Question

Which one of the following does not have intermolecular H-bonding?

• A. $C{H}_4$
• B. $H_{2}Se$
• C. $N_2{H}_4$
• D. $H_{2}S$

Answer 1

Answer: (A), (B), (D)

$C{H}_4$
$H_{2}Se$
$H_{2}S$

Condition for H-Bonding

• Highly Electronegative atom bonded to Hydrogen molecules
  must contain High EN atom such as N, O, or F covalently bonded to Hydrogen.
  ex: $HF,H_{2}O,{NH}_3$
• The small size of EN atom
  Smaller the size of the atom, greater will be an attraction for the bonded electron pair. In other words, a polarity of a bond between H atom and the electronegative atom should be high.
  Out of all the molecules, only $N_2{H}_4$ fits into the condition.