We elaborate the uses of sulfur and atomic properties with characteristics. Sulfur is a lemon-yellow chemical element with an atomic number 16. Its symbol is S and it belongs to the group of nonmetals and its usual state in nature is solid. Sulfur is located at position 16 on the periodic table.
On this page you can discover the chemical properties of sulfur and information about sulfur and other elements on the periodic table such as oxygen, selenium, phosphorus or chlorine. You will also learn what sulfur is for and know its uses through its properties associated with sulfur such as its atomic number or the usual state in which sulfur can be found.
You will be able to see sulfur qualities such as its melting and boiling point, its magnetic properties or what its chemical symbol is. In addition, here you will find information about its atomic properties such as the distribution of electrons in sulfur atoms and other properties.
For some elements, some of this information is unknown. In these cases we show the properties attributed to them.
One of the properties of non-metal elements such as sulfur is for example that non-metal elements are poor conductors of heat and electricity. Sulfur, like the other non-metal elements, has no luster. Due to their brittleness, nonmetals such as sulfur cannot be flattened to form sheets or stretched to become threads.
The state of sulfur in its natural form is solid. Sulfur is a lemon yellow chemical element and belongs to the group of non-metals. The atomic number of sulfur is 16. The chemical symbol for sulfur is S. The melting point of sulfur is 388.36 degrees Kelvin or 116.21 degrees Celsius or degrees Celsius. The boiling point of sulfur is 717.87 degrees Kelvin or 445.72 degrees Celsius or degrees Celsius.
Uses of sulfur
Sulfur is a bright yellow crystalline solid that is essential for life. If you’ve ever wondered what sulfur is for , here is a list of its possible uses:
- Most sulfur is converted to sulfuric acid. Sulfuric acid is extremely important to many industries around the world. It is used in the manufacture of fertilizers, petroleum refining, wastewater treatment, batteries lead for cars, ore mining, removal of oxide iron , nylon manufacturing and production of hydrochloric acid.
- Sulfur can be used as a pesticide and fungicide. Many farmers who grow organic food use sulfur as a natural pesticide and fungicide.
- Sulfur-containing magnesium sulfate is used as a laxative, in bath salts, and as a magnesium supplement for plants.
- Sulfur is important to life. Therefore, it is added to fertilizers (in soluble form) so that plants have more sulfur available in the soil.
- Carbon disulfide , a sulfur compound, can be used to make cellophane and rayon (a material used in clothing).
- Sulfur is used to vulcanize rubber. Rubber vulcanization makes it more difficult. It ensures that the rubber maintains its shape. Vulcanized rubber is used to make car tires, shoe soles, hoses, and ice hockey pucks.
- Other sulfur compounds (sulfites) are used to bleach the paper and preserve the fruit.
- Sulfur is also a component of gunpowder.
Atomic properties of sulfur
The atomic mass of an element is determined by the total mass of neutrons and protons that can be found in a single atom belonging to this element. As for the position where to find sulfur within the periodic table of the elements, sulfur is in group 16 and period 3. Sulfur has an atomic mass of 32,065 u.
The electronic configuration for sulfur is [Ne] 3s2 3p4. The electronic configuration of the elements, determines the form in which the electrons are structured in the atoms of an element. The average radius of sulfur is 100 pm, its atomic radius or Bohr radius is 88 pm, its covalent radius is 102 pm, and its Van der Waals radius is 180 pm. Sulfur has a total of 16 electrons whose distribution is as follows: In the first layer it has 2 electrons, in the second it has 8 electrons and in its third layer it has 6 electrons.
Below you can see a table showing the main characteristics of sulfur.
|Density||1960 kg / m3|
|Atomic mass||32,065 u|
|Average radius||100 pm|
|Covalent radius||102 pm|
|Van der Waals radio||180 pm|
|Electronic configuration||[Ne] 3s2 3p4|
|Electrons per layer||2, 8, 6|
|Oxidation states||+ -2,4,6 (strong acid)|
|Melting point||388.36 K|
|Boiling point||717.87 K|
|Heat of fusion||1.7175 kJ / mol|
|Vapor pressure||2.65 × 10-20Pa at 388 K|
|Specific heat||710 J / (K · kg)|
|Electric conductivity||5.0 × 10-16S / m|
|Thermal conductivity||0.269 W / (Km)|
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