An element 'E' has the ionisation enthalpy value of 374 kJ mol $^{-1}$ . 'E' reacts with elements A, B, C and D with electron gain enthalpy values of $-328$ , $-349$ , $-325$ and $-295$ kJ mol $^{-1}$ , respectively.

The correct order of the products EA, EB, EC and ED in terms of ionic character is:

Question

An element 'E' has the ionisation enthalpy value of 374 kJ mol $^{-1}$ . 'E' reacts with elements A, B, C and D with electron gain enthalpy values of $-328$ , $-349$ , $-325$ and $-295$ kJ mol $^{-1}$ , respectively.

The correct order of the products EA, EB, EC and ED in terms of ionic character is:

Paaras Thakur · Accepted Answer

EB EA EC ED. 🧠 More exothermic EGE → more stable anion → more ionic compound Ionic character of a compound between E and a non-metal depends on how strongly the non-metal attracts the electron. A more negative EGE means the anion is more stable, and the bond is more ionic. 🗺️ Rank by EGE magnitude Element E has IE = 374 kJ/mol (very low — a highly electropositive metal, likely Cs or Rb). - B: -349 kJ/mol — most exothermic. Most stable anion. Most ionic compound (EB). - A: -328 kJ/mol. - C: -325 kJ/mol. - D: -295 kJ/mol — least exothermic. Least ionic. Order of ionic character: EB EA EC ED. {{Answer: (a)}}

Answer

EB EA EC ED

Answer

ED EC EA EB

Answer

EA EB EC ED

Answer

ED EC EB EA

An element 'E' has the ionisation enthalpy value of 374 kJ mol-1. 'E' reacts with elements A, B, C and D with electron…

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