Examius

🇮🇳 RRB Group D · subject

RRB Group D General Science - Chemistry Syllabus

The General Science - Chemistry syllabus for RRB Group D in full: 3 chapters, 10 topics and 24 sub-topics, every one listed below, plus 50 General Science - Chemistry flashcards with answers.

3Chapters
10Topics
24Sub-topics
50Flashcards

General Science - Chemistry syllabus: all 3 chapters

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

  1. Matter and Its Nature

     3 topics
    • States of Matter
      • Solid, liquid and gas properties
      • Change of state and interconversion
    • Elements, Compounds and Mixtures
      • Pure substances vs mixtures
      • Separation techniques
    • Atomic Structure
      • Atoms, molecules, atomic and mass number
      • Electronic configuration and valency
      • Isotopes and isobars

  2. Periodic Classification and Bonding

     3 topics
    • Periodic Table
      • Groups, periods and periodic trends
      • Metals, non-metals and metalloids
    • Chemical Bonding
      • Ionic and covalent bonds
      • Valency and formula writing
    • Chemical Reactions and Equations
      • Types of chemical reactions
      • Balancing equations
      • Oxidation and reduction

  3. Acids, Bases, Salts and Metals

     4 topics
    • Acids, Bases and Salts
      • Properties and indicators
      • pH scale and neutralization
    • Metals and Non-metals
      • Physical and chemical properties
      • Reactivity series and corrosion
      • Extraction of metals basics
    • Carbon and Its Compounds
      • Allotropes of carbon
      • Hydrocarbons and functional groups
      • Common organic compounds in daily life
    • Everyday Chemistry
      • Common compounds and their uses
      • Fuels and combustion

RRB Group D General Science - Chemistry flashcards — 50 questions with answers

  1. What are the three common states of matter, and what distinguishes them by shape and volume?

    Solid (definite shape and definite volume), Liquid (no definite shape, definite volume), and Gas (no definite shape, no definite volume - takes the shape and volume of its container).

  2. What is the process of a solid changing directly into a gas without becoming a liquid called? Give an example.

    Sublimation. Examples: camphor, naphthalene (mothballs), dry ice (solid CO2), and iodine.

  3. Define melting point and boiling point.

    Melting point is the temperature at which a solid changes into a liquid; boiling point is the temperature at which a liquid changes into a gas. For water at sea level these are 0 C and 100 C respectively.

  4. What is the change of a gas directly into a solid called (the reverse of sublimation)?

    Deposition (also called desublimation), e.g., formation of frost from water vapour.

  5. What is the difference between evaporation and boiling?

    Evaporation is a slow surface phenomenon occurring at any temperature; boiling is a rapid process occurring throughout the liquid only at the boiling point.

  6. What is an element? Give the definition and an example.

    An element is a pure substance made of only one kind of atom that cannot be broken down into simpler substances by chemical means, e.g., hydrogen, oxygen, gold, iron.

  7. What is a compound, and how does it differ from a mixture?

    A compound is a pure substance formed when two or more elements combine chemically in a fixed ratio (e.g., water H2O); a mixture contains two or more substances mixed physically in any ratio with components retaining their properties.

  8. What is the difference between a homogeneous and a heterogeneous mixture? Give an example of each.

    A homogeneous mixture has a uniform composition throughout (e.g., salt solution, air); a heterogeneous mixture has a non-uniform composition with visibly distinct parts (e.g., sand and water, oil and water).

  9. What is an alloy? Give two common examples with their constituents.

    An alloy is a homogeneous mixture of two or more metals (or a metal with a non-metal). Examples: Brass (copper + zinc), Bronze (copper + tin), Steel (iron + carbon).

  10. Which separation technique is used to separate two miscible liquids with different boiling points?

    Distillation (and fractional distillation when boiling points are close), e.g., separating water from alcohol or fractions of crude oil/petroleum.

  11. Name the three subatomic particles of an atom along with their charges.

    Proton (positive charge), Neutron (no charge / neutral), and Electron (negative charge).

  12. Where are protons, neutrons, and electrons located in an atom?

    Protons and neutrons are located in the nucleus (centre); electrons revolve around the nucleus in shells/orbits.

  13. What is the atomic number and the mass number of an atom?

    Atomic number = number of protons in the nucleus; Mass number = number of protons + number of neutrons.

