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Matric (SSC) Chemistry Syllabus
The Chemistry syllabus for Matric (SSC) in full: 16 chapters and 57 topics, every one listed below, plus 51 Chemistry flashcards with answers.
Chemistry syllabus: all 16 chapters
Expand any chapter to see its topics and sub-topics.
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Fundamentals of Chemistry
4 topics- Branches of Chemistry
- Atomic, Molecular and Formula Mass
- The Mole Concept and Avogadro's Number
- Empirical and Molecular Formula
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Structure of Atoms
4 topics- Discovery of Subatomic Particles
- Rutherford and Bohr Atomic Models
- Electronic Configuration
- Isotopes and Their Applications
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Periodic Table and Periodicity of Properties
3 topics- Historical Development of the Periodic Table
- Modern Periodic Table and Periodic Law
- Periodic Trends
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Structure of Molecules
5 topics- Chemical Bond and Why Atoms React
- Ionic and Covalent Bonds
- Coordinate Covalent and Metallic Bonds
- Intermolecular Forces
- Nature of Bonding and Physical Properties
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Physical States of Matter
3 topics- Gaseous State and Gas Laws
- Liquid State and Its Properties
- Solid State and Types of Solids
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Solutions
4 topics- Solution, Solute and Solvent
- Concentration Units
- Saturated, Unsaturated and Supersaturated Solutions
- Solubility and Factors Affecting It
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Electrochemistry
4 topics- Oxidation and Reduction (Redox)
- Oxidation Number and Balancing Equations
- Electrolytic and Galvanic Cells
- Corrosion and Its Prevention
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Chemical Reactivity
3 topics- Reactivity of Metals
- Reactivity of Non-Metals
- Comparison of Metals and Non-Metals
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Chemical Equilibrium
3 topics- Reversible Reactions and Dynamic Equilibrium
- Law of Mass Action and Equilibrium Constant
- Le Chatelier's Principle
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Acids, Bases and Salts
3 topics- Concepts of Acids and Bases
- pH Scale
- Salts and Their Preparation
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Organic Chemistry
4 topics- Introduction to Organic Compounds
- Sources of Organic Compounds
- Alkanes, Alkenes and Alkynes
- Functional Groups and Homologous Series
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Hydrocarbons
3 topics- Classification of Hydrocarbons
- Reactions of Alkanes
- Reactions of Alkenes and Alkynes
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Biochemistry
4 topics- Carbohydrates
- Proteins
- Lipids
- Nucleic Acids and Vitamins
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The Atmosphere
3 topics- Composition and Layers of the Atmosphere
- Air Pollutants and Their Sources
- Acid Rain, Ozone Depletion and Global Warming
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Water
3 topics- Properties of Water
- Soft and Hard Water
- Water Pollution and Treatment
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Chemical Industries
4 topics- Metallurgical Operations
- Manufacture of Sodium Carbonate (Solvay Process)
- Manufacture of Urea and Fertilizers
- Petroleum and Its Refining
Matric (SSC) Chemistry flashcards — 51 questions with answers
What is Chemistry?
The branch of science that deals with the composition, structure, properties, and reactions of matter.
Name and define the branch of chemistry that deals with the elements and compounds NOT containing carbon (minerals, metals, non-metals).
Inorganic Chemistry — the study of compounds of all elements except the hydrocarbons and their derivatives.
Which branch of chemistry studies carbon-containing compounds (hydrocarbons and their derivatives)?
Organic Chemistry.
Define Physical Chemistry.
The branch of chemistry that deals with the relationship between the composition and physical properties of matter, along with the energy changes that accompany chemical reactions.
What is Biochemistry?
The branch of chemistry that studies the structure, composition, and chemical reactions of substances found in living organisms.
Which branch of chemistry deals with the quantitative and qualitative analysis of substances (determining composition and amount)?
Analytical Chemistry.
Define Industrial (Applied) Chemistry.
