Test: Hydrogen Bonding (NCERT)

HF

H₂O

NH

CH₃OH

Displacement of electrons towards more electronegative atom resulting in fractional positive chargeon hydrogen

Displacement of electrons towards hydrogenatom resulting in a polar molecule

Formation of a bond between hydrogen atoms of one molecule and the other

Existence of an attractive force which binds hydrogen atoms together.

Cl and N have comparable electronegativities yet there is no H-bonding in HCl because size of Cl is large

Intermolecular H-bonding results in decrease in m.p. and b.p

Ice has maximum density at 0⁰C due toH-bonding

KHCI₂₍HCI^-₂) exists but KHF₂(HF^-₂) does not exist due to lack of H-bonding in HCl

HF

HCl

HBr

HI

(i), (ii) and (iii)

(i) and (iii)

(ii) and (iii)

(i) and (ii)

Paired electrons

Unpaired electrons

Lone pair of electrons

Bond order more than one.

Methanol is transparent like water

Due to hydrogen bonding between methanol and water molecules

Due to van der Waals' forces between methanoland water

Due to covalent attraction forces

Solids have lesser density than liquids

It has open-cage like structure in which lesser molecules are packed per mL than water

Ice is lighter than water

When ice is formed water molecules come closer and start floating.

o-Nitrophenol

p-Nitrophenol

Benzoic acid

Ethanol

Intermolecular hydrogen bonds are formed between two different molecules of compounds

Intramolecular hydrogen bonds are formed between two different molecules of the same compound

Intramolecular hydrogen bonds are formed within the same molecule

Hydrogen bonds have strong influence on the physical properties of a compound