Kerala SSLC Chemistry Sure Questions & Revision Notes

Posted on Feb 18, 2026 in Chemistry

Kerala SSLC Chemistry Sure Questions (Model Papers)

To help you prepare effectively for the Kerala SSLC Chemistry exam, I have analyzed the official SCERT Model Question Papers (Sets A, B, and C). Below are the “Sure Questions” that appear frequently across all sets, followed by Microbit-style short notes designed for quick revision.

Part 1: SSLC Chemistry “Sure Questions” (Based on Model Papers)

Based on the patterns in the provided documents, these topics are guaranteed to carry high weightage:

  • Subshell Electronic Configuration: Writing the configuration for elements like Chromium (Cr, 24) and Copper (Cu, 29) and identifying their Period, Group, and Block.
  • Gas Laws (Numericals): Calculations involving Boyle’s Law (P1V1 = P2V2) and volume/mole conversions at STP (Standard Temperature and Pressure).
  • Mole Concept: Finding the number of moles, mass, or number of molecules (Avogadro’s number) in a given sample.
  • Galvanic & Electrolytic Cells: Identifying the Anode/Cathode, writing cell equations, and understanding the energy change (chemical <–> electrical).
  • Metallurgy (Industrial Production): The Haber Process for Ammonia, the Chlor-alkali process for NaOH, and the extraction of Iron in a Blast Furnace.
  • Organic Nomenclature: Giving IUPAC names for branched alkanes and identifying functional groups or isomers (position, functional, and metamerism).

Part 2: Microbit-Style Short Notes (Ready to Study)

⚡ Periodic Table & Electrons

  • Shells vs. Subshells: Electrons are filled in subshells (s, p, d, f).
  • Energy Order: Follows the n + l rule. Subshells with lower n + l are filled first (e.g., 4s is filled before 3d because 4 + 0 = 4 < 3 + 2 = 5).
  • Special Cases:
    • Cr (24): [Ar] 3d5 4s1 (Half-filled d-subshell is more stable).
    • Cu (29): [Ar] 3d10 4s1 (Completely filled d-subshell is more stable).

🎈 Gas Laws & Moles

  • Boyle’s Law: V ∝ 1/P (at constant T). If pressure increases, volume decreases.
  • Charles’s Law: V ∝ T (at constant P). If temperature increases, volume increases.
  • STP Constants:
    • 1 mole of any gas = 22.4 Litres.
    • 1 mole = 6.022 × 1023 molecules.

🔋 Electrochemistry

  • Galvanic Cell: Chemical energy → Electrical energy.
  • Anode: Oxidation (Loss of e–). The more reactive metal.
  • Cathode: Reduction (Gain of e–). The less reactive metal.
  • Electrolytic Cell: Electrical energy → Chemical energy.

🛠 Metallurgy & Reactions

  • Concentration Methods:
    • Levigation: Based on density differences (ore is heavier).
    • Froth Flotation: For sulphide ores (ore is lighter/attracted to oil).
  • Industrial Chemicals:
    • Ammonia: N2 + 3H2 ⇌ 2NH3 + heat. Use high pressure and 450°C.
    • Iron: Reducing agent is CO (carbon monoxide). Limestone is added as a flux to remove impurities (gangue).

🧪 Organic Chemistry

  • Functional Groups:
    • -OH: Alcohol (Suffix: -ol).
    • -CHO: Aldehyde (Suffix: -al).
    • -COOH: Carboxylic acid (Suffix: -oic acid).
  • Isomerism:
    • Chain Isomers: Different arrangement of carbon skeleton.
    • Position Isomers: Functional group attached to different carbon atoms.
    • Metamerism: Different alkyl groups on either side of the functional group (common in ethers).

Exam Strategy Tip

Always use your 15-minute cool-off time to read the choice questions (A or B). Choose the one where you can write the full chemical equation, as these carry the most precise marks.

Note on PDF: As an AI, I provide the content here which you can easily Print to PDF or Copy–Paste into a document. This format ensures you have the most up-to-date points based on your specific uploaded files.

Good luck with your exams!