Given these pairs of atoms, indicate whether the following bonds are polar or non-polar covalent bonds.
C-H
N-H
O-H
C-C
Polar
Polar
Polar
Non polar
To determine whether a bond is polar or non-polar covalent, we need to consider the electronegativity difference between the bonded atoms.
1. C-H bond: Carbon (C) has an electronegativity value of 2.5, and hydrogen (H) has an electronegativity of 2.1. The electronegativity difference is 0.4, which is relatively small. As a result, the C-H bond is considered non-polar covalent.
2. N-H bond: Nitrogen (N) has an electronegativity of 3.0, while hydrogen (H) has an electronegativity of 2.1. The electronegativity difference is 0.9, indicating a moderate polarity. Thus, the N-H bond is polar covalent.
3. O-H bond: Oxygen (O) has an electronegativity of 3.5, and hydrogen (H) has an electronegativity of 2.1. The electronegativity difference is 1.4, which is relatively large. Therefore, the O-H bond