Look inside the OCR A-Level Chemistry A guide (H432)

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Look inside the OCR A-Level Chemistry A guide

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OCR · A-Level · H432
Chemistry A
Active Recall Guide
1,913 questions
Chemistry AContents
Contents
17 sections, 160 subtopics
  1. Foundations in Chemistry284
  2. Bonding and Structure117
  3. Periodic Table and Energy177
  4. Enthalpy Changes89
  5. Chemical Equilibrium36
  6. Basic Concepts of Organic Chemistry82
  7. Core Organic Chemistry116
  8. Alkenes86
  9. Organic Synthesis52
  10. How Fast?107
  11. Physical Chemistry and Transition Elements101
  12. Acids, Bases and Buffers120
  13. and 5 more
ii
Bonding and StructureQuestions
Bonding and Structure
Ionic bonding and the properties of ionic compounds
  1. What is an ionic bond?
  2. What type of force holds ions together in an ionic lattice?
  3. Describe the structure of ionic compounds.
  4. Why do ionic compounds have high melting and boiling points?
  5. Why do solid ionic compounds not conduct electricity?
  6. In what physical states can ionic compounds conduct electricity, and why not in the solid state?
  7. Why do ionic compounds conduct electricity when molten?
  8. Why do ionic compounds conduct electricity when dissolved in water?
  9. Explain why ionic compounds are often soluble in polar solvents such as water.
12
Bonding and StructureAnswers
Answers
Ionic bonding and the properties of ionic compounds
  1. The strong electrostatic attraction between oppositely charged ions
  2. Strong electrostatic attraction
  3. Giant ionic lattice structures with ions arranged in a regular repeating three-dimensional pattern
  4. A large amount of energy is required to overcome the strong electrostatic attractions between ions throughout the lattice
  5. The ions are held in fixed positions within the lattice and cannot move
  6. Molten or dissolved in water, because ions are free to move; in the solid state ions are fixed in position and cannot carry charge
  7. The ions become free to move and carry charge
  8. The ions become free to move and carry charge
  9. Polar water molecules can surround and stabilise the ions
13
Core Organic ChemistryQuestions
Core Organic Chemistry
Combustion of alkanes and their reaction with halogens
  1. What products are formed during the complete combustion of an alkane?
  2. What products may form during the incomplete combustion of an alkane?
  3. Why is carbon monoxide produced from incomplete combustion dangerous to humans?
  4. Under what conditions do alkanes react with chlorine or bromine?
  5. What type of reaction occurs between alkanes and halogens in UV light?
  6. Define homolytic fission.
  7. How is a radical represented in chemical notation?
  8. What are the three stages of the radical substitution mechanism?
34
Core Organic ChemistryAnswers
Answers
Combustion of alkanes and their reaction with halogens
  1. Carbon dioxide and water.
  2. Carbon monoxide and/or carbon (soot), along with water.
  3. It is a toxic gas that binds to haemoglobin, preventing oxygen transport in the blood.
  4. When exposed to ultraviolet radiation.
  5. Radical substitution.
  6. The breaking of a covalent bond so that each atom retains one electron from the bonding pair, forming two radicals.
  7. By a single dot (•).
  8. Initiation, propagation, and termination.
35
Redox and Electrode PotentialsQuestions
Redox and Electrode Potentials
Oxidising and reducing agents, and balancing half-equations
  1. What is an oxidising agent?
  2. Why does an oxidising agent become reduced during a reaction?
  3. What is a reducing agent?
  4. Why does a reducing agent become oxidised during a reaction?
  5. In a redox reaction, what happens to the electrons of the reducing agent?
  6. When constructing a redox equation, how do you write the oxidation half-equation?
  7. In balancing a half-equation, how do you balance atoms other than oxygen and hydrogen?
  8. How do you balance oxygen atoms in a half-equation?
  9. How do you balance hydrogen atoms in a half-equation?
56
Redox and Electrode PotentialsAnswers
Answers
Oxidising and reducing agents, and balancing half-equations
  1. A species that accepts electrons from another species, causing that species to be oxidised, while the oxidising agent itself is reduced.
  2. Because it accepts electrons from another species, and gaining electrons is the definition of reduction.
  3. A species that donates electrons to another species, causing that species to be reduced, while the reducing agent itself is oxidised.
  4. Because it loses electrons to another species, and losing electrons is the definition of oxidation.
  5. The reducing agent loses electrons and is oxidised.
  6. Write the half-equation showing the species that loses electrons, with electrons appearing on the product side.
  7. Add coefficients to ensure the number of each type of atom (excluding O and H) is equal on both sides.
  8. Add water molecules (H₂O) to the side deficient in oxygen atoms.
  9. Add hydrogen ions (H⁺) to the side deficient in hydrogen atoms.
57
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