Factors Affected by Hydrogen Bonding

Q. Among $H_{2}O,H_{2}S,H_{2}Se$ and $H_{2}Te$, the one with the highest boiling point is:

1. $H_{2}O$ because of $H-$ bonding
2. $H_{2}Te$ because of higher molecular weight
3. $H_{2}S$ because of H - bonding
4. $H_{2}Se$ because of lower molecular weight

Q. $N{H}_3$ is more liquefiable when compared to HCl. Why?

1. Lower molecular mass

2. H - bonding

3. Presence of H

4. Presence of Cl

Q. The carboxylic acid which has maximum solubility in water is:

1. Phthalic acid
2. Succinic acid
3. Malonic acid
4. Salicylic acid

Q.

Highest viscosity is exhibited by :

1. Glycerol

2. Ethylene glycol

3. Ethanol

4. Water

Q. H2SO4 has higher viscosity than water. Reason being bonding.

1. intermolecular H-
2. intramolecular H-
3. covalent

Q. $o$-nitrophenol is more volatile than $p$-nitrophenol because of:

1. Steric hindrance
2. Hyperconjugation
3. Intra-molecular H-bonding
4. Resonance

Q. $o$-nitrophenol is more volatile than $p$-nitrophenol because of:

1. Steric hindrance
2. Hyperconjugation
3. Intra-molecular H-bonding
4. Resonance

Q. Arrange the following types of interactions in order of their increasing stability.

1. van der Waals force<Covalent <Hydrogen bonding
2. Covalent <van der Waals force< Hydrogen bonding
3. Hydrogen < van der Waals force < Covalent bonding
4. van der Waals force < Hydrogen bonding < Covalent

Q. An ether is more volatile than an alcohol having the same molecular formula. This is due to:

1. Dipolar character of ethers
2. Alcohols having resonance structures
3. Inter- molecular hydrogen bonding in ethers
4. Inter- molecular hydrogen bonding in alcohols

Q. Identify the correct order of boiling points of the following compounds?
I) $C{H}_{3}C{H}_{2}C{H}_{2}C{H}_{2}OH$
II) $C{H}_{3}C{H}_{2}C{H}_{2}CHO$
III) $C{H}_{3}C{H}_{2}C{H}_{2}COOH$

1. $I>II>III$
2. $II>III>I$
3. $I>III>II$
4. $III>I>II$

Q. Which of the following is the correct decreasing order of boiling points?

1. $HF>HI>HBr>HCl$
2. $HF>HBr>HI>HCl$
3. $HCl>HBr>HI>HF$
4. $HCl>HI>HBr>HF$

Q. Which of the following statements are correct regarding band theory of metallic bond ?

1. Overlapping of conduction & valence band occurs in semiconductors
2. Valence band is empty or half filled in metal
3. Energy gap between conduction and valence band is very less in non-conductors
4. Conduction band is empty in metal

Q.

Arrange in decreasing order of basicity,

$H_{2}O,O{H}^{-},C{H}_{3}OH,C{H}_3{O}^{-}$

1. $C{H}_{3}OH>C{H}_3{O}^{-}>H_{2}O>O{H}^{-}$

2. $C{H}_3{O}^{-}>O{H}^{-}>H_{2}O>C{H}_{3}OH$

3. $C{H}_3{O}^{-}>O{H}^{-}>C{H}_{3}OH>H_{2}O$

4. $C{H}_{3}OH>C{H}_3{O}^{-}>O{H}^{-}>H_{2}O$

Q.

The boiling point of methanol, water and dimethyl ether are respectively ${65}^{0}C,{100}^{0}Cand{34.5}^{0}C$. Which of the following best explains these wide variations in b.p.?

1. The molecular mass increases from water (18) to methanol (32) to diethyl ether (74)

2. The extent of H-bonding decreases from water to methanol while it is absent in ether

3. The extent of intramolecular H-bonding decreases from ether to methanol to water

4. The density of water is $1.00gm{l}^{-1}$, methanol $0.7914gm{l}^{-1}$ and that of diethyl ether is $0.7137gm{l}^{-1}$

Q.

The boiling point of methanol, water and dimethyl ether are respectively ${65}^{0}C,{100}^{0}Cand{34.5}^{0}C$. Which of the following best explains these wide variations in b.p.?

1. The molecular mass increases from water (18) to methanol (32) to diethyl ether (74)

2. The extent of H-bonding decreases from water to methanol while it is absent in ether

3. The extent of intramolecular H-bonding decreases from ether to methanol to water

4. The density of water is $1.00gm{l}^{-1}$, methanol $0.7914gm{l}^{-1}$ and that of diethyl ether is $0.7137gm{l}^{-1}$

Q. Pure phosphoric acid is very viscous. Because:

1. It is a strong acid
2. It is tribasic acid
3. It is hygroscopic
4. It forms hydrogen bonding

Q. The variation of the boiling points of the hydrogen halides is in the order $HF>HI>HBr>HCl$. What explains the higher boiling point of hydrogen fluoride?

1. The bond energy of $HF$ molecules is greater than in other hydrogen halides
2. The effect of nuclear shielding is much reduced in fluorine which polarises the $HF$ molecule
3. The electronegativity of fluorine is much higher than for other elements in the group.
4. There is strong hydrogen bonding between $HF$ molecules

Q. Arrange in decreasing order of acid strength.

$HF,HCl,HBr,HI$

1. $HF>HCl>HBr>HI$

2. $HCl>HBr>HI>HF$

3. $HI>HBr>HCl>HF$

4. $HBr>HI>HCl>HF$

Q. The variation of the boiling points of the hydrogen halides is in the order $HF>HI>HBr>HCl$. What explains the higher boiling point of hydrogen fluoride?

1. The bond energy of $HF$ molecules is greater than in other hydrogen halides
2. The effect of nuclear shielding is much reduced in fluorine which polarises the $HF$ molecule
3. The electronegativity of fluorine is much higher than for other elements in the group.
4. There is strong hydrogen bonding between $HF$ molecules

Q. Which of the following is not hygroscopic?

<!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> AIIMS 2011

1. $CsCl$
2. $LiCl$
3. $MgC{l}_2$
4. $CaC{l}_2$