Since at normal room temperature methanol is a liquid and silicon is a solid, it should be fairly obvious that the answer is "no."
Silicon dioxide. Silicon dioxide silica is the mineral quartz and is a giant molecule with a melting point of over 16000C. Methanol is a molecular compound (an alcohol) with a melting point of -980C
Chlorine has a higher melting point than silicon because chlorine molecules are held together by stronger covalent bonds compared to the silicon atoms in silicon. This makes it harder to break the bonds in chlorine, requiring higher temperatures to melt. Silicon has weaker metallic bonds which results in a lower melting point.
The melting point of silicon is: 1 414 0C.
The melting point of silicon is 1683 K. The boiling point of silicon is 2628 K.
The melting point of silicon is 1414 degrees Celsius (2577 degrees Fahrenheit). At this temperature, silicon transitions from a solid to a liquid state.
Silicon dioxide. Silicon dioxide silica is the mineral quartz and is a giant molecule with a melting point of over 16000C. Methanol is a molecular compound (an alcohol) with a melting point of -980C
Silicon dioxide has a higher melting point than methanol. Silicon dioxide requires temperatures of around 1710 degrees Celsius to melt, while methanol melts at -98 degrees Celsius.
Chlorine has a higher melting point than silicon because chlorine molecules are held together by stronger covalent bonds compared to the silicon atoms in silicon. This makes it harder to break the bonds in chlorine, requiring higher temperatures to melt. Silicon has weaker metallic bonds which results in a lower melting point.
Methanol melts between -98oC and -97oC. It boils at 64.7oC.
Melting point depends upon the binding forces among the atoms or molecules and compactness of the material , the pure Silicon as an element has great compactness as compare to its compound SiCl4.
The melting point of silicon is: 1 414 0C.
Siliocone has a higher one. Chlorine is already a gas at room temperature.
Silicon dioxide has a higher melting point than oxygen because the covalent bonds in silicon dioxide are stronger than the diatomic oxygen molecules, requiring more energy to break them apart and transition from solid to liquid state. Additionally, silicon dioxide has a more complex crystal structure with a higher degree of symmetry, contributing to its higher melting point compared to oxygen.
At STP, neon is a gas, so its melting point is low whereas silicon is a solid, so its melting point is high
The melting point of silicon is 1683 K. The boiling point of silicon is 2628 K.
The melting point of silicon is 1414 degrees Celsius (2577 degrees Fahrenheit). At this temperature, silicon transitions from a solid to a liquid state.
Silicon dioxide has a higher melting point than silicon tetrachloride because silicon dioxide forms a network solid structure with strong covalent bonds, requiring more energy to break compared to the weaker forces holding silicon tetrachloride molecules together. Additionally, silicon dioxide molecules are larger and have a higher molecular weight, contributing to a stronger intermolecular forces between the molecules.