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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?

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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 ₹35,600 - 75,400. Direct recruitment with age limits and qualification criteria apply.Direct RecruitmentDegree in Science with Chemistry required

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Q1. 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

Q2. 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.

Q3. 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

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. The atomic number of an element is 20. Using the Modern Periodic Law, predict the group and period of this element in the periodic table.

  1. Group 2, Period 4
  2. Group 18, Period 3
  3. Group 1, Period 4
  4. Group 16, Period 4

Q6. 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

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. 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.

Q9. 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

Q10. 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.

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. 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

Q13. 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.

Q14. 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

Q15. 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.
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