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Free Technical Assistant( Kerala Drugs Control ) Mock Test

Test your knowledge under timed conditions. Get scored results instantly — no sign-up required.

❓
Questions
15
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Time Limit
15 min
📝
Format
Multiple Choice

Instructions

  • Answer all 15 questions within 15 minutes.
  • You can skip questions and come back to them later.
  • The timer starts when you click “Start Mock Test”.
  • Your score will be shown immediately after submission.
  • Sign up free to see detailed rationales for every answer.

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About This Mock Test

The Free Mock Test for Technical Assistant (Kerala Drugs Control) (615/2025) is designed to help candidates prepare effectively for the upcoming examination. This mock test focuses on assessing your knowledge and understanding of key concepts relevant to the Technical Assistant role within Kerala Drugs Control. It offers a realistic simulation of the actual exam environment, enabling you to evaluate your readiness and identify areas for improvement.

Exam Pattern

  • Duration: 15 minutes
  • Number of Questions: 15
  • Difficulty Level: Medium
  • Pass Percentage: 75%

Topics Covered

  • Basic Concepts of Chemistry

Why Take This Mock Test?

  • Gain familiarity with the exam format and time constraints specific to the Technical Assistant (Kerala Drugs Control) exam.
  • Identify your strengths and weaknesses in the Basic Concepts of Chemistry to focus your study efforts efficiently.
  • Build confidence by practicing under realistic conditions, helping to reduce exam-day anxiety.
  • Track your progress and improve your chances of achieving the required 75% pass percentage.

Take the free Technical Assistant (Kerala Drugs Control) mock test now to boost your preparation and move one step closer to success!

📋 Preview All 15 Mock Test Questions

Q1. Consider the ions Na+, Mg2+, and Al3+. Which of the following correctly ranks their ionic radii from largest to smallest?

  1. Na+ > Mg2+ > Al3+
  2. Al3+ > Mg2+ > Na+
  3. Mg2+ > Na+ > Al3+
  4. Na+ > Al3+ > Mg2+

Q2. Arrange the following factors in order of their influence on ionization enthalpy from most to least significant:1. Effective nuclear charge2. Atomic radius3. Electron shielding4. Subshell configuration stability

  1. 1 > 2 > 3 > 4
  2. 2 > 1 > 4 > 3
  3. 3 > 1 > 2 > 4
  4. 4 > 3 > 2 > 1

Q3. Which of the following best explains why elements in the same group of the Modern Periodic Table exhibit similar chemical properties?

  1. They have the same number of electron shells.
  2. They have the same number of valence electrons.
  3. They have similar atomic masses.
  4. They have identical atomic numbers.

Q4. Consider two elements X and Y where X has atomic number 15 and Y has atomic number 16. According to the Modern Periodic Law, which of the following is true about their chemical properties?

  1. They have completely different chemical properties because their atomic masses differ.
  2. They have similar chemical properties because they are in the same group.
  3. They have different chemical properties because they belong to different groups.
  4. Their chemical properties depend only on their physical states.

Q5. Which of the following statements best defines the Modern Periodic Law?

  1. Properties of elements are a periodic function of their atomic masses.
  2. Properties of elements are a periodic function of their atomic numbers.
  3. Elements are arranged in order of increasing density.
  4. Elements are grouped based on their physical states at room temperature.

Q6. Consider two elements, X and Y, in the same group of the periodic table where Y is below X. Which statement correctly compares their atomic radii?

  1. Element X has a larger atomic radius than element Y.
  2. Element Y has a larger atomic radius than element X.
  3. Both elements have the same atomic radius.
  4. Atomic radius depends only on the number of protons, so cannot be compared.

Q7. What is the correct definition of ionization enthalpy?

  1. Energy released when an electron is added to a neutral atom
  2. Energy required to remove one mole of electrons from one mole of gaseous atoms
  3. Energy required to break one mole of bonds in a molecule
  4. Energy released when one mole of gaseous atoms gains an electron

Q8. Calculate the approximate atomic radius of an element if the effective nuclear charge (Z_eff) experienced by its outermost electron is 5 and the principal quantum number (n) is 3, using the simplified formula: Atomic radius ∝ n² / Z_eff. Which of the following values is closest?

  1. 1.8 (arbitrary units)
  2. 2.4 (arbitrary units)
  3. 3.6 (arbitrary units)
  4. 5.0 (arbitrary units)

Q9. Calculate the approximate ionization enthalpy trend given the following data for elements A, B, and C in the same period: Atomic number of A = 11, B = 12, C = 13. Assume effective nuclear charge increases by 0.5 units per atomic number increment and ionization enthalpy is proportional to effective nuclear charge. If ionization enthalpy of A is 500 kJ/mol, estimate the ionization enthalpy of C.

  1. 750 kJ/mol
  2. 1000 kJ/mol
  3. 1250 kJ/mol
  4. 1500 kJ/mol

Q10. In a hypothetical scenario, if the shielding effect in a period increased significantly while the nuclear charge remained constant, what would be the expected trend in atomic radii across that period?

  1. Atomic radius would increase across the period.
  2. Atomic radius would decrease across the period.
  3. Atomic radius would remain constant across the period.
  4. Atomic radius would first increase then decrease across the period.

Q11. Calculate the energy required to remove 2 moles of electrons from 2 moles of gaseous sodium atoms if the first ionization enthalpy of sodium is 496 kJ/mol.

  1. 496 kJ
  2. 992 kJ
  3. 248 kJ
  4. 1984 kJ

Q12. Explain why the ionic radius of an anion is generally larger than that of its parent atom.

  1. Addition of electrons increases electron-electron repulsion, expanding the electron cloud
  2. The nuclear charge increases, pulling electrons closer
  3. The number of protons decreases, reducing attraction
  4. The atom loses electrons, causing the radius to increase

Q13. Consider the elements magnesium (Mg) and aluminum (Al). Which one has a higher first ionization enthalpy and why?

  1. Mg has higher ionization enthalpy due to completely filled s-orbital
  2. Al has higher ionization enthalpy because it has more protons
  3. Both have the same ionization enthalpy as they are in the same period
  4. Al has lower ionization enthalpy due to electron entering a p-orbital

Q14. Which of the following best explains the trend in ionic radii of isoelectronic ions as the atomic number increases?

  1. Ionic radius increases due to more electron-electron repulsion
  2. Ionic radius decreases due to increasing nuclear charge pulling electrons closer
  3. Ionic radius remains constant because the number of electrons is the same
  4. Ionic radius fluctuates randomly with atomic number

Q15. Which factor primarily causes the decrease in ionization enthalpy down a group in the periodic table?

  1. Increase in nuclear charge
  2. Increase in atomic radius and shielding effect
  3. Decrease in number of electrons
  4. Increase in effective nuclear charge
Free Technical Assistant( Kerala Drugs Control ) Mock Test | Kerala PSC Prep