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Silicon was not initially characterized in its pure form until the year 1824 when scientist Jons Jakob Berzelius first managed to do so. Silicon was characterized in its pure form because of the fact that it has a high chemical affinity to oxygen. The oxides form the silicon form Silicates, which contain silicon and oxygen. Silicon’s melting point is surpassed by only boron out of all the metalloids and nonmetals. Si is a strong but breakable crystalline, and has a metallic blue-grey colour, and Si is tetravalent, that is, its valency is 4, also a semiconductor. For the most part, Silicon is unreactive. Let’s learn more about silicon and discuss some important questions.
| Table of Content |
Key Takeaways: Silicates, semiconductor, compounds, germanium, flerovium, aluminum-silicon, Oxygen, metalloids
What is Silicon?
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Silicon is a member of the carbon family and is a non-metallic chemical, has an atomic number 14, and is part of group 14, the 3rd phase in the p-block of the periodic table. Carbon is above it, while germanium, tin, lead, and flerovium are below it. Silicon is metallic, one of seven compounds that have both non-metallic and metallic properties depending on the element it encounters. The silicon used in electronics acts like metal, while the silicon composite glass has non-metallic properties. This element is defined as 'Si'. Electronic silicon configuration is (Ne) 3s2 3p2. Silicon is solid at 20 ° C. Si is used in moulding compounds.
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Properties of Silicon
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- One of silicon's allotrope is in the form of needle-like crystals, glossy, dark grey or flat plates, while others have no crystalline structure and are usually present in a brown powder.
- The atomic number of silicon is 14 and its relative atomic weight is 28.085 u.
- Silicon density is 2.3296 grams per cubic centimetre.
- The melting point of the silicon is 1,410 ° C and its boiling point is 3,265 ° C.
- Silicon is purely an internal semiconductor although adding impurities in small quantities helps to greatly increase semiconductor power.
- Silicon is electropositive only in its chemical properties, has a metallic lusture, and is considered very brittle.
- Silicon is very similar to metals in terms of chemical behaviour.
- At room temperature, silicon is a non-functional element. Being sturdy, it does not absorb oxygen or other closely related nutrients.
- Silicon is highly effective at high temperatures.
- Silicon also contains oxygen, phosphorus, nitrogen, and other nutrients. It also forms alloys in a melted state.
Uses of Silicon
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- Silicon is used in the manufacture of bricks, mortar, and fire bricks.
- Silicon is used to make many alloys such as aluminum-silicon and ferrosilicon known as iron-silicon which is widely used in the steel industry.
- Silicon is used to make silicon-oxygen polymers with a methyl adhesive group known as silicone and its oil is a lubricant added to hair conditioner and cosmetics.
- Silicone rubber is used in waterproofing systems for toilets, roofs and plumbing.
- As a semiconductor, silicon is used in transistors and solid-state devices that include microelectronics and the computer industry.
- The raw form of silicon is used to make silica sand, clay, and stone.
- Highly purified silicon is also used in electronics.
Things to Remember
- Silicon split and was forced to upgrade its first crystals in 1854.
- In the periodic table, one can find silicon under carbon in the third row of the periodic table.
- In Portland, the most common type of cement, silicates are used.
- Silicon electrons are arranged in a carbon-like manner.
- In 1824, Silicon was discovered by Jons Jacob Berzelius.
- The silicon atomic structure consists of 14 electrons with 4 electrons in the outer shell (with high energy), 8 electrons in the second orbit, and 2 electrons in the first orbit.
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Sample Questions
Ques. How does Silicon occur in nature? (2 marks)
Ans. Silicon is the second most abundant electropositive component that makes up 27.7% of the world's crust mass. It occurs in an ecosystem called silicon dioxide known as silica. About 97% of the earth's crust is made up of rocks and contains silicon and oxygen compounds. Silicon is present in nature in many forms of oxide, forming compounds with oxygen, phosphorus, magnesium, and others. Minerals containing silicon dioxide are known as silicates.
Ques. State few chemical properties of silicon. (4 marks)
Ans.
- Silicon is very similar to metals in terms of chemical behaviour.
- At room temperature, silicon is a non-functional element. Being sturdy, it does not absorb oxygen or other closely related nutrients.
- Silicon is highly effective at high temperatures.
- Silicon also contains oxygen, phosphorus, nitrogen, and other nutrients. It also forms alloys in a melted state.
Ques. Give 4 uses of Silicon. (4 marks)
Ans.
- The raw form of silicon is used to make silica sand, clay, and stone.
- Highly purified silicon is also used in electronics.
- Silicon is used in the manufacture of bricks, mortar, and fire bricks.
- Silicon is used to make many alloys such as aluminum-silicon and ferrosilicon known as iron-silicon which is widely used in the steel industry.
Ques. Name a few compounds of Silicon. (4 marks)
Ans.
- Silicides: - Silicides have similar properties to borides and carbides. Because of their similar structure, the structural temperature of these elements is the same. Silicon carbide is also known as Carborundum which is widely used as a powder for polishing or grinding other materials and has antagonistic properties.
- Silica: - Silica (Silicon dioxide) mainly contains granite and sandstone used for glass construction, abrasives, water filters, as a food additive, and much more.
- Halides: - Silicon compounds, especially carbides, form silicon tetrahalides when they react with stable halogens. Unlike carbon tetrahalides, these easily convert hydrolyze into water.
- Silicic Acids: - Silica gases are formed due to increased water concentration. Many silica gels are found occurring in wetlands.
Ques. Does silicon have any isotopes? (3 marks)
Ans. Yes, the silicon element has an isotope. Silicon has a total of five known isotopes in which three isotopes are naturally occurring. Silicon-28, Silicon-29, and Silicon-30 are naturally occurring siloton isotopes. Natural Silicon comprises these three isotopes in 92.2% silicon-28, 4.7% silicon-29, and 3.1% silicon-30 respectively and all of these isotopes are stable. Silicon-28 and Silicon-30 are considered essential silicon isotopes. In addition to naturally occurring isotopes, silicon has well-known synthetic radioactive isotopes. These isotopes made of silicon radiation have no commercial function.
Ques. What are the health effects of silicon? (2 marks)
Ans. Silicon dust affects the lungs less aggressively and does not appear to produce toxic effects or organic disease in the event of exposed to exposure limits.
- Silicon has the potential to cause permanent respiratory effects because silicon dioxide (crystalline silica) is a potent respiratory hazard.
- Crystalline silicon, when in contact with the eyes and skin, acts as an irritator. It leads to dizziness and redness of the eyes due to irritation. Inhaling silicon will cause irritation to the mucous membranes and lungs. Skin inflammation is characterized by itching, redness, and elasticity.
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