Question

Arrange the following in the order of property indicated for each set

1. F2 cl2 br2 i2 increasing bond dissociation enthalpy.


2. HF HCL HBR HI increasing acidic strength.

3. NH3 PH3 AsH3 SbH3 BiH3 increasing basic strength.



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Answer 1

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step-by-step explanation:

1. Bond dissociation enthalpy of X—X bond decreases from Cl2 to I2 as the size of the atom increases.

=> F2 as an exception has smaller bond dissociation enthalpy than those of Cl2 and Br2.

=> The reason for the exception being a small size of F — atoms and large electron- electron repulsion among lone pairs of fluorine atoms.

=> Thus, the correct order is

Cl2 > Br2 > F2 > I2

2. The stability of hydrogen halide decreases down the group due to decrease in bond (H—X) dissociation enthalpy in the order

H—F > H—Cl > H—Br > H—I

=> Thus, the acidic strength increases from HF to HI in the following order

HF < HCl < HBr < HI

3. Basic character decreases down the group due to increase in atomic size.

=> These hydrides are living spaces due to the presence of lone pair of electrons on the central atom.

=> Order of basic character is

NH3 > PH3 > AsH3 > SbH3 ≥ BiH3

Answer 2

1) Cl2 Br2 I2 F2 left to right decreasing order

2)HF HCL HBr left to right increasing order

3)NH3< PH3< ASH3 <SBH3< BIH3