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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 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

Q2. 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

Q3. Which of the following trends correctly describes the variation of first ionization enthalpy across a period in the modern periodic table?

  1. It decreases from left to right across a period
  2. It remains constant across a period
  3. It generally increases from left to right across a period
  4. It fluctuates randomly with no trend

Q4. 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

Q5. 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

Q6. 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.

Q7. 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

Q8. 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

Q9. How did the discovery of atomic number influence the arrangement of elements in the Modern Periodic Table?

  1. It allowed elements to be arranged by increasing atomic mass.
  2. It resolved anomalies in Mendeleev's periodic table by arranging elements by nuclear charge.
  3. It grouped elements based on their melting points.
  4. It led to the classification of elements by their isotopic masses.

Q10. 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

Q11. Which of the following best explains why ionization enthalpy decreases down a group despite increasing nuclear charge?

  1. Increase in atomic radius and electron shielding
  2. Decrease in number of electron shells
  3. Increase in effective nuclear charge
  4. Decrease in nuclear charge

Q12. 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

Q13. 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

Q14. 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.

Q15. 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
Free Technical Assistant( Kerala Drugs Control ) Mock Test | Kerala PSC Prep