Inorganic chemistry

Reactivity decreases down Group 7 because the atomic radius and electron shielding increase, making it harder for the nucleus to attract and gain an extra electron. Option B is incorrect because electron affinity generally becomes less exothermic down the group, reflecting this weaker attraction.

Transition metals exhibit variable oxidation states because the energy levels of the 3d and 4s subshells are very close, allowing electrons from both to be lost during chemical reactions. Option A is incorrect because first-row transition metals do not have or use f orbitals for bonding.

Down Group 2, each successive element has an additional occupied electron shell, which increases the overall atomic radius. A diagram for this topic isn't available yet — the worked example below walks the same reasoning step by step.

• !Option A is incorrect because the increasing nuclear charge is shielded by these extra inner shells, preventing the outer electrons from being pulled closer.
• !Option B is incorrect because electron affinity generally becomes less exothermic down the group, reflecting this weaker attraction.
• !Option A is incorrect because first-row transition metals do not have or use f orbitals for bonding.
• !Option B is incorrect because tetrahedral geometry is typically associated with a coordination number of 4.

Answer each from memory — you'll see instantly whether you're right and why.

Run a focused 10-question mini-mock on Inorganic chemistry and see it stick.