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Is the bond SiCL in Cl3SiSiCl3 a pure or polar covalent?
Probably just covalent. You need ~ 1.4 variance in electronegativity to make a polar covalent bond. The variance here is only 1.26, so probably not a great enough variance.
How can you separate silicon from sand?
To separate silicon from sand, you can use a process called "extraction." Silicon is typically found in sand in the form of silicon dioxide (SiO₂). Here's a common method to separate silicon from sand: **Conversion to Silicon Tetrachloride (SiCl₄):** Heat a mixture of sand (SiO₂) and carbon in the presence of a catalyst (usually copper) to produce silicon carbide (SiC). [ SiO_2 + 3C \xrightarrow{\text{heat}} SiC + 2CO ] React silicon carbide with chlorine gas (Cl₂) to form silicon tetrachloride (SiCl₄). [ SiC + 2Cl_2 \rightarrow SiCl_4 + CCl_4 ] **Distillation:** Silicon tetrachloride is a volatile compound, and it can be separated from other components through distillation because of its different boiling point. **Reduction to Obtain Silicon:** React silicon tetrachloride with hydrogen gas (H₂) to obtain silicon and hydrochloric acid (HCl). [ SiCl_4 + 2H_2 \rightarrow Si + 4HCl ] The silicon obtained in this step is typically in a powdered form. **Purification:** The obtained silicon may undergo additional purification processes, such as zone refining or chemical purification, to achieve high-purity silicon. This process outlines a common method used in industry to extract silicon from sand. Keep in mind that industrial processes may vary, and the specific method used can depend on factors such as the required purity of the silicon and economic considerations.
Is the bond SiCL in Cl3SiSiCl3 a pure or polar covalent?
Probably just covalent. You need ~ 1.4 variance in electronegativity to make a polar covalent bond. The variance here is only 1.26, so probably not a great enough variance.
Is SiCl plus Mg---MgCl2 plus Si Balanced?
Mg + MgCl2
What is S for silicon tetrachloride?
SiCl4 Silicon tetrachloride or tetrachlorosilane is the inorganic compound with the formula SiCl₄. It is a colourless volatile liquid that fumes in air. It is used to produce high purity silicon and silica for commercial applications Formula: SiCl4 Molar mass: 169.9 g/mol Boiling point: 135.8°F (57.65°C) Melting point: -91.73°F (-68.74°C) Density: 1.48 g/cm³
How can you separate silicon from sand?
To separate silicon from sand, you can use a process called "extraction." Silicon is typically found in sand in the form of silicon dioxide (SiO₂). Here's a common method to separate silicon from sand: **Conversion to Silicon Tetrachloride (SiCl₄):** Heat a mixture of sand (SiO₂) and carbon in the presence of a catalyst (usually copper) to produce silicon carbide (SiC). [ SiO_2 + 3C \xrightarrow{\text{heat}} SiC + 2CO ] React silicon carbide with chlorine gas (Cl₂) to form silicon tetrachloride (SiCl₄). [ SiC + 2Cl_2 \rightarrow SiCl_4 + CCl_4 ] **Distillation:** Silicon tetrachloride is a volatile compound, and it can be separated from other components through distillation because of its different boiling point. **Reduction to Obtain Silicon:** React silicon tetrachloride with hydrogen gas (H₂) to obtain silicon and hydrochloric acid (HCl). [ SiCl_4 + 2H_2 \rightarrow Si + 4HCl ] The silicon obtained in this step is typically in a powdered form. **Purification:** The obtained silicon may undergo additional purification processes, such as zone refining or chemical purification, to achieve high-purity silicon. This process outlines a common method used in industry to extract silicon from sand. Keep in mind that industrial processes may vary, and the specific method used can depend on factors such as the required purity of the silicon and economic considerations.
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What is an optical fiber made of?
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