RRB Group D General Science - Chemistry Syllabus

General Science - Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for General Science - Chemistry in RRB Group D, not a summary of it.

1. 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. 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. 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

General Science - Chemistry flashcards for RRB Group D

19 of 50 cards from the General Science - Chemistry deck — real questions with worked 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.

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