The branch of chemistry concerned with the manufacture of chemical compounds on a commercial/large scale in industries.
What is Nuclear Chemistry?
The branch of chemistry that deals with the changes occurring in the nuclei of atoms, including radioactivity and nuclear reactions.
Define atomic mass (atomic mass unit, amu).
The mass of an atom of an element relative to 1/12 the mass of one carbon-12 atom; one amu = 1/12 the mass of a C-12 atom.
What is molecular mass?
The sum of the atomic masses of all the atoms present in one molecule of a substance (e.g. H2O = 18 amu).
How does formula mass differ from molecular mass?
Formula mass is the sum of atomic masses in one formula unit of an ionic compound (which has no discrete molecules), e.g. NaCl = 58.5 amu; molecular mass applies to covalent molecular substances.
Calculate the molecular mass of water (H2O). (H=1, O=16)
(2 × 1) + 16 = 18 amu.
Define the mole.
The amount of a substance that contains as many particles (atoms, molecules, ions) as there are atoms in exactly 12 g of carbon-12; i.e. 6.022 × 10^23 particles.
What is Avogadro's number and its value?
The number of particles in one mole of a substance; NA = 6.022 × 10^23 particles per mole.
What is molar mass?
The mass in grams of one mole of a substance; it is numerically equal to its atomic/molecular/formula mass expressed in grams (g/mol).
Give the formula relating number of moles to mass.
Number of moles = mass of substance (g) ÷ molar mass (g/mol).
Give the formula relating number of moles to number of particles.
Number of moles = number of particles ÷ Avogadro's number (6.022 × 10^23).
How many molecules are present in 2 moles of any substance?
2 × 6.022 × 10^23 = 1.2044 × 10^24 molecules.
Define empirical formula.
The formula that gives the simplest whole-number ratio of atoms of each element present in a compound (e.g. CH2O for glucose).
Define molecular formula.
The formula that shows the actual number of atoms of each element present in one molecule of a compound (e.g. C6H12O6 for glucose).
Show the other 31 Chemistry flashcards
State the relationship between molecular formula and empirical formula.
Molecular formula = n × (empirical formula), where n = molecular mass ÷ empirical formula mass.
The empirical formula of benzene is CH and its molecular mass is 78. What is its molecular formula? (CH = 13)
n = 78 ÷ 13 = 6, so molecular formula = C6H6.
Who discovered the electron and through which experiment?
J. J. Thomson discovered the electron through the cathode ray (discharge tube) experiment.
What is the charge and relative mass of an electron?
Charge = −1.602 × 10^−19 C (negative); mass ≈ 9.11 × 10^−31 kg (about 1/1836 of a proton).
Who discovered the proton and via what rays?
E. Goldstein discovered the proton through canal rays (positive/anode rays) in the discharge tube experiment.
What is the charge and relative mass of a proton?
Charge = +1.602 × 10^−19 C (positive); mass ≈ 1.6726 × 10^−27 kg (about 1840 times an electron).
Who discovered the neutron and what is its charge?
James Chadwick discovered the neutron; it is electrically neutral (no charge), with mass slightly greater than a proton.
What did Rutherford's gold foil (alpha-scattering) experiment conclude?
That an atom has a tiny, dense, positively charged nucleus at its centre, and most of the atom is empty space with electrons revolving around the nucleus.
State two defects of Rutherford's atomic model.
1) It could not explain the stability of the atom (a revolving electron should lose energy and spiral into the nucleus). 2) It could not explain the atomic line spectrum.
State the main postulate of Bohr's atomic model regarding electron orbits.
Electrons revolve around the nucleus only in fixed circular orbits (energy levels/shells) of definite energy without radiating energy; these are called stationary states.
According to Bohr, what happens when an electron jumps between energy levels?
Energy is absorbed when an electron jumps to a higher orbit and energy is emitted (as radiation) when it falls to a lower orbit; the energy = difference between the two levels.
