Very Short Question
1. Write the molecular formula for:
a. Blue Vitriol
b. Gypsum Salt
c. Calomel
d. Bleaching power
2. What is chemical equation? Mention its significance and Mention it’s limitations?
3. Define electronegativity and ionization potential.
4. State Mendeleev’s periodic law. Write any two limitations ofMendeleev’s periodic table.
5. State Modern periodic law. Write any two Advantages.
6. Write the electronic configuration of:
a. Atomic number 11
b. Atomic number 29
c. Atomic number 24
7. Explain in brief about ionic and covalent bond.
8. What do you mean by Hund’s rule? Explain.
9. Define the term +I effect and – I effect.
4. Find the oxidation number of underlined atoms.
a. KMnO4
b. K2CrO4 ( Search and practice yourself )
10. Calculate pH of 0.5 molar solution of HCI.
11. What do you mean by saturated and supersaturated solution?
12. Define normality and molarity of a solution.
13. What do you mean by antipyretics and antibiotic?
14. Define reversible and irreversible reaction.
15. What happens when nickel metal is heated with carbon monoxide?
16. What happens when ethyne gas is passed through red hotcopper tube?
17. Write the medical use of milk of magnesia and plaster of paris.
18. What is protein? List two functions of protein.
19. Write the biological important of sodium, magnesium, Calcium and potassium?
20. What is heavy water? Give its two uses.
Short / Long Questions
1. Define ideal gas. State Dalton’s law of partial pressure. Derive pV=nRT.
2. How do you identify primary, secondary and tertiaryalcohol by oxidation method?
3. Define Strong and weak electrolytes with examples. State and explain Faraday’s 1st and 2nd law ofelectrolysis.
4. What do you mean by Markovnikov’s and Anti-Markovnikov’s rule? Explain with examples.
5. What is atomic Bohr’s Model? What are the postulates of Bohr’s atomic model?
6. Define acidimetry and alkalimetry. 10 mL of Na₂CO₃ solution is titrated with N/10 HCl. Calculate its strength in terms of normality and g/L if 4.1 mL of HCl was used. (Numerical is similar )
7. What do you mean by osmosis? Mention its biologicalimportance.
8. Calculate the resulting normality of a solution formed by mixing 20 mL 0.8N NaOH and 30 mL 0.4M H₂SO₄. (Numerical is similar)
9. Explain Hess’ law of constant heat summation.
10. Define functional group with some examples.
11. What is isomerism? Describe different types ofstructural isomerism with example.
12. Explain the laboratory preparation of ammonia, withneat diagram. Write its physical and chemicalproperties.
13. Describe Raoults law in brief. Also, list the colligative properties.
14. How can you prepare chloroform in the laboratory?What are its physical and chemical properties?
15. How can you prepare nitrobenzene in a laboratory? Explain itsproperties.
16. 50 gm of CaCO3 reacts with 40 gm of HCI to produce CaCl2, CO2 and H2O. Find out
a. Limiting reagent.
b. Amount of unreacted substance left over.
c. Volume of CO2 formed at NTP.
d. Mass of NaOH solution required to absorb CO2 formed. ( Numerical is similar )
17. Explain the process of fermentation.
18. Define Reimer-Tiemann reaction, Canizzaro’s reaction, Friedel Craft’s reaction,Diazotisation, coupling reaction and Tollen’s reaction.
19. Explain the function of carbohydrates and lipid in detail.
20. Describe the laboratory preparation of ethoxyethane withwell labelled diagram.
21 Write short notes on: (any two)
a. Ozone Layer Depletion
b. Air Pollution and its Effects
c. Laboratory Preparation of Carbon Monoxide
d. Global warming
e Functions of protein
f. Properties of H2S
22. What is hardness of water, and what are its causes? Explain how permutit process removes both temporary and permanent hardness.
23. What is the difference between temporary and permanent hardness of water? How can temporary hardness be removed by boiling, and permanent hardness be removed by permutit process or washing soda process?
CTEVT Chemistry Fixed Questions 2082
