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Punjab (PTB) · Full book test (board pattern) · Free

1st Year Chemistry Full Book Paper

85 marks · 3 hours · 55 questions. Covers: 16 chapters (CHAP 1: Periodic Table and Periodic Properties to CHAP 16: Lab Safety and Practical Skills).

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1st Year Chemistry Full Book Paper

1st Year · Chemistry · Punjab (PTB)

Name: ____________Roll No: ________Class/Section: ________Date: ________Total marks: 85Time: 3 hours

Q1. Multiple choice questions (Attempt all · 17 × 1 = 17)

  1. The mobile source of air pollution is:

    1. Cement factory

    2. Power plant

    3. Airplane

    4. Oil refinery

  2. Ion gives a yellow precipitate with ammonium molybdate and nitric acid:

    1. Sulfate

    2. Carbonate

    3. Phosphate

    4. Chloride

  3. Element is typically used to dope silicon to create a p-type semiconductor:

    1. Group 1 element

    2. Group 14 element

    3. Group 13 element

    4. Group 15 element

  4. Which type of equilibrium involves a change of state?

    1. Chemical

    2. Physical

    3. Ionic

    4. Molecular

  5. n-Butanol and diethyl ether are:

    1. Geometrical isomers

    2. Position isomers

    3. Chain isomers

    4. Functional group isomers

  6. London dispersion forces increase with:

    1. Decreasing molar mass

    2. Increasing polarity

    3. Increasing molecular size

    4. Decreasing temperature

  7. Which one of the following elements has the highest ionization energy?

    1. Sodium (Na)

    2. Magnesium (Mg)

    3. Aluminium (Al)

    4. Argon (Ar)

  8. For effective separation using simple distillation, the minimum required difference in boiling points between the components should be approximately:

    1. 5°C

    2. 10°C

    3. 15°C

    4. 25°C or more

  9. True about theoretical yield is:

    1. It is always less than actual yield

    2. It is always equal to actual yield

    3. It is always greater than actual yield

    4. It may be equal or less than actual yield

  10. The pH of 10-3mol dm-3 of an aqueous solution of H2SO4 is:

    1. 3.0

    2. 2.7

    3. 2.0

    4. 1.5

  11. For the half-reaction if the concentration of , if the concentration of M n + ions is decreased below 1 M at 298 K, how will the actual electrode potential (E) change? 

    1. E will become more positive

    2. E will remain unchanged

    3. E will become less positive (or more negative)

    4. E will always become 0 V

  12. The order of reaction is:

    1. The total number of molecules taking part in the rate determining step

    2. The total number of molecules taking part in a chemical reaction

    3. Both a and b

    4. None of these

  13. If absolute temperature of a gas is double and the pressure is reduced to one half, the volume of the gas will:

    1. Remain unchanged

    2. Increase four times

    3. Reduce to

    4.  Be doubled

  14. Nitrosomonas helps in conversion of:

    1. NO4- to NO2-

    2. NO4+ to NO2-

    3. NO4- to N2

    4. N2 to NO3-

  15. AgNO3 forms a precipitate with a halide ion due to formation of:

    1. Ionic bonds

    2. Complex compounds

    3. Silver halide salts

    4. Covalent halide radicals

  16. An energy profile shows a very flat region after the first peak before rising to a second, higher peak; what does this suggest about the intermediate?

    1. It is highly reactive.

    2. It is consumed quickly.

    3. It is relatively stable.

    4. It has a high activation energy for the next step.

  17. Which atmospheric layer would a commercial airplane typically fly in to avoid weather turbulence?

    1. Troposphere

    2. Stratosphere

    3. Mesosphere

    4. Thermospher

Q2. Short questions (Attempt any 8 of 12 · 8 × 2 = 16)

  1. Why do ionic compounds not possess molecular formulas?

  2. How do you differentiate between crystalline solids and amorphous solids?

  3. Sketch the hybrid orbital and bond formation in PCI3, SiCI4, and NH4+.

  4. What is the n +  rule or Wiswesser rule? Give example.

  5. Why the elements of group VI-A have less ionization energy values than V-A?

  6. Explain why bond breaking is always an endothermic process, while bond formation is always exothermic, in the context of r.

  7. Calculate the mass in grams of 2.74 moles of KMnO4.

  8. Why does wind increase the rate of evaporation of a liquid?

  9. Draw the Lewis (electron dot) structures for the following species: (i) HCN (ii) 3

  10. How many orbitals are possible for n = 4? Show how you calculate it.

  11. Define metals and give example?

  12. If a reaction involves a phase change in one of the reactants or products, how must bond energy calculations be adjusted to provide a more accurate ?

Q3. Short questions (Attempt any 8 of 12 · 8 × 2 = 16)

  1. Write down name of the following compounds according to IUPAC-System. (i) CH2=CH-CH=CH2 (ii)CH2=C-CH2CH2CH3 (image) (iii) (CH2CH2)3CH

  2. Give an example of a sulfur-containing fragrance compound and its application.

  3. Why electrode potential of Cu is called reduction potential?

  4. Why is the water molecule considered amphoteric according to the Bronsted-Lowry theory? Provide equations to illustrate its behavior as both an acid and a base.

  5. Why does changing the concentration of a substance not alter the value of the equilibrium constant?

  6. What is meant by order of reaction?

  7. Differentiate between open and closed chain hydrocarbons.

  8. How does V2O5 catalyze the formation of SO3?

  9. State the value of Avogadro's constant and Faraday's constant.

  10. Explain the concept of a conjugate acid-base pair using a specific example.

  11. The change of volume disturbs the equilibrium position for some of the gas phase reactions but not the equilibrium constant.

  12. A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration is doubled and reduced to half?

Q4. Short questions (Attempt any 6 of 9 · 6 × 2 = 12)

  1. Describe the appearance of copper(II) hydroxide.

  2. Why does iodine sublimate on heating instead of melting?

  3. What are hydrocarbons and how do they enter the atmosphere?

  4. List three practical applications of paper chromatography.

  5. What are the consequences of ignoring safety instructions in a lab?

  6. The ionic equation for a reaction is:.Explain which species is oxidized in this reaction. Why?

  7. Why is carbon monoxide dangerous? And How is carbon dioxide a threat to the environment?

  8. Differentiate between filtrate and residue with examples.

  9. Why must the burette be rinsed with the titrant before use?

Q5. Long questions (Attempt any 3 of 5 · 3 × 8 = 24)

  1. Describe the free radical halogenation of methane using Cl2 as an example.

  2. What is the standard enthaply change? Give different types of enthaply changes with their examples.

  3. Write down the Kc for the following reactions. Suppose that the reaction mixture in all the case is ‘V’ dm-3 (i) CH3COOH + CH3CH2OH (eq) CH3COOC2H5 + H2O (ii) 2HI (eq) H2 + I2 (iii) N2 + 3H2 2NH3

  4. Explain the process of chlorination in water purification. Also explain the role of active species formed during chlorination and factors affecting chlorination. How it is regulated?

  5. Describe the criterion to choose the suitable solvent in the process of crystallization.