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NDA Examination Chemistry (General Ability Test - General Knowledge) Syllabus

The Chemistry (General Ability Test - General Knowledge) syllabus for NDA Examination in full: 4 chapters, 13 topics and 23 sub-topics, every one listed below, plus 50 Chemistry (General Ability Test - General Knowledge) flashcards with answers.

4Chapters
13Topics
23Sub-topics
50Flashcards

Chemistry (General Ability Test - General Knowledge) syllabus: all 4 chapters

Expand any chapter to see its topics and sub-topics.

  1. Matter and Its Composition

     3 topics
    • Physical and Chemical Changes
      • Distinguishing changes with examples
    • Elements, Mixtures and Compounds
      • Properties and differences
      • Symbols, formulae and equations
    • Laws of Chemical Combination
      • Law of conservation of mass
      • Law of constant proportions

  2. Atomic Structure and Periodic Classification

     3 topics
    • Structure of the Atom
      • Electrons, protons and neutrons
      • Atomic number and mass number
      • Isotopes and isobars
    • Chemical Bonding
      • Valency
      • Ionic and covalent bonds
    • Periodic Table
      • Groups and periods
      • Metals, non-metals and metalloids

  3. Chemical Reactions and Solutions

     4 topics
    • Acids, Bases and Salts
      • Properties and indicators
      • pH scale and neutralization
    • Oxidation and Reduction
      • Redox reactions
    • Common Industrial Processes
      • Preparation of oxygen, hydrogen and carbon dioxide
      • Rusting, combustion and rancidity
    • Carbon and Its Compounds
      • Allotropes of carbon
      • Fuels and combustion

  4. Applied and Everyday Chemistry

     3 topics
    • Fertilizers
      • Natural and artificial fertilizers
    • Materials and Products
      • Glass, soap and paper
      • Cement, paints and plastics
    • Explosives and Safety Materials
      • Gun powder and common explosives

NDA Examination Chemistry (General Ability Test - General Knowledge) flashcards — 50 questions with answers

  1. What is the key difference between a physical change and a chemical change?

    A physical change alters only physical properties (shape, state, size) with no new substance formed and is usually reversible, e.g. melting ice. A chemical change forms one or more new substances with different properties, is usually irreversible, and involves energy change, e.g. rusting of iron.

  2. Give two examples each of a physical change and a chemical change.

    Physical changes: melting of ice, dissolving sugar in water, boiling water, magnetising iron. Chemical changes: burning of paper, rusting of iron, curdling of milk, digestion of food.

  3. What is the difference between an element, a compound, and a mixture?

    An element is a pure substance made of only one kind of atom (e.g. oxygen, gold). A compound is a pure substance made of two or more elements chemically combined in a fixed ratio (e.g. water, H2O). A mixture is two or more substances physically combined in any ratio, retaining their properties (e.g. air, salt solution).

  4. What is the difference between a homogeneous and a heterogeneous mixture?

    A homogeneous mixture has a uniform composition throughout with no visible boundaries between components (e.g. salt solution, air). A heterogeneous mixture has a non-uniform composition with distinguishable parts (e.g. sand and iron filings, oil and water).

  5. State the Law of Conservation of Mass and who proposed it.

    Proposed by Antoine Lavoisier, it states that in a chemical reaction matter is neither created nor destroyed; the total mass of reactants equals the total mass of products.

  6. State the Law of Constant (Definite) Proportions.

    Proposed by Joseph Proust, it states that a given chemical compound always contains its constituent elements in a fixed ratio by mass, regardless of its source or method of preparation. E.g. water always has H and O in a 1:8 mass ratio.

  7. State the Law of Multiple Proportions.

    Proposed by John Dalton, it states that when two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other are in a simple whole-number ratio. E.g. in CO and CO2 the oxygen ratio is 1:2.

  8. State Gay-Lussac's Law of Gaseous Volumes and Avogadro's Law.

    Gay-Lussac's Law: when gases react, they do so in volumes that bear a simple whole-number ratio to each other and to the products, measured at the same temperature and pressure. Avogadro's Law: equal volumes of all gases at the same temperature and pressure contain equal numbers of molecules.

