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Identify the wrong statement in the following:

  1. A
    Atomic radius of the elements decreases as one moves across from left to right in the 2nd period of the periodic table
  2. B
    Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the ionic radius
  3. C
    Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius
  4. D
    Atomic radius of the elements increases as one moves down the first group of the periodic table.

Solution & Step-by-step Explanation

1. Correct: Effective nuclear charge increases across a period, pulling electrons closer.2. Incorrect: For isoelectronic species (same number of electrons), as the positive charge increases, the nucleus attracts the electrons more strongly, so the ionic radius decreases. Therefore, a smaller positive charge corresponds to a larger radius.3. Correct: Higher negative charge means more electron-electron repulsion and lower effective nuclear charge per electron, increasing size.4. Correct: New shells are added down a group.

Practice this question

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Identify the wrong statement in the following:
A
Atomic radius of the elements decreases as one moves across from left to right in the 2nd period of the periodic table
B
Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the ionic radius
C
Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius
D
Atomic radius of the elements increases as one moves down the first group of the periodic table.

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Inorganic ChemistryPeriodic PropertiesAtomic Radius

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