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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
⏳
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. 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.

Q2. 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.

Q3. Which factor primarily causes the atomic radius to decrease when moving from left to right across a period in the periodic table?

  1. Increase in number of electron shells.
  2. Increase in effective nuclear charge without significant increase in shielding.
  3. Decrease in nuclear charge.
  4. Increase in electron-electron repulsion in the outer shell.

Q4. Consider two elements, X and Y, where X has a smaller atomic radius but lower ionization enthalpy than Y. Which factor could explain this anomaly?

  1. Higher electron shielding in X
  2. X has a half-filled or fully filled subshell
  3. Y has a higher effective nuclear charge
  4. X has more protons than Y

Q5. 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.

Q6. Which of the following factors primarily causes the ionization enthalpy to increase across a period in the modern periodic table?

  1. Increase in atomic radius
  2. Increase in effective nuclear charge
  3. Increase in electron shielding
  4. Decrease in nuclear charge

Q7. 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.

Q8. 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+

Q9. 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

Q10. Which of the following best explains the general trend in atomic radii across a period in the modern periodic table?

  1. Atomic radius increases due to increasing number of protons.
  2. Atomic radius decreases due to increasing effective nuclear charge.
  3. Atomic radius remains constant because electron shielding is unchanged.
  4. Atomic radius increases due to addition of electron shells.

Q11. Given the ionic radii of O2- (140 pm), F- (133 pm), and Na+ (102 pm), which of the following statements is true regarding their sizes?

  1. O2- is smaller than F- due to higher nuclear charge
  2. Na+ is the smallest because it has the highest positive charge
  3. F- is larger than O2- because it has fewer electrons
  4. All ions have the same size because they are isoelectronic

Q12. 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

Q13. 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

Q14. 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

Q15. Calculate the effective nuclear charge (Zeff) experienced by the outermost electrons of Mg2+ ion, given that Mg has atomic number 12 and the shielding constant (S) for the 10 electrons is approximately 10. Use Zeff = Z - S.

  1. 2
  2. 10
  3. 12
  4. 22
Free Technical Assistant( Kerala Drugs Control ) Mock Test | Kerala PSC Prep