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🇵🇰 ETEA Engineering Test · subject
ETEA Engineering Test Chemistry Syllabus
Every chapter and topic of Chemistry examined in ETEA Engineering Test — 11 chapters, 30 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 ETEA Engineering Test, not a summary of it.
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Stoichiometry and Atomic Structure
3 topics- Mole Concept and Stoichiometry
- Atomic Models and Quantum Numbers
- Electronic Configuration
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States of Matter
3 topics- Gas Laws and Kinetic Theory
- Liquids and Intermolecular Forces
- Solids and Crystal Structure
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Chemical Bonding
3 topics- Ionic and Covalent Bonding
- Hybridization and Molecular Geometry
- Dipole Moment and Bond Energy
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Thermochemistry and Energetics
2 topics- Enthalpy and Heat of Reaction
- Hess's Law
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Chemical Equilibrium
3 topics- Law of Mass Action and Kc
- Le Chatelier's Principle
- Ionic Equilibria and pH
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Reaction Kinetics
2 topics- Rate of Reaction and Order
- Factors Affecting Rate and Catalysis
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Electrochemistry
3 topics- Oxidation-Reduction Reactions
- Electrolytic and Galvanic Cells
- Electrode Potential
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Periodic Table and Periodicity
2 topics- Periodic Law and Trends
- s, p and d Block Elements
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Fundamentals of Organic Chemistry
2 topics- Classification and Nomenclature
- Hydrocarbons
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Functional Groups
4 topics- Alkyl Halides
- Alcohols and Phenols
- Aldehydes and Ketones
- Carboxylic Acids
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Macromolecules and Industrial Chemistry
3 topics- Polymers
- Carbohydrates, Proteins and Lipids
- Environmental and Industrial Chemistry
Chemistry flashcards for ETEA Engineering Test
21 of 50 cards from the Chemistry deck — real questions with worked answers.
What is Avogadro's number, and what does one mole represent?
Avogadro's number is $N_A = 6.022 \times 10^{23}$. One mole is the amount of substance containing $6.022 \times 10^{23}$ elementary entities (atoms, molecules, ions, etc.).
Write the formula relating number of moles ($n$) to mass ($m$) and molar mass ($M$).
$$n = \frac{m}{M}$$ where $m$ is mass in grams and $M$ is molar mass in $\text{g mol}^{-1}$.
What volume does 1 mole of any ideal gas occupy at STP?
$22.414\ \text{dm}^3$ (i.e. $22.4\ \text{L}$) at STP ($0\,^{\circ}\text{C}$, $1\ \text{atm}$).
In a chemical reaction, what is the limiting reactant?
The reactant that is completely consumed first, thereby limiting the amount of product formed. It is identified by comparing mole ratios of reactants to the balanced equation.
How do you calculate the number of molecules in a given number of moles $n$?
$$\text{Number of molecules} = n \times N_A = n \times 6.022 \times 10^{23}$$
State the postulates of Bohr's atomic model regarding electron orbits.
Electrons revolve in fixed circular orbits (stationary states) without radiating energy; angular momentum is quantized as $mvr = \frac{nh}{2\pi}$; energy is emitted or absorbed only when an electron jumps between orbits.
What are the four quantum numbers and what does each describe?
Principal ($n$): energy/shell size; Azimuthal ($l$): subshell/shape; Magnetic ($m_l$): orbital orientation; Spin ($m_s = \pm\frac{1}{2}$): direction of electron spin.
For a given principal quantum number $n$, what values can the azimuthal quantum number $l$ take?
$l = 0, 1, 2, \ldots, (n-1)$, corresponding to $s, p, d, f$ subshells respectively.
How many orbitals and electrons can a subshell with azimuthal quantum number $l$ hold?
Number of orbitals $= 2l+1$; maximum electrons $= 2(2l+1)$. E.g. for $l=1$ (p): 3 orbitals, 6 electrons.