  9. Name the three fundamental subatomic particles, their charges, and their discoverers.

    Electron (negative charge, discovered by J.J. Thomson), Proton (positive charge, discovered by Goldstein/Rutherford), and Neutron (no charge/neutral, discovered by James Chadwick).

  10. What did Rutherford's alpha-particle scattering experiment conclude about atomic structure?

    It showed that an atom is mostly empty space, with a tiny, dense, positively charged nucleus at the centre containing nearly all the mass, and electrons revolving around it. Most alpha particles passed straight through; a few were deflected by the nucleus.

  11. Define atomic number and mass number.

    Atomic number (Z) is the number of protons in the nucleus of an atom (equal to electrons in a neutral atom). Mass number (A) is the total number of protons plus neutrons in the nucleus.

  12. What are isotopes, isobars, and isotones?

    Isotopes: atoms of the same element with the same atomic number but different mass numbers (different neutrons), e.g. C-12 and C-14. Isobars: atoms of different elements with the same mass number but different atomic numbers, e.g. Ar-40 and Ca-40. Isotones: atoms with the same number of neutrons.

  13. What is the maximum number of electrons in a shell, and what is the formula?

    The maximum number of electrons in a shell is given by 2n^2, where n is the shell number. Thus K shell (n=1) holds 2, L shell (n=2) holds 8, M shell (n=3) holds 18, and N shell (n=4) holds 32 electrons.

  14. State the octet rule and the duplet rule.

    The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable configuration of 8 electrons in their outermost shell (like noble gases). The duplet rule applies to light atoms (H, He, Li) which become stable with 2 electrons in the outer shell.

  15. What is an ionic (electrovalent) bond? Give an example.

    An ionic bond is formed by the complete transfer of one or more electrons from a metal atom to a non-metal atom, producing oppositely charged ions held together by electrostatic attraction. Example: NaCl, where Na loses an electron to Cl.

  16. What is a covalent bond and what are its types?

    A covalent bond is formed by the mutual sharing of electron pairs between atoms (usually non-metals). Types: single bond (one shared pair, e.g. H2), double bond (two shared pairs, e.g. O2), and triple bond (three shared pairs, e.g. N2).

  17. Compare the general properties of ionic and covalent compounds.

    Ionic compounds: high melting/boiling points, usually solid, soluble in water, conduct electricity when molten or in solution. Covalent compounds: low melting/boiling points, often liquids or gases, generally insoluble in water, poor conductors of electricity.

  18. Who proposed the modern periodic law and what does it state?

    Henry Moseley proposed the modern periodic law, which states that the physical and chemical properties of elements are a periodic function of their atomic numbers. (Mendeleev's earlier law was based on atomic mass.)

  19. How many periods and groups are there in the modern periodic table?

    The modern periodic table has 7 horizontal periods (rows) and 18 vertical groups (columns). Elements are arranged in order of increasing atomic number.

  20. How do atomic size and metallic character vary across a period and down a group?

    Across a period (left to right): atomic size decreases and metallic character decreases (non-metallic character increases). Down a group (top to bottom): atomic size increases and metallic character increases.

Show the other 30 Chemistry (General Ability Test - General Knowledge) flashcards

  1. What are the common names for Group 1, Group 2, Group 17, and Group 18 elements?

    Group 1: alkali metals; Group 2: alkaline earth metals; Group 17: halogens; Group 18: noble (inert) gases.

  2. How do acids and bases taste, and how do they affect litmus paper?

    Acids taste sour and turn blue litmus red. Bases taste bitter, feel soapy/slippery, and turn red litmus blue. Neutral substances do not change litmus colour.

  3. What is the pH scale and what do its values indicate?

    The pH scale runs from 0 to 14 and measures the acidity or basicity of a solution. pH 7 is neutral, pH less than 7 is acidic, and pH greater than 7 is basic (alkaline). Lower pH means stronger acid; higher pH means stronger base.

  4. What is a neutralization reaction? Give the general equation.

    Neutralization is the reaction between an acid and a base to form a salt and water. General equation: Acid + Base -> Salt + Water. Example: HCl + NaOH -> NaCl + H2O. It is an exothermic reaction.

