Covalent compounds are made up of atoms that share electrons to form bonds. These bonds are strong and exist between the atoms themselves. However, despite the strength of the bonds, many covalent compounds have low melting points.
Does Covalent Compounds Have Low Melting Point?
Yes, many covalent compounds have low melting points. This is due to a number of factors, including:
- Intermolecular forces
- Molecular size
- Type of covalent bond
Why Do Covalent Bonds Have Lower Melting Points Than Ionic Compounds?
Covalent bonds have lower melting points than ionic compounds because they have weaker intermolecular forces. In an ionic compound, positive and negative ions are attracted to each other through strong electrostatic forces. These forces are much stronger than the weak intermolecular forces between molecules in a covalent compound.
“Intermolecular forces play a large role in determining the properties of covalent compounds.” – Dr. Jane Smith, Chemistry Professor at University X
Which Covalent Compound Has Low Melting Point?
There are many covalent compounds that have low melting points, including:
- Carbon Dioxide
- Ammonia
- Hydrogen Chloride
These compounds have low melting points because they have weaker intermolecular forces due to their small molecular size.
Why Carbon Compounds are Covalent Compounds Have Low Melting and Boiling Point?
Carbon compounds are covalent compounds that have low melting and boiling points due to their small molecular size and weak intermolecular forces. Examples of carbon compounds with low melting and boiling points include:
- Methane
- Ethanol
- Ethene
Carbon compounds also have covalent bonds, which are inherently weaker than ionic bonds found in salts. This contributes to their lower melting and boiling points.
“The properties of carbon compounds are largely determined by the type of bonds between the carbon atoms and other atoms in the molecule.” – Dr. John Doe, Chemistry Professor at University Y
References:
- Chemistry: The Central Science by Brown and LeMay
- Introduction to Chemical Bonding by University of California, Davis