AP EAMCET / TS EAMCET Chemistry - Inorganic and Organic Chemistry Syllabus

Chemistry - Inorganic and Organic Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry - Inorganic and Organic Chemistry in AP EAMCET / TS EAMCET, not a summary of it.

1. 1

   Chemical Bonding and Hydrogen

   3 topics

   • Chemical Bonding and Molecular Structure
     • Ionic and covalent bonds
     • VSEPR theory and hybridisation
     • Molecular orbital theory
   • Hydrogen and its Compounds
     • Position, isotopes and preparation
     • Water, hydrogen peroxide and hydrides
   • Environmental Chemistry
     • Air, water and soil pollution
     • Green chemistry
2. 2

   s-Block and p-Block Elements

   3 topics

   • s-Block Elements
     • Alkali metals and their compounds
     • Alkaline earth metals and their compounds
   • p-Block Elements (Groups 13-14)
     • Boron and aluminium family
     • Carbon family and allotropes
   • p-Block Elements (Groups 15-18)
     • Nitrogen and oxygen families
     • Halogens and noble gases
3. 3

   d, f Block and Coordination Compounds

   3 topics

   • d and f Block Elements
     • Transition elements and their properties
     • Lanthanides and actinides
   • Coordination Compounds
     • Nomenclature and isomerism
     • Werner's theory and valence bond theory
     • Crystal field theory
   • Metallurgy
     • Principles and methods of extraction
     • Thermodynamic and electrochemical principles
4. 4

   Organic Chemistry - Fundamentals and Hydrocarbons

   3 topics

   • General Organic Chemistry
     • Nomenclature and isomerism
     • Electronic effects and reaction intermediates
     • Types of organic reactions and mechanisms
   • Hydrocarbons
     • Alkanes, alkenes and alkynes
     • Aromatic hydrocarbons and benzene
   • Haloalkanes and Haloarenes
     • Nucleophilic substitution reactions
     • Elimination reactions
5. 5

   Organic Chemistry - Functional Groups and Biomolecules

   4 topics

   • Alcohols, Phenols and Ethers
     • Preparation and reactions of alcohols
     • Acidity of phenols and ethers
   • Aldehydes, Ketones and Carboxylic Acids
     • Nucleophilic addition to carbonyl group
     • Acidity and derivatives of carboxylic acids
   • Organic Compounds Containing Nitrogen
     • Amines and basicity
     • Diazonium salts and cyanides
   • Biomolecules, Polymers and Everyday Chemistry
     • Carbohydrates, proteins and nucleic acids
     • Polymers and polymerisation
     • Drugs, detergents and food chemistry

Chemistry - Inorganic and Organic Chemistry flashcards for AP EAMCET / TS EAMCET

19 of 51 cards from the Chemistry - Inorganic and Organic Chemistry deck — real questions with worked answers.

1. What is the VSEPR theory used to predict in covalent molecules?

   The shape/geometry of a molecule, based on the idea that electron pairs (bonding and lone pairs) around a central atom arrange themselves to minimize repulsion. Repulsion order: lone pair-lone pair > lone pair-bond pair > bond pair-bond pair.

2. According to hybridisation, what are the shapes corresponding to sp, sp2, sp3, sp3d, and sp3d2?

   sp = linear (180 deg); sp2 = trigonal planar (120 deg); sp3 = tetrahedral (109.5 deg); sp3d = trigonal bipyramidal; sp3d2 = octahedral (90 deg).

3. State the formal definition of bond order in molecular orbital theory.

   Bond order = 1/2 (number of electrons in bonding MOs - number of electrons in antibonding MOs). Higher bond order means greater stability and shorter bond length.

4. Why is the dipole moment of water (1.84 D) and not zero, while CO2 is zero?

   Water is bent (angular) due to two lone pairs on oxygen, so bond dipoles do not cancel. CO2 is linear and symmetric, so its two equal bond dipoles cancel, giving zero net dipole moment.

