Chemistry Exam Review 2018/19

Chemistry Exam Review - 2018/19

• Orbital Filling (Hydrogen Atom): The ground state hydrogen atom fills the 1s orbital.
• Oxidation: A process involving loss of electrons. An example is Zn → Zn²⁺ + 2e⁻.
• Maximum Electrons (L shell): The maximum number of electrons that can occupy the L shell is 8.
• Primary Bond Types: Ionic, covalent, and metallic bonds are the primary bond types.
• Brønsted Bases: Proton acceptors.
• Brønsted Acids: Proton donors.
• Lewis Acids: Electron-pair acceptors.
• Lewis Bases: Electron-pair donors.
• pH Comparison (Solutions A & B): If solution A has a pH of 1, and solution B has a pH of 2, solution B has 10 times the concentration of H⁺ ions as solution A.
• Boiling Point Definition: The temperature at which a liquid changes to a gas when the vapour pressure equals the external pressure.
• Density: A measure of mass per unit volume; an intensive property (g/dm³).
• Gibbs Free Energy Formula: $\Delta G$ = $\Delta H$ - T$\Delta S$, where G= Gibbs free energy, H= enthalpy, T= temperature (K), S = entropy.
• Gibbs Free Energy Definition: The thermodynamic quantity representing energy available to do useful work in a system or process.
• Micelle Definition: An aggregation of surfactant molecules in a liquid colloid, consisting of a hydrophilic head and a hydrophobic tail. Common example is soap.
• Ligand Definition (Complexometry): An ion or molecule attached to a metal atom by coordinate bonding. Common examples include NH₃, Cl⁻, and H₂O.
• Ideal Gas Law Formula: PV=nRT (Pressure x Volume = number of moles x gas constant x Temperature)
• Exothermic vs. Endothermic Reactions: Exothermic reactions release energy, and endothermic reactions absorb energy.
• Isotopes Definition: Atoms with the same atomic number but different mass numbers.
• Colligative Properties: Properties of solutions that depend on the concentration of solute, not its identity e.g., osmotic pressure, boiling point elevation, freezing point depression.
• Ionization Energy: The energy to remove an electron from a gaseous atom; higher from right to left on periodic table.
• Galvanic Cell vs. Electrolysis: Galvanic cells use electrochemical energy to produce electrical current, while electrolysis uses electrical energy to force chemical reactions.
• Bond Order Definition: Half the difference between bonding electrons and antibonding electrons in a molecule. O₂ bond order is 2.
• Arsenic Detection: Arsenic (III) ions can be detected by Griess-Ilosvay reagent.
• Hydrogen Bonding: Hydrogen bonding can occur with molecules containing H directly bonded to highly electronegative atoms such as N, O, and F.
• Substances Existing Only in Solid State at Standard Conditions: The substance CaCO₃ is solid at standard conditions; other possible answers are KMnO₄, I₂ , Br₂ and S.
• Hydrogen Halides (HX): Generally, from HF to HI, the ionic character of the H-X bond increases, and so does the bond energy.
• Solubility: The ability of a substance, (the solute), to dissolve in a solvent.
• Buffer Solution Definition (Example): A solution that resists changes to pH when small amounts of acid or base are added. Examples include CH₃COOH/CH₃COO⁻ and NH₃/NH₄⁺.
• Autocatalysis: Involves a reaction that has one of its products acting as a catalyst.

Prepare for your chemistry exam with this comprehensive review quiz from the 2018/19 academic year. The quiz covers essential topics including orbital filling, oxidation, bond types, and the concepts of acidity and pH. Test your knowledge on key chemistry principles to enhance your understanding and performance.