Question:
The boiling points of the following hydrides follow the order of
The boiling points of the following hydrides follow the order of
Updated On: Aug 15, 2024
- $\ce{SbH3 > NH3 > AsH3 > PH3}$
- $\ce{NH3 > AsH3 > PH3 > SbH3}$
- $\ce{SbH3 > AsH3 > PH3 > NH3}$
- $\ce{NH3 > PH3 > AsH3 > SbH3}$
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The Correct Option is A
Solution and Explanation
Boiling point of $\ce{NH_3}$ is high due to intermolecular hydrogen bonding. In others it varies directly with molecular weight of molecule due to increased van der Wall�s force. This force is least in $\ce{PH_3}$ & highest in $\ce{SbH_3}$.
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Concepts Used:
Group 16 Elements
The group 16 elements (oxygen group elements) of the periodic classification are also known as chalcogens because most of the copper ores have copper in the form of oxides and sulphides. The word chalcogen means “ore formation” which is derived from the Greek word “Chalcos” (Ore) and “gen” (formation).
There are 5 elements that come under Group 16 of the Modern Periodic Table namely:
- Oxygen (O)
- Sulphur (S)
- Selenium (Se)
- Tellurium (Te)
- Polonium (PO)
Electronic Configuration:
The general electronic configuration of the chalcogens can be written as ‘ns2np4’, where ‘n’ denotes the value of the principal quantum number corresponding to the valence shell of the element.
The electron configuration of the synthetic element livermorium (believed to be a chalcogen) is predicted to be [Rn]5f146d107s27p4.
Metallic Nature of the Group 16 Elements:
- Oxygen and sulfur are classified as non-metals.
- Selenium and tellurium are classified as metalloids.
- Under standard conditions, polonium exhibits metallic characteristics. However, it is important to note that polonium is a radioactive element.