Factors Affected by Hydrogen Bonding
HF, HCl, HBr, HI
The correct order of thermal stability of hydrogen halides (H – X) is
HF >HCl>HBr> HI
HCl> HF >HBr> HI
HI >HCl> HF >HBr
HI >HBr>HCl> HF
The correct order of acidic strength of HOCl, HClO2, HClO3 and HClO4 are:
While separating a mixture of ortho and para nitrophenols by steam distillation, name the isomer which will be steam volatile. Give reason.
Why ice is lighter than water?
If the boiling point of H2O is 373 K, the boiling point of H2S will be
Greater than 300 K but less than 373 K
Equal to 373 K
More than 373 K
Less than 300 K
Why does an acidic strength increase down the group?
- Phthalic acid
- Malonic acid
- Succinic acid
- Salicylic acid
Hydrogen bonds are formed in many compounds e.g., H2O, HF, NH3. The boiling point of such compounds depends to a extent on the strength of hydrogen bond and the number of hydrogen bonds. The correct decreasing order of the boiling points above compounds is
- Hydrogen < van der Waals force < Covalent bonding
- van der Waals force < Hydrogen bonding < Covalent
- Covalent <van der Waals force< Hydrogen bonding
- van der Waals force<Covalent <Hydrogen bonding
- Steric hindrance
- Intra-molecular H-bonding
Use the information and date given below to answer the question (a) to (c),
Stronger intermolecular forces result in higher boiling point.
Strength of London forces increases with the number of electrons in the molecule.
Boiling point of HF, HCl, HBr and Hi are 293 k, 189 k, 206 k and 238 k respectively.
(a) Which type of intermolecular forces are present in the molecules HF, HCl, HBr an HI?
(b) Looking at the trend of boiling points of HCl, HBr and HI, explain out of dipole-dipole interaction and London interaction, which one is predominant here.
(c) Why is boiling point of hydrogen fluoride highest while that of hydrogen chloride lowest?
Sugar is soluble in water due to:
High solvation energy
Hydrogen bond formation with water
High dipole moment of water
Ionic charachter of sugar
Are alcohols capable of hydrogen bonding?
The boiling point of methanol, water and dimethyl ether are respectively 650 C, 1000 C and 34.50 C. Which of the following best explains these wide variations in b.p.?
The extent of H-bonding decreases from water to methanol while it is absent in ether
The extent of intramolecular H-bonding decreases from ether to methanol to water
The molecular mass increases from water (18) to methanol (32) to diethyl ether (74)
The density of water is 1.00 g ml-1, methanol 0.7914 g ml-1 and that of diethyl ether is 0.7137 g ml-1
Alcohols are comapratively more soluble in water than hydrocarbons of comparable molecular masses. Explain this fact.
In solid argon, the atoms are held together by
Van der Waals forces
- intermolecular H-
- intramolecular H-
Bond angle in is higher than that in PH3. Why?