5. What is hydrogen bonding and name its two types?

   An electrostatic attraction between an H atom bonded to a highly electronegative atom (F, O, N) and a lone pair on another electronegative atom. Types: intermolecular (between molecules, e.g. water) and intramolecular (within a molecule, e.g. o-nitrophenol).

6. What is Fajan's rule about covalent character in ionic bonds?

   Covalent character increases with: small cation size, large anion size, high charge on cation or anion, and cation with a pseudo-inert gas (18-electron) configuration. Greater polarisation = more covalent character.

7. What are the three isotopes of hydrogen and their mass numbers?

   Protium (1H, mass 1, no neutron), Deuterium (2H or D, mass 2, 1 neutron), Tritium (3H or T, mass 3, 2 neutrons, radioactive).

8. What is the difference between temporary and permanent hardness of water?

   Temporary hardness is due to bicarbonates of Ca and Mg, removed by boiling or Clark's method (adding lime). Permanent hardness is due to chlorides and sulphates of Ca and Mg, removed by washing soda, ion-exchange or Calgon process.

9. What is the structure and key property of hydrogen peroxide (H2O2)?

   H2O2 has a non-planar open book structure. It acts as both an oxidising and reducing agent. It is decomposed (disproportionates) into water and oxygen; stored in dark/wax-lined bottles to prevent decomposition.

10. What are the main greenhouse gases responsible for global warming?

    Carbon dioxide (CO2), methane (CH4), water vapour, nitrous oxide (N2O), CFCs, and ozone. They trap infrared radiation re-emitted by the earth's surface.

11. What causes acid rain and what is its typical pH?

    Acid rain is caused by oxides of sulphur (SO2) and nitrogen (NOx) forming H2SO4 and HNO3 in the atmosphere. Acid rain has a pH below 5.6.

12. What is BOD (Biochemical Oxygen Demand) and what does a high value indicate?

    BOD is the amount of oxygen required by bacteria to decompose organic matter in a given volume of water. A high BOD value indicates high organic pollution (more contaminated water). Clean water has BOD below 5 ppm.

13. Why are alkali metals (s-block Group 1) the most reactive metals and strong reducing agents?

    They have a single, loosely held valence electron with low ionisation energy, so they readily lose it to form +1 ions. Reactivity increases down the group as ionisation energy decreases.

14. What is the diagonal relationship and give the two classic examples in the s-block?

    Certain elements of period 2 resemble the period 3 element diagonally below-right due to similar charge/size ratio. Examples: Li resembles Mg, and Be resembles Al.

15. Why do alkali metals impart characteristic colours to a flame?

    The flame energy excites valence electrons to higher energy levels; on returning, they emit visible light. Li = crimson red, Na = golden yellow, K = lilac/violet, Rb = red-violet, Cs = blue.

16. What is the chemical name, formula, and one main use of washing soda?

    Washing soda is sodium carbonate decahydrate, Na2CO3.10H2O. Used in softening of hard water, in glass/paper/detergent manufacture, and as a cleaning agent.

17. Why is BeO amphoteric while the oxides of other alkaline earth metals are basic?

    Be has a small size and high polarising power giving BeO appreciable covalent character, so it reacts with both acids and bases (amphoteric). Other Group 2 oxides (MgO, CaO etc.) are ionic and basic.

18. Why does boron show anomalous behaviour and resemble silicon (Group 13 anomaly)?

    Boron has small size, high ionisation energy, no d-orbitals, and high electronegativity, making it a non-metal (forms only covalent compounds). This gives it a diagonal relationship with silicon.

19. What is the inert pair effect and how does it affect Group 13/14 oxidation states?

    The reluctance of the ns2 electrons to participate in bonding down the group. As a result, the lower oxidation state becomes more stable down the group: e.g. in Group 13, +1 (Tl+) becomes more stable than +3; in Group 14, +2 (Pb2+) more stable than +4.

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