State the Heisenberg Uncertainty Principle as a formula.
$$\Delta x \cdot \Delta p \geq \frac{h}{4\pi}$$ It is impossible to simultaneously determine the exact position and momentum of an electron.
State the Aufbau principle for filling electronic orbitals.
Electrons fill orbitals in order of increasing energy (lowest energy first). The order follows the $(n+l)$ rule; for equal $(n+l)$, the orbital with lower $n$ fills first.
State the Pauli Exclusion Principle.
No two electrons in an atom can have the same set of all four quantum numbers; an orbital holds at most 2 electrons with opposite spins.
State Hund's rule of maximum multiplicity.
Electrons occupy degenerate (equal-energy) orbitals singly with parallel spins before any orbital is doubly occupied, minimizing electron repulsion.
Write the ground-state electronic configuration of chromium ($Z=24$) and explain its anomaly.
$\text{[Ar]}\,3d^{5}\,4s^{1}$. A half-filled $3d^5$ and half-filled $4s^1$ give extra stability, so one $4s$ electron shifts to $3d$.
State the ideal gas equation with each symbol defined.
$$PV = nRT$$ $P$ = pressure, $V$ = volume, $n$ = moles, $R = 0.0821\ \text{L atm mol}^{-1}\text{K}^{-1}$ (gas constant), $T$ = absolute temperature in K.
State Boyle's law and Charles's law.
Boyle's law: at constant $T$ and $n$, $V \propto \frac{1}{P}$ (so $PV = \text{constant}$). Charles's law: at constant $P$ and $n$, $V \propto T$ (so $\frac{V}{T} = \text{constant}$).
State Dalton's law of partial pressures.
The total pressure of a mixture of non-reacting gases equals the sum of partial pressures: $$P_{\text{total}} = P_1 + P_2 + P_3 + \cdots$$
According to kinetic molecular theory, how is the average kinetic energy of gas molecules related to temperature?
Average kinetic energy is directly proportional to absolute temperature: $$\overline{KE} = \frac{3}{2}kT$$ where $k$ is the Boltzmann constant. It is independent of the gas's identity.
What is the root-mean-square speed of gas molecules?
$$u_{rms} = \sqrt{\frac{3RT}{M}}$$ It increases with temperature and decreases with molar mass $M$.
Define vapour pressure of a liquid and how it relates to boiling point.
Vapour pressure is the pressure exerted by vapour in equilibrium with its liquid at a given temperature. A liquid boils when its vapour pressure equals the external (atmospheric) pressure.
List the three main types of intermolecular forces in order of increasing strength.
London dispersion forces < dipole-dipole forces < hydrogen bonding. (All are weaker than ionic or covalent bonds.)
Planning Chemistry for ETEA Engineering Test
Chemistry is about 23% of the ETEA Engineering Test syllabus by topic count — 30 of 130 topics, spread over 11 chapters. At roughly 45 minutes per topic plus 12 minutes per sub-topic, a first pass runs to about 25 hours.
The heaviest chapters are Functional Groups (4 topics), Stoichiometry and Atomic Structure (3 topics), States of Matter (3 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 (ETEA Engineering Test) FAQ
What is in the ETEA Engineering Test Chemistry syllabus?
Chemistry is split into 11 chapters — Stoichiometry and Atomic Structure, States of Matter, Chemical Bonding, Thermochemistry and Energetics, Chemical Equilibrium and Reaction Kinetics, and 5 more, containing 30 topics and 0 sub-topics in total.
How many chapters are there in Chemistry for ETEA Engineering Test?
11 chapters. Chemistry accounts for about 23% of the topics in the whole ETEA Engineering Test syllabus (30 of 130).
How long should I spend on Chemistry for ETEA Engineering Test?
Budget around 25 hours for a first pass through Chemistry — about 45 minutes per topic plus 12 minutes per sub-topic across its 30 topics. Add revision cycles on top.
Are there flashcards for ETEA Engineering Test 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.