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🇵🇰 FSc Pre-Engineering · subject
FSc Pre-Engineering Chemistry Syllabus
Every chapter and topic of Chemistry examined in FSc Pre-Engineering — 14 chapters, 45 topics, plus 50 flashcards written against it.
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 FSc Pre-Engineering, not a summary of it.
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Basic Concepts of Chemistry
4 topics- Atoms, Molecules and Ions
- The Mole and Avogadro's Number
- Empirical and Molecular Formulae
- Stoichiometry and Limiting Reactant
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States of Matter
3 topics- Gaseous State and Gas Laws
- Liquid State and Intermolecular Forces
- Solid State and Crystal Lattices
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Atomic Structure
4 topics- Sub-Atomic Particles and Rutherford Model
- Bohr's Model and Atomic Spectrum
- Quantum Numbers and Orbitals
- Electronic Configuration
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Chemical Bonding
3 topics- Ionic and Covalent Bonds
- VSEPR Theory and Molecular Geometry
- Hybridization and Bond Theories
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Thermochemistry and Energetics
3 topics- System, Surroundings and Enthalpy
- Hess's Law
- Bond Energies and Heat of Reaction
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Chemical Equilibrium
3 topics- Law of Mass Action and Kc
- Le Chatelier's Principle
- Ionic Product, pH and Buffers
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Reaction Kinetics
3 topics- Rate of Reaction and Order
- Factors Affecting Reaction Rate
- Catalysis
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Electrochemistry
3 topics- Oxidation and Reduction
- Galvanic and Electrolytic Cells
- Electrode Potential and Nernst Equation
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Periodic Classification and s/p-Block Elements
3 topics- Periodic Law and Periodic Trends
- Chemistry of s-Block Elements
- Chemistry of p-Block Elements
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Transition Elements
2 topics- Properties of Transition Metals
- Complex Compounds and Coordination
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Fundamental Principles of Organic Chemistry
3 topics- Classification and Nomenclature
- Functional Groups and Isomerism
- Reaction Mechanisms and Hybridization in Carbon
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Hydrocarbons
3 topics- Alkanes
- Alkenes and Alkynes
- Benzene and Aromatic Compounds
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Functional Group Chemistry
4 topics- Alkyl Halides
- Alcohols, Phenols and Ethers
- Aldehydes and Ketones
- Carboxylic Acids and Derivatives
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Biochemistry and Industrial Chemistry
4 topics- Carbohydrates, Proteins and Lipids
- Enzymes and Nucleic Acids
- Industrial Processes and Polymers
- Environmental Chemistry
Chemistry flashcards for FSc Pre-Engineering
21 of 50 cards from the Chemistry deck — real questions with worked answers.
Define an atom, a molecule, and an ion.
An atom is the smallest particle of an element that can take part in a chemical reaction. A molecule is the smallest particle of a substance (element or compound) that can exist independently and shows all properties of that substance. An ion is an atom or group of atoms carrying a net electric charge (cation = positive, anion = negative).
State the law of conservation of mass and the law of definite proportions.
Law of conservation of mass: matter is neither created nor destroyed in a chemical reaction; total mass of reactants equals total mass of products. Law of definite proportions: a given compound always contains the same elements in the same fixed proportion by mass.
What is the difference between an empirical formula and a molecular formula?
An empirical formula shows the simplest whole-number ratio of atoms in a compound (e.g. $\ce{CH2O}$). A molecular formula shows the actual number of atoms of each element in a molecule (e.g. glucose $\ce{C6H12O6}$). Molecular formula $=$ (empirical formula)$_n$.
What is Avogadro's number, and what does it represent?
Avogadro's number is $N_A = 6.022 \times 10^{23}\ \text{mol}^{-1}$. It is the number of elementary particles (atoms, molecules, ions) present in one mole of a substance.
Define one mole and give the formula relating mass to number of moles.
One mole is the amount of substance containing $6.022 \times 10^{23}$ particles, equal to the substance's molar mass in grams. $$n = \frac{m}{M}$$ where $n$ is moles, $m$ is mass in grams, and $M$ is molar mass in $\text{g mol}^{-1}$.
How do you calculate the number of particles from the number of moles?
Multiply moles by Avogadro's number: $$N = n \times N_A = n \times 6.022 \times 10^{23}$$
What volume does one mole of an ideal gas occupy at STP?
At STP ($0\,^{\circ}\text{C} = 273.15\ \text{K}$ and $1\ \text{atm}$), one mole of any ideal gas occupies a molar volume of $22.4\ \text{dm}^{3}$ (litres).
Outline the steps to determine the empirical formula from percentage composition.
1) Take the percentage of each element as grams. 2) Divide each mass by the element's atomic mass to get moles. 3) Divide all mole values by the smallest. 4) Round to whole numbers (multiply through if needed) to get the simplest atom ratio.
