To calculate the electronegativity difference between carbon and hydrogen atoms in methane CH4 , we need to know the electronegativity values of both carbon and hydrogen. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. The most commonly used scale for electronegativity is the Pauling scale.According to the Pauling scale:- Electronegativity of Carbon C = 2.55- Electronegativity of Hydrogen H = 2.20Now, we can calculate the electronegativity difference between carbon and hydrogen atoms.Electronegativity difference EN = | Electronegativity of Carbon - Electronegativity of Hydrogen |EN = | 2.55 - 2.20 |EN = 0.35The electronegativity difference between carbon and hydrogen in methane is 0.35.Now, let's interpret what this value indicates about the bonding between the atoms. In general, the greater the electronegativity difference between two atoms, the more polar the bond between them will be. Here's a rough guideline for classifying bonds based on electronegativity difference:- Nonpolar covalent bond: EN < 0.5- Polar covalent bond: 0.5 EN < 1.7- Ionic bond: EN 1.7Since the electronegativity difference between carbon and hydrogen in methane 0.35 is less than 0.5, the bond between carbon and hydrogen in methane is considered a nonpolar covalent bond. This means that the electrons are shared relatively equally between the carbon and hydrogen atoms, and there is no significant charge separation between them.