This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Welcome back — missed you this week. c) i) Step 1: Identify the formula for the oxide of each element in the +4 oxidation state. • Carbon: CO_2 • Silicon: SiO_2 • Germanium: GeO_2 • Tin: SnO_2 • Lead: PbO_2 Step 2: Identify which oxides are amphoteric. Amphoteric oxides react with both acids and bases. • GeO_2, SnO_2, and PbO_2 are amphoteric. Step 3: Identify which oxide is a greenhouse gas. • CO_2 is a greenhouse gas. | Element | Oxide | Amphoteric | A green house gas | | :------ | :---- | :--------- | :---------------- | | C | CO_2 | | | | Si | SiO_2 | | | | Ge | GeO_2 | | | | Sn | SnO_2 | | | | Pb | PbO_2 | | | ii) Step 1: Write the balanced chemical equation for the reaction of germanium tetrachloride (GeCl_4) with water (H_2O). Germanium tetrachloride undergoes hydrolysis to form germanium dioxide and hydrochloric acid. GeCl_4(l) + 2H_2O(l) GeO_2(s) + 4HCl(aq) d) i) A transition metal is an element that has a partially filled d subshell in its atomic or ionic state. ii) A: form complexes Transition metals form complexes because they have vacant d orbitals of suitable energy to accept lone pairs of electrons from ligands. They also have a high charge density and relatively small size, which attracts ligands. B: show variable oxidation states Transition metals show variable oxidation states because the energy levels of their (n-1)d and ns orbitals are very close. This allows electrons from both subshells to be removed with comparable ease, leading to multiple stable oxidation states. Send me the next one 📸