  14. What are isotopes? Give an example.

    Isotopes are atoms of the same element with the same atomic number but different mass numbers (different number of neutrons), e.g., the isotopes of hydrogen: protium, deuterium, and tritium; or Carbon-12 and Carbon-14.

  15. What is the maximum number of electrons that can be held in the first, second, and third shells of an atom?

    The maximum electrons in a shell = 2n2: first shell (K) = 2, second shell (L) = 8, third shell (M) = 18 (though the outermost shell never holds more than 8).

  16. Who proposed the modern periodic law and what is it based on?

    Henry Moseley; the modern periodic law states that the properties of elements are a periodic function of their atomic numbers (not atomic masses as Mendeleev proposed).

  17. What are the horizontal rows and vertical columns of the periodic table called?

    Horizontal rows are called periods; vertical columns are called groups. The modern periodic table has 7 periods and 18 groups.

  18. Where are metals, non-metals, and metalloids located in the periodic table?

    Metals are on the left and centre, non-metals on the upper right, and metalloids (e.g., silicon, boron, germanium) lie along the zig-zag staircase line dividing metals from non-metals.

  19. What is the name and a key property of Group 18 elements?

    Group 18 elements are the noble gases (helium, neon, argon, krypton, xenon, radon). They are chemically inert/unreactive because they have a complete (stable) outermost electron shell.

  20. How does atomic size and metallic character change across a period and down a group?

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

Show the other 30 General Science - Chemistry flashcards

  1. What is a chemical bond, and what are its two main types?

    A chemical bond is the force of attraction that holds atoms together in a molecule. The two main types are ionic (electrovalent) bonds and covalent bonds.

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

    An ionic bond is formed by the complete transfer of electrons from one atom to another, creating oppositely charged ions that attract. Example: sodium chloride (NaCl), where Na loses an electron to Cl.

  3. What is a covalent bond? Give an example.

    A covalent bond is formed by the mutual sharing of electrons between atoms. Example: water (H2O), methane (CH4), oxygen molecule (O2).

  4. What is valency? What is the valency of carbon?

    Valency is the combining capacity of an atom, equal to the number of electrons it loses, gains, or shares to achieve a stable configuration. The valency of carbon is 4 (tetravalent).

  5. What is the octet rule?

    The octet rule states that atoms tend to combine in such a way that they have eight electrons in their outermost (valence) shell, giving them a stable noble-gas configuration.

  6. What is a chemical equation, and what does balancing it ensure?

    A chemical equation is the symbolic representation of a chemical reaction using formulae. Balancing ensures the number of atoms of each element is equal on both sides, satisfying the law of conservation of mass.

  7. Name the main types of chemical reactions.

    Combination (synthesis), Decomposition, Displacement, Double displacement, and Oxidation-reduction (redox) reactions.

  8. What is the difference between an exothermic and an endothermic reaction?

    An exothermic reaction releases heat energy (e.g., burning of fuel, respiration); an endothermic reaction absorbs heat energy (e.g., photosynthesis, decomposition of calcium carbonate).

  9. Define oxidation and reduction in terms of oxygen and hydrogen.

    Oxidation is the gain of oxygen or loss of hydrogen (or loss of electrons); Reduction is the loss of oxygen or gain of hydrogen (or gain of electrons).

  10. What is a displacement reaction? Give an example.

    A reaction in which a more reactive element displaces a less reactive element from its compound. Example: Fe + CuSO4 -> FeSO4 + Cu (iron displaces copper).

  11. What is the difference between an acid and a base in terms of ions produced in water?

    An acid produces hydrogen ions (H+ / hydronium H3O+) in water; a base produces hydroxide ions (OH-) in water. A base that is soluble in water is called an alkali.

  12. What is the pH scale, and what do values below 7, equal to 7, and above 7 indicate?

    The pH scale measures acidity/alkalinity from 0 to 14. pH < 7 is acidic, pH = 7 is neutral (e.g., pure water), and pH > 7 is basic/alkaline.

  13. What is a neutralization reaction? Give the general product.

    A neutralization reaction is the reaction between an acid and a base to form salt and water. General: Acid + Base -> Salt + Water (e.g., HCl + NaOH -> NaCl + H2O).