Define stoichiometry and the limiting reactant.
Stoichiometry is the quantitative study of the mole/mass relationships between reactants and products in a balanced chemical equation. The limiting reactant is the reactant that is completely consumed first and therefore determines the maximum amount of product formed; the others are in excess.
Define theoretical yield, actual yield, and percentage yield.
Theoretical yield is the maximum product calculated from stoichiometry. Actual yield is the amount obtained experimentally. $$\text{\% yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100$$
State Boyle's law with its equation.
At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure: $$P \propto \frac{1}{V} \quad\Rightarrow\quad P_1 V_1 = P_2 V_2$$
State Charles's law with its equation.
At constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute (Kelvin) temperature: $$V \propto T \quad\Rightarrow\quad \frac{V_1}{T_1} = \frac{V_2}{T_2}$$
State Avogadro's law.
Equal volumes of all gases, at the same temperature and pressure, contain an equal number of molecules. Equivalently, at constant $T$ and $P$, $V \propto n$.
Write Dalton's law of partial pressures.
The total pressure of a mixture of non-reacting gases equals the sum of the partial pressures of the component gases: $$P_{\text{total}} = P_1 + P_2 + P_3 + \cdots$$
Write the ideal gas equation and identify each term.
$$PV = nRT$$ where $P$ is pressure, $V$ is volume, $n$ is number of moles, $T$ is absolute temperature (K), and $R$ is the general gas constant.
What is the value of the general gas constant $R$ in SI units?
$R = 8.314\ \text{J K}^{-1}\,\text{mol}^{-1}$, equivalently $0.0821\ \text{dm}^{3}\,\text{atm K}^{-1}\,\text{mol}^{-1}$.
Derive the expression for molar mass from the ideal gas equation.
Substituting $n = \frac{m}{M}$ into $PV = nRT$ gives $PV = \frac{m}{M}RT$, so $$M = \frac{mRT}{PV} = \frac{\rho RT}{P}$$ where $\rho$ is the gas density.
State the main postulates of the kinetic molecular theory of gases.
1) Gases consist of tiny particles in constant random motion. 2) The volume of the particles is negligible compared with the container. 3) Intermolecular forces are negligible. 4) Collisions are perfectly elastic (no net energy loss). 5) The average kinetic energy of the particles is directly proportional to absolute temperature.
How is average kinetic energy of gas molecules related to temperature?
The average translational kinetic energy per molecule is directly proportional to absolute temperature: $$\overline{KE} = \frac{3}{2}kT$$ where $k$ is the Boltzmann constant. Per mole, $\overline{KE} = \frac{3}{2}RT$.
State Graham's law of diffusion/effusion.
At constant temperature and pressure, the rate of diffusion (or effusion) of a gas is inversely proportional to the square root of its density (or molar mass): $$\frac{r_1}{r_2} = \sqrt{\frac{M_2}{M_1}} = \sqrt{\frac{\rho_2}{\rho_1}}$$
Define evaporation and explain why it causes cooling.
Evaporation is the escape of high-energy molecules from a liquid surface into the vapour phase below the boiling point. Because the most energetic molecules leave, the average kinetic energy (and thus temperature) of the remaining liquid falls, producing a cooling effect.
Planning Chemistry for FSc Pre-Engineering
Chemistry is about 33% of the FSc Pre-Engineering syllabus by topic count — 45 of 138 topics, spread over 14 chapters. At roughly 45 minutes per topic plus 12 minutes per sub-topic, a first pass runs to about 35 hours.
The heaviest chapters are Basic Concepts of Chemistry (4 topics), Atomic Structure (4 topics), Functional Group Chemistry (4 topics) . Front-load those while your energy is high; the short chapters are better revision filler later.
Work top-down: read the chapter, then tick topics off individually rather than marking the whole chapter done. Sub-topics are where silent gaps hide.
Chemistry (FSc Pre-Engineering) FAQ
What is in the FSc Pre-Engineering Chemistry syllabus?
Chemistry is split into 14 chapters — Basic Concepts of Chemistry, States of Matter, Atomic Structure, Chemical Bonding, Thermochemistry and Energetics and Chemical Equilibrium, and 8 more, containing 45 topics and 0 sub-topics in total.
How many chapters are there in Chemistry for FSc Pre-Engineering?
14 chapters. Chemistry accounts for about 33% of the topics in the whole FSc Pre-Engineering syllabus (45 of 138).
How long should I spend on Chemistry for FSc Pre-Engineering?
Budget around 35 hours for a first pass through Chemistry — about 45 minutes per topic plus 12 minutes per sub-topic across its 45 topics. Add revision cycles on top.
Are there flashcards for FSc Pre-Engineering Chemistry?
Yes — a 50-card Chemistry deck. Sample cards are printed on this page, and the full deck is free in the Examius app with spaced repetition scheduling.