Read the passage given below and answer the following question
Current investigations, for example, on antimony(III) and arsenic(III) halogen compounds, have indicated quite similar structural principles as in Te(IV) analogous. In the series of the binary halides of selenium and tellurium the crystal structure determinations of tellurium tetrafluoride and of tellurium tetrachloride on twinned crystal are the key to understanding the various and partly contradictory spectroscopic and other macroscopic properties, a well as the synthetic potential of the compounds. The chapter discusses the characteristic structural and bonding features of the halogen compounds of the chalcogen(IV) systems, in which the role of the inert pair determines much of the stereochemistry and reactive properties of the whole class of compounds. `SCl_4` as the only stable tetrahalide of sulfur besides `SF_4`, is known to be easily prepared at temperatures below `-34^@C` from the elements or from the reversible reaction of equimolar amounts of `SC_12` and chlorine.
Source : https:`////`www.researchgate.net`//`publication`//`277691468_A_Summary_of_Functional_Groups_Containing_Selenium_and_Tellurium_A_Catalog_of_the_Many_Groups_that_are_Known_and_Some_that _are_Not
The boiling points of hydrides of group 16 are in the order:

Options

A. `H_2O gt H_2Te gt H_2S gt H_2Se`
B. `H_2O gt H_2S gt H_2Se gt H_2Te`
C. `H_2O gt H_2 gt H_2Se gt H_2S`
D. None of these

Answer

To determine the order of the boiling points of the hydrides of Group 16 elements (which include H2S, H2Se, H2Te, and H2Po), we need to consider the factors that influence boiling points, such as molecular size, intermolecular forces, and the presence of hydrogen bonding.

### Step-by-Step Solution:

1. **Identify the Hydrides of Group 16**:
The hydrides of Group 16 elements are:
- H2O (water)
- H2S (hydrogen sulfide)
- H2Se (hydrogen selenide)
- H2Te (hydrogen telluride)
- H2Po (hydrogen polonide, though it is less common)

2. **Understand the Role of Molecular Size**:
As we move down the group from sulfur (S) to tellurium (Te), the molecular size increases. This generally leads to an increase in boiling points due to stronger Van der Waals forces (dispersion forces) between larger molecules.

3. **Consider Hydrogen Bonding**:
Hydrogen bonding significantly affects the boiling points of certain hydrides, particularly H2O. Water has a much higher boiling point than expected due to strong hydrogen bonds. In contrast, H2S, H2Se, and H2Te do not exhibit hydrogen bonding to the same extent.

4. **Analyze the Boiling Points**:
- H2O has a boiling point of 100°C due to hydrogen bonding.
- H2S has a boiling point of -60°C.
- H2Se has a boiling point of -41°C.
- H2Te has a boiling point of -2°C.
- H2Po is less studied, but it is expected to have a boiling point higher than H2Te due to increased molecular size.

5. **Establish the Order**:
Based on the analysis, the order of boiling points for the hydrides of Group 16 can be summarized as:
- H2O > H2Te > H2Se > H2S

### Final Order of Boiling Points:
**H2O > H2Te > H2Se > H2S**