The melting point of a compound is not influenced by which of the following?
A. polarity
B. electronegativity of its atoms
C. Van der Waals forces
D. hydrogen bonds
E. isotope of carbon
No answers.
Van der Waals forces
Polarity
To determine which of the following does not influence the melting point of a compound, we can consider each option and its correlation to melting point.
A. Polarity: Polarity can affect the intermolecular forces between molecules, which can in turn impact the melting point. For example, polar compounds tend to have higher melting points than nonpolar compounds. Therefore, polarity does influence the melting point.
B. Electronegativity of its atoms: The electronegativity of atoms plays a role in determining the polarity of a compound, as previously mentioned. Since polarity can affect the melting point, it follows that the electronegativity of atoms indirectly influences the melting point.
C. Van der Waals forces: Van der Waals forces, which include London dispersion forces, dipole-dipole interactions, and hydrogen bonding, are intermolecular forces that affect the melting point. Compounds with stronger Van der Waals forces tend to have higher melting points.
D. Hydrogen bonds: Hydrogen bonding is a type of intermolecular force that is particularly strong, resulting in higher melting points for compounds that can form hydrogen bonds. Therefore, hydrogen bonds do influence the melting point.
E. Isotope of carbon: The isotopes of an element have no significant influence on the chemical properties of a compound. Since the melting point is a physical property and is determined by the intermolecular forces, the isotope of carbon would not have a direct impact on the melting point.
Therefore, the correct answer is E. the isotope of carbon.