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Elements are arranged by increasing proton number.
They have the same number of outer electrons.
Atomic radius decreases due to increased nuclear charge.
Atomic radius increases due to added electron shells.
Minimum energy to remove one mole of electrons from gaseous atoms.
It increases due to decreasing atomic radius.
Increasing atomic radius and electron shielding.
A large jump between successive ionisation energies.
An electron is removed from a higher energy level.
Repulsion within the 2p orbital from paired electrons.
A lattice of positive ions surrounded by delocalised electrons.
Greater charge leads to stronger attractive forces.
Larger ions produce weaker attraction due to lower charge density.
Delocalised electrons move freely, carrying charge.
Uniform layers of positive ions can slide over each other.
Strong electrostatic forces require significant energy to overcome.
Diamond has a rigid structure with each carbon bonded to four others.
Delocalised electrons move between layers of carbon atoms.
Weak van der Waals forces allow layers to slide easily.
A single layer of carbon atoms arranged in a hexagonal pattern.
They peak due to differences in bond strength and structure.
Melting points increase with greater positive charge of ions.
It increases due to additional electron shells.
Increased shielding and atomic radius make outer electrons easier to lose.
Metal hydroxides and hydrogen gas.
The reaction is faster with steam due to extra energy.
Metal chlorides, which are white precipitates.
They form metal oxides, often vigorously.