ā† Back to Technical Assistant( Kerala Drugs Control )

Free Technical Assistant( Kerala Drugs Control ) Practice

Question 1 of 15

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

You're trying 15 free practice questions. Sign up to unlock the full question bank with detailed rationales and progress tracking.

Free Technical Assistant( Kerala Drugs Control ) Practice Questions

Kerala Public Service CommissionRecruitment for the post of Technical Assistant in Kerala Drugs Control Department. The role involves scientific duties with a pay scale of ā‚¹35,600 - 75,400. Direct recruitment with age limits and qualification criteria apply.Direct RecruitmentDegree in Science with Chemistry required

Try 15 free syllabus-aligned practice questions for the Technical Assistant( Kerala Drugs Control ) exam. Each question includes instant feedback so you can learn as you go. No sign-up required.

šŸ“‹ Preview All 15 Practice 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. 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

Q3. 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.

Q4. 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

Q5. 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

Q6. 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.

Q7. 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

Q8. 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

Q9. 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+

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. 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 āˆ nĀ² / 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)

Q12. 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

Q13. 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.

Q14. 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

Q15. 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
Free Technical Assistant( Kerala Drugs Control ) Practice Questions | Kerala PSC Prep