  14. What colour do litmus, methyl orange behave with acids and bases?

    Acids turn blue litmus red; bases turn red litmus blue. With methyl orange, acids give red/pink and bases give yellow.

  15. Name common acids found in lemon, vinegar, curd (sour milk), and ant sting.

    Lemon - citric acid; Vinegar - acetic acid; Curd/sour milk - lactic acid; Ant sting - formic (methanoic) acid.

  16. What is the chemical name and common use of baking soda and washing soda?

    Baking soda is sodium bicarbonate (NaHCO3), used in cooking and antacids; washing soda is sodium carbonate (Na2CO3.10H2O), used for cleaning and removing water hardness.

  17. List three general physical properties of metals.

    Metals are generally lustrous (shiny), malleable (can be hammered into sheets), ductile (can be drawn into wires), and are good conductors of heat and electricity.

  18. Name two non-metals that are exceptions to typical non-metal properties.

    Carbon in the form of diamond is the hardest natural substance and graphite (also carbon) is a good conductor of electricity, both exceptions to non-metals being soft/non-conductors.

  19. What is the most reactive metal and the least reactive metal commonly cited in the reactivity series?

    Potassium is among the most reactive metals (top of the series); gold is among the least reactive (bottom). Order top to bottom: K > Na > Ca > Mg > Al > Zn > Fe > Pb > H > Cu > Ag > Au.

  20. What is rust, and what conditions are needed for iron to rust?

    Rust is hydrated iron(III) oxide (Fe2O3.xH2O), a reddish-brown coating. Both oxygen (air) and moisture (water) are required for rusting.

  21. What is galvanization?

    Galvanization is the process of coating iron or steel with a thin layer of zinc to protect it from rusting/corrosion.

  22. 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 bond with one another forming long chains, branches, and rings.

  23. What are the main allotropes of carbon?

    Diamond (hardest natural substance), Graphite (soft, conducts electricity), and Fullerenes / Buckminsterfullerene (e.g., C60). All are made of pure carbon.

  24. What are hydrocarbons, and what is the difference between saturated and unsaturated hydrocarbons?

    Hydrocarbons are compounds of carbon and hydrogen only. Saturated hydrocarbons (alkanes) have only single bonds; unsaturated hydrocarbons have double bonds (alkenes) or triple bonds (alkynes).

  25. Give the molecular formula and one use of methane and ethanol.

    Methane is CH4 (main component of natural gas/biogas, used as fuel); Ethanol is C2H5OH (alcohol used in drinks, fuel, and as a solvent/antiseptic).

  26. What is the general molecular formula of alkanes?

    The general formula of alkanes is CnH2n+2 (e.g., methane CH4, ethane C2H6, propane C3H8, butane C4H10).

  27. What is the main constituent of LPG and of CNG used as fuels?

    LPG (Liquefied Petroleum Gas) is mainly butane and propane; CNG (Compressed Natural Gas) is mainly methane.

  28. What gas is released during photosynthesis and what gas is consumed?

    During photosynthesis, plants consume carbon dioxide (CO2) and water and release oxygen (O2), producing glucose using sunlight and chlorophyll.

  29. What is the chemical name of common salt, and chalk/marble (limestone)?

    Common salt is sodium chloride (NaCl); chalk, marble, and limestone are all forms of calcium carbonate (CaCO3).

  30. What gas is mainly responsible for the greenhouse effect and acid rain respectively?

    Carbon dioxide (CO2) is the main greenhouse gas; acid rain is mainly caused by sulphur dioxide (SO2) and nitrogen oxides (NOx) which form sulphuric and nitric acids.

RRB Group D General Science - Chemistry FAQ

What is in the RRB Group D General Science - Chemistry syllabus?

RRB Group D General Science - Chemistry is split into 3 chapters: Matter and Its Nature, Periodic Classification and Bonding and Acids, Bases, Salts and Metals. Together they contain 10 topics and 24 sub-topics.

How many chapters are in RRB Group D General Science - Chemistry?

3 chapters, containing 10 topics and 24 sub-topics. The largest chapter is Acids, Bases, Salts and Metals, with 4 topics.

Are there flashcards for RRB Group D General Science - Chemistry?

Yes — a 50-card General Science - Chemistry 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.