What is electronic configuration?
The distribution/arrangement of electrons in the various shells (energy levels) and subshells of an atom.
What is the maximum number of electrons a shell can hold (formula)?
Maximum electrons in a shell = 2n², where n is the shell number (K=2, L=8, M=18, N=32).
Write the electronic configuration (shell-wise) of sodium (Z = 11).
2, 8, 1 (K=2, L=8, M=1).
Write the electronic configuration of chlorine (Z = 17).
2, 8, 7.
What are valence electrons?
The electrons present in the outermost (valence) shell of an atom; they determine the chemical properties and bonding behaviour of the element.
Define isotopes.
Atoms of the same element that have the same atomic number (number of protons) but different mass numbers (different numbers of neutrons).
Why do isotopes of an element have identical chemical properties?
Because they have the same number of protons and the same electronic configuration (same number of valence electrons); they differ only in number of neutrons (mass).
Name the three isotopes of hydrogen.
Protium (¹H), Deuterium (²H), and Tritium (³H).
Give one medical and one other application of isotopes.
Medical: Cobalt-60 is used in radiotherapy to treat cancer; Iodine-131 to treat thyroid disorders. Other: Carbon-14 is used for radiocarbon dating of fossils/age determination.
Who arranged elements into triads, and what is Döbereiner's law of triads?
J. W. Döbereiner; in a triad of three chemically similar elements, the atomic mass of the middle element is approximately the average of the other two.
State Newlands' Law of Octaves.
When elements are arranged in order of increasing atomic mass, every eighth element has properties similar to the first (like musical octaves).
On what basis did Mendeleev arrange his periodic table, and what was its key strength?
He arranged elements in order of increasing atomic mass; he left gaps for undiscovered elements and successfully predicted their properties (e.g. eka-silicon = germanium).
State one major defect of Mendeleev's periodic table.
The position of isotopes was not clear, and certain heavier elements were placed before lighter ones (e.g. Ar before K) to keep similar properties together — an anomaly of atomic-mass ordering.
State the Modern Periodic Law.
The properties of elements are a periodic function of their atomic numbers (Moseley); elements are arranged in order of increasing atomic number.
How many periods and groups are there in the modern (long-form) periodic table?
7 periods (horizontal rows) and 18 groups (vertical columns).
What do elements in the same group of the periodic table have in common?
They have the same number of valence electrons, so they show similar chemical properties.
Define atomic radius and state how it changes across a period and down a group.
Atomic radius is the distance from the nucleus to the outermost shell. It decreases across a period (left to right) and increases down a group.
How does ionization energy vary across a period and down a group?
Ionization energy (energy to remove the outermost electron) increases across a period and decreases down a group.
How does electronegativity change across a period and down a group, and which element is most electronegative?
Electronegativity increases across a period and decreases down a group; fluorine is the most electronegative element.
What is a chemical bond, and why do atoms react/combine?
A chemical bond is the force of attraction that holds atoms together in a molecule or compound. Atoms react to complete their outermost shell (achieve a stable noble-gas/octet or duplet configuration) and attain minimum energy/stability.
Matric (SSC) Chemistry FAQ
What is in the Matric (SSC) Chemistry syllabus?
Matric (SSC) Chemistry is split into 16 chapters: Fundamentals of Chemistry, Structure of Atoms, Periodic Table and Periodicity of Properties, Structure of Molecules, Physical States of Matter, Solutions, Electrochemistry, Chemical Reactivity, Chemical Equilibrium, Acids, Bases and Salts, Organic Chemistry and Hydrocarbons, and 4 more. Together they contain 57 topics.
How many chapters are in Matric (SSC) Chemistry?
16 chapters, containing 57 topics. The largest chapter is Structure of Molecules, with 5 topics.
Are there flashcards for Matric (SSC) Chemistry?
Yes — a 51-card 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.