
What are the factors affecting ionisation energy?
Atomic radius, nuclear charge and shielding
When does the ionisation energy decrease across a period?
When an electron is added to a new sub shell and when the first pairing electron in a P, D, F shell.
Why does the first pairing electron in a sub shell have. A decreased ionisation energy?
Because the electron its is pair of electrons repel each other making loosing an electron easier.
Why is there a large decrease in ionisation energy in a new period?
Because a new shell is added which means the highest energy electron is further away from the nucleus and has more electron shielding
What are macroscopic properties?
Properties that can be directly observed
What are macromolecular structures?
Giant lattice structures
What is the structure of a metallic lattice?
Positive metal ions in a regular structure held in place by strong electrostatic forces between the positive metal ions and the delocalised electrons.
What are the properties of metallic bonding?
Can conduct electricity and heat, high melting and boiling point, ductile/malleable.
Properties of giant covalent lattices?
Insoluble in most solvents, don’t conduct electricity (except graphite), high melting and boiling point.
Properties of simple molecular molecules?
