Scottish National 5 (Nat 5) Chemistry Syllabus

Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry in Scottish National 5 (Nat 5), not a summary of it.

1. 1

   Chemical Changes and Structure

   4 topics

   • Rates of Reaction
     • Collision theory and factors affecting rate
     • Calculating average rate
   • Atomic Structure and Bonding
     • Subatomic particles and the periodic table
     • Covalent and ionic bonding
     • Structures: molecular, covalent network and ionic lattice
   • Formulae and Reacting Quantities
     • Chemical formulae and balancing equations
     • The mole and gram formula mass calculations
   • Acids and Bases
     • pH scale and concentration of ions
     • Neutralisation and salt formation
2. 2

   Nature's Chemistry

   4 topics

   • Homologous Series
     • Alkanes, alkenes and cycloalkanes
     • Naming and structural formulae
   • Everyday Consumer Products
     • Alcohols and carboxylic acids
   • Energy from Fuels
     • Combustion and energy released calculations
   • Reactions of Hydrocarbons
     • Addition reactions and the test for unsaturation
3. 3

   Chemistry in Society

   4 topics

   • Metals and Reactivity
     • Reactivity series and electrochemical cells
     • Redox reactions and ion-electron equations
   • Plastics and Polymers
     • Addition polymerisation and monomers
   • Fertilisers
     • Essential elements and the Haber process
   • Chemical Analysis
     • Practical techniques and percentage calculations

Chemistry flashcards for Scottish National 5 (Nat 5)

21 of 57 cards from the Chemistry deck — real questions with worked answers.

1. In terms of collision theory, what two conditions must particles meet for a successful reaction to occur?

   The particles must collide with each other, and they must collide with sufficient energy (at least the activation energy) and the correct orientation.

2. Define the term 'activation energy' ($E_a$).

   Activation energy is the minimum kinetic energy that colliding particles must have in order to react and form products.

3. State four factors that increase the rate of a chemical reaction.

   Increasing concentration, increasing temperature, increasing surface area (smaller particle size), and adding a catalyst.

4. How does a catalyst speed up a reaction, and what happens to it during the reaction?

   A catalyst provides an alternative reaction pathway with a lower activation energy. It is not used up and remains chemically unchanged at the end of the reaction.

5. Write the formula linking average rate of reaction to change in quantity and time.

   $$\text{average rate} = \frac{\Delta \text{quantity}}{\Delta t}$$ where quantity may be mass, volume or concentration.

6. Why does increasing temperature increase reaction rate (in terms of particles)?

   At higher temperature particles move faster and have more kinetic energy, so collisions are more frequent and a greater proportion of collisions have energy equal to or greater than the activation energy.

7. What are the relative charge and relative mass of a proton, neutron and electron?

   Proton: charge $+1$, mass $1$. Neutron: charge $0$, mass $1$. Electron: charge $-1$, mass approximately $0$ (negligible).

8. Define 'atomic number' and 'mass number'.

   Atomic number is the number of protons in an atom (it identifies the element). Mass number is the total number of protons plus neutrons in an atom.

9. What are isotopes?

   Isotopes are atoms of the same element (same number of protons / atomic number) that have different numbers of neutrons, and therefore different mass numbers.

10. Explain how a covalent bond holds two atoms together.

    A covalent bond forms when two non-metal atoms share one or more pairs of electrons; the bond is the electrostatic attraction between the positive nuclei and the shared (negative) electron pair.

11. Describe the structure and bonding in an ionic compound.

    An ionic compound consists of a giant lattice of oppositely charged ions held together by strong electrostatic forces of attraction between positive metal ions and negative non-metal ions.

12. Why do ionic compounds conduct electricity when molten or in solution but not when solid?

    When molten or dissolved, the ions are free to move and carry charge. In the solid state the ions are held fixed in the lattice and cannot move, so no current flows.

13. Distinguish between a covalent molecular and a covalent network substance, giving an example of each.

    Covalent molecular substances have discrete molecules with weak forces between them (e.g. $\ce{CO2}$), giving low melting points. Covalent network substances form a giant lattice of strong covalent bonds throughout (e.g. diamond / $\ce{SiO2}$), giving very high melting points.

14. Calculate the relative formula mass of magnesium nitrate, $\ce{Mg(NO3)2}$. (Use $\ce{Mg}=24$, $\ce{N}=14$, $\ce{O}=16$.)

    $$24 + 2\times(14 + 3\times16) = 24 + 2\times62 = 148$$

15. State the formula relating number of moles, mass and gram formula mass (molar mass).

    $$n = \frac{m}{\text{GFM}}$$ where $n$ is moles, $m$ is mass in grams and GFM is the gram formula mass in $\text{g mol}^{-1}$.

16. Write the equation linking moles, concentration and volume of a solution.

    $$n = C \times V$$ where $n$ is moles, $C$ is concentration in $\text{mol L}^{-1}$ and $V$ is volume in litres.

17. Calculate the number of moles in $\ce{20 g}$ of $\ce{NaOH}$ (GFM $= 40\ \text{g mol}^{-1}$).

    $$n = \frac{m}{\text{GFM}} = \frac{20}{40} = 0.5\ \text{mol}$$

18. Write the ionic formulae of the ions in calcium chloride and give the compound's chemical formula.

    Ions are $\ce{Ca^2+}$ and $\ce{Cl^-}$. To balance charges the formula is $\ce{CaCl2}$.

19. What ion is responsible for acidity, and what is the pH range of an acid?

    The hydrogen ion $\ce{H+}$ (more correctly $\ce{H3O+}$) causes acidity. Acids have a pH less than 7.

20. What ion makes a solution alkaline, and what is the pH of a neutral solution?

    The hydroxide ion $\ce{OH-}$ makes a solution alkaline. A neutral solution has a pH of exactly 7.

21. What happens to the concentration of $\ce{H+}$ and $\ce{OH-}$ ions when an acid is diluted with water?

    Diluting an acid lowers the concentration of $\ce{H+}$ ions, so the pH rises towards 7 (but never reaches or exceeds 7). The $\ce{OH-}$ concentration increases slightly.

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