AQA A-Level Chemistry 3.2 Inorganic chemistry overview quiz quiz

More electron shells are steadily added across the period, so each successive atom becomes larger

Shielding from the inner electrons increases far faster than the nuclear charge does

Nuclear charge increases while shielding stays roughly constant, pulling the outer shell in

The atoms steadily gain extra protons but at the same time lose outer electrons

Aluminium has fewer protons in its nucleus than magnesium does, so its nucleus pulls the outer electrons less strongly overall

Aluminium has noticeably more shielding because it has gained a whole extra inner electron shell

Magnesium has an especially stable half-filled sub-shell that makes its electron harder to remove

The electron removed from aluminium is in a higher-energy 3p orbital, partly shielded by 3s, so it is easier to remove

Hydroxides become more soluble while sulfates become less soluble

Both increase down the group

Both decrease down the group

Hydroxides become less soluble while sulfates become more soluble

The atoms lose an outer electron progressively more and more easily as you move down the group from the top to the very bottom

The larger atoms with more shielding attract an incoming electron less strongly, so they gain an electron less easily

Electronegativity steadily increases as you go down the group from fluorine to iodine

The boiling point of the elements increases down the group as the molecules get larger

Sulfur dioxide

Hydrogen chloride

Hydrogen sulfide

Chlorine

A white precipitate

A yellow precipitate

No precipitate

A cream precipitate

It is giant covalent (macromolecular) with many strong covalent bonds to break

It is simple molecular and held together by unusually strong van der Waals forces

It is a giant ionic lattice with strong electrostatic forces between the ions

It is a giant metallic lattice with delocalised electrons holding the cations

Purely basic in character

Amphoteric

Purely acidic in character

Completely neutral

It is not found in the d block of the periodic table at all

It does not form any ions under normal chemical conditions

Its only ion, Zn2+, has a full 3d10 sub-shell, not an incomplete d sub-shell

It has no 4s electrons present at all in its ground-state electron configuration

Electrons jump back and forth between all of the different metal atoms within the lattice structure, and in doing so give off light

The central metal ion simply reflects every wavelength of visible light that falls upon it

The water ligands surrounding the metal ion are themselves intrinsically coloured substances

Ligands split the 3d orbitals; an electron absorbs visible light to be promoted, and the complementary colour is transmitted

Fe3+ has a higher charge density, so it polarises the coordinated water more, releasing more H+

Fe3+ has a much lower charge density than Fe2+, so it polarises the coordinated water less strongly

Fe2+ does not form a hexaaqua complex ion in aqueous solution at all

Fe3+ actively removes hydroxide ions from the surrounding water molecules

A blue precipitate that stays blue and does not redissolve at all in excess sodium hydroxide

A white precipitate that redissolves in excess sodium hydroxide to a colourless solution

A red-brown precipitate that does not dissolve in any excess of sodium hydroxide

A deep blue solution forming straight away without any precipitate appearing first