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Chapter 1: Q18E (page 55)

A sulfur atom and a sulfur molecule are not identical. What is the difference?

Short Answer

Expert verified

A sulfur atom does not exist in nature, while a sulfur molecule exists. The reasons are given as follows:

Step by step solution

01

Describing the structure of the sulfur molecule

Sulfur exists inallotropic forms. Each S forms two bonds in this structure, with each S atom having two lone pairs.

The sulfur molecule has a crown-like cyclic or ring octagonal structure with the formula of S8.

02

Describing the sulfur exists in molecular rather than atomic with S8 molecular formula

The sulphur atom has an electronic configuration of 1s2,2s2 2p6,3s2 3p4. For complete stability, the last two half-filled orbitals need to be filled. Hence, to gain a stable electronic configuration sulfur atom shares electrons with another sulfur atom and forms two covalent bonds each.

Also, the sulfur atom is large with the Vander Waals force between the atoms. It forms a pi-pi bond but is not stable as oxygen.

Therefore, the sulfur atom and sulfur molecule are not identical, and the sulfur does not exist in nature in atomic form while the molecular form exists.

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Most popular questions from this chapter

Convert the boiling temperature of liquid ammonia, \( - 28.1^\circ F,\) into degrees Celsius and kelvin.

Explain the difference between extensive properties and intensive properties.

(a) To three decimal places, what is the volume of a cube with an edge length of?(b) If the cube in part (a) is copper and has a mass of what is the density of copper to two decimal places

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Both graphite and diamond burn.

\({\bf{C}}\left( {{\bf{s, diamond}}} \right){\bf{ + }}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right) \to {\bf{C}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right)\)

For the conversion of graphite to diamond:

\({\bf{C}}\left( {{\bf{s, graphite}}} \right) \to {\bf{C}}\left( {{\bf{s, diamond}}} \right){\bf{ \Delta {\rm H}}}_{{\bf{298}}}^{\bf{^\circ }}{\bf{ = 1}}{\bf{.90 kJ}}\)

Which produces more heat, the combustion of graphite or the combustion of a diamond?
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