  5. Distinguish between a strong acid and a weak acid with examples.

    A strong acid ionizes completely in water releasing many H+ ions (e.g. HCl, H2SO4, HNO3). A weak acid ionizes only partially releasing fewer H+ ions (e.g. acetic acid CH3COOH, carbonic acid H2CO3).

  6. Name the acids present in vinegar, lemon, sour milk, and ant sting.

    Vinegar: acetic acid; Lemon/citrus: citric acid; Sour milk (curd): lactic acid; Ant sting: formic acid (methanoic acid).

  7. What is a salt, and what type of salt is common table salt?

    A salt is an ionic compound formed when the hydrogen of an acid is replaced by a metal (or formed from acid-base neutralization). Common table salt is sodium chloride (NaCl), formed from the strong acid HCl and the strong base NaOH, so it is neutral.

  8. What is oxidation and reduction in terms of oxygen, hydrogen, and electrons?

    Oxidation is gain of oxygen, loss of hydrogen, or loss of electrons. Reduction is loss of oxygen, gain of hydrogen, or gain of electrons. Both occur together in a redox reaction.

  9. What is a redox reaction? Identify the oxidizing and reducing agents.

    A redox reaction is one in which oxidation and reduction occur simultaneously. The oxidizing agent gets reduced (gains electrons) and the reducing agent gets oxidized (loses electrons). Example: in 2Mg + O2 -> 2MgO, Mg is reduced (oxidizing agent is O2) and O2 is the oxidizer while Mg is the reducer.

  10. What is corrosion and rusting? Give the formula of rust.

    Corrosion is the slow eating up of a metal surface by air, moisture, or chemicals. Rusting is the corrosion of iron forming a reddish-brown layer of hydrated iron(III) oxide, Fe2O3.xH2O, in the presence of oxygen and water.

  11. Name the industrial process for manufacturing ammonia and its conditions.

    The Haber process manufactures ammonia (NH3) from nitrogen and hydrogen: N2 + 3H2 -> 2NH3. It uses high pressure (about 200 atm), a temperature of about 450 C, and an iron catalyst.

  12. Name the industrial process used to manufacture sulphuric acid.

    The Contact process is used to manufacture sulphuric acid (H2SO4). It involves oxidizing SO2 to SO3 using a vanadium pentoxide (V2O5) catalyst, then dissolving SO3 to form oleum and finally H2SO4.

  13. What is the Solvay process used to manufacture?

    The Solvay process is used to manufacture sodium carbonate (washing soda, Na2CO3) from brine (NaCl), ammonia, and carbon dioxide. It is also called the ammonia-soda process.

  14. Why is carbon called tetravalent and what is catenation?

    Carbon is tetravalent because it has 4 valence electrons and forms 4 covalent bonds. Catenation is the unique ability of carbon atoms to link with one another forming long chains, branched chains, and rings, which leads to a vast number of carbon compounds.

  15. What are the major allotropes of carbon and a key property of each?

    Diamond: hardest natural substance, each carbon bonded to 4 others, non-conductor. Graphite: soft, slippery, good conductor of electricity, each carbon bonded to 3 others. Fullerene (e.g. C60/buckyball): spherical molecular form of carbon.

  16. What are hydrocarbons, and how do saturated and unsaturated hydrocarbons differ?

    Hydrocarbons are compounds made of only carbon and hydrogen. Saturated hydrocarbons (alkanes) have only single C-C bonds (e.g. methane CH4). Unsaturated hydrocarbons have double bonds (alkenes, e.g. ethene C2H4) or triple bonds (alkynes, e.g. ethyne C2H2).

  17. Give the molecular formulas of methane, ethane, ethene, and ethyne.

    Methane: CH4; Ethane: C2H6; Ethene (ethylene): C2H4; Ethyne (acetylene): C2H2.

  18. What are the general formulas of alkanes, alkenes, and alkynes?

    Alkanes: CnH2n+2; Alkenes: CnH2n; Alkynes: CnH2n-2 (where n is the number of carbon atoms).

  19. What is the chemical formula and common use of ethanol and methanol?

    Ethanol (C2H5OH) is the alcohol in alcoholic drinks, used as a solvent and fuel additive. Methanol (CH3OH) is highly toxic, used as an industrial solvent and fuel; consumption can cause blindness or death.

  20. What are the three primary nutrients supplied by fertilizers, and which element does each provide?

    The three primary nutrients are Nitrogen (N) for leafy growth, Phosphorus (P) for root and flower development, and Potassium (K) for overall plant health and disease resistance. They are referred to as N-P-K fertilizers.

  21. Name three common nitrogenous fertilizers.

    Common nitrogenous fertilizers include urea [CO(NH2)2], ammonium nitrate (NH4NO3), ammonium sulphate [(NH4)2SO4], and calcium ammonium nitrate (CAN). Urea has the highest nitrogen content among solid fertilizers (about 46%).

  22. What is the difference between a fertilizer and a manure?

    A fertilizer is a man-made (inorganic) chemical substance rich in specific plant nutrients, fast-acting but adds no humus. A manure is a natural organic substance from decomposed plant/animal waste, nutrient-poor per unit but improves soil texture and adds humus.

  23. What are the chemical names and formulas of baking soda, washing soda, and bleaching powder?

    Baking soda: sodium hydrogen carbonate, NaHCO3. Washing soda: sodium carbonate decahydrate, Na2CO3.10H2O. Bleaching powder: calcium oxychloride, CaOCl2.

  24. What is the chemical name and formula of plaster of Paris, and what is its main use?

    Plaster of Paris is calcium sulphate hemihydrate, CaSO4.1/2H2O. It is used for setting fractured bones in casts, making moulds, and decorative items; it hardens when mixed with water to form gypsum.

  25. What are the chief constituents of glass, and what is added to make it heat-resistant?

    Ordinary glass is made chiefly from silica (sand, SiO2), sodium carbonate (soda), and calcium carbonate (limestone). Adding boron oxide produces heat-resistant borosilicate glass (e.g. Pyrex).

  26. What is the difference between thermoplastics and thermosetting plastics? Give examples.

    Thermoplastics soften on heating and can be remoulded repeatedly (e.g. polythene, PVC, polystyrene). Thermosetting plastics set permanently on heating and cannot be remoulded once formed (e.g. bakelite, melamine).

  27. What are alloys? Name the constituents of brass, bronze, and steel.

    Alloys are homogeneous mixtures of two or more metals (or a metal and a non-metal). Brass = copper + zinc; Bronze = copper + tin; Steel = iron + carbon (stainless steel also contains chromium and nickel).

  28. Name the explosive substances TNT, RDX, and gunpowder by their composition or nature.

    TNT is trinitrotoluene, a common military high explosive. RDX (cyclonite) is a powerful high explosive used in bombs. Gunpowder is a low explosive mixture of potassium nitrate (saltpetre), charcoal, and sulphur.

  29. What is dynamite and who invented it?

    Dynamite is an explosive made by absorbing nitroglycerine into an inert porous material (like kieselguhr) to make it stable and safe to handle. It was invented by Alfred Nobel.

  30. What is the difference between a high explosive and a low (deflagrating) explosive?

    A high explosive detonates with a supersonic shock wave producing a sudden, violent blast (e.g. TNT, RDX, nitroglycerine). A low explosive deflagrates (burns rapidly, subsonic) and is used as a propellant (e.g. gunpowder).

NDA Examination Chemistry (General Ability Test - General Knowledge) FAQ

What is in the NDA Examination Chemistry (General Ability Test - General Knowledge) syllabus?

NDA Examination Chemistry (General Ability Test - General Knowledge) is split into 4 chapters: Matter and Its Composition, Atomic Structure and Periodic Classification, Chemical Reactions and Solutions and Applied and Everyday Chemistry. Together they contain 13 topics and 23 sub-topics.

How many chapters are in NDA Examination Chemistry (General Ability Test - General Knowledge)?

4 chapters, containing 13 topics and 23 sub-topics. The largest chapter is Chemical Reactions and Solutions, with 4 topics.

Are there flashcards for NDA Examination Chemistry (General Ability Test - General Knowledge)?

Yes — a 50-card Chemistry (General Ability Test - General Knowledge) deck, printed in full in the flashcards section of this page and available in the Examius app with spaced repetition. The free plan covers one exam of your choice, including its flashcards; Examius Pro, a one-time purchase, unlocks every other exam and deck.