p-Block Elements (Group 15–18) · Question 27

Name the gas that can readily decolourise acidified KMnO4 solution.

1. SO2
2. NO2
3. P2O5
4. CO2

HgCl2 and I2 both when dissolved in water containing I- ions, the pair of species formed is

1. HgI2, I-
2. HgI42-, I3-
3. Hg2I2, I-
4. HgI2, I3-

Match the compounds given in column I with the hybridisation and shape given in column II and mark the correct option

1. (a)-(iv), (b)-(iii), (c)-(i), (d)-(ii)
2. (a)-(iv), (b)-(i), (c)-(ii), (d)-(iii)
3. (a)-(i), (b)-(iii), (c)-(iv), (d)-(ii)
4. (a)-(i), (b)-(ii), (c)-(iv), (d)-(iii)

Which is the correct statement for the given acids?

1. Phosphinic acid is a monoprotic acid while phosphonic acid is a diprotic acid.
2. Phosphinic acid is a diprotic acid while phosphonic acid is a monoprotic acid.
3. Both are diprotic acids.
4. Both are triprotic acids.

Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?

1. Br2 > I2 > F2 > Cl2
2. F2 > Cl2 > Br2 > I2
3. I2 > Br2 > Cl2 > F2
4. Cl2 > Br2 > F2 > I2

When copper is heated with conc. HNO3 it produces

1. Cu(NO3)2, NO and NO2
2. Cu(NO3)2 and N2O
3. Cu(NO3)2 and NO2
4. Cu(NO3)2 and NO

Among the following the correct order of acidity is

1. HClO2 < HClO < HClO3 < HClO4
2. HClO4 < HClO2 < HClO < HClO3
3. HClO3 < HClO4 < HClO2 < HClO
4. HClO < HClO2 < HClO3 < HClO4

Hot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidizing behaviour?

1. Cu + 2H2SO4 CuSO4 + SO2 + 2H2O
2. 3S + 2H2SO4 3SO2 + 2H2O
3. C + 2H2SO4 CO2 + 2SO2 + 2H2O
4. CaF2 + H2SO4 CaSO4 + 2HF

Strong reducing behavior of H3PO2 is due to

1. high electron gain enthalpy of phosphorus
2. high oxidation state of phosphorus
3. presence of two -OH groups and one P-H bond
4. presence of one -OH group and two P-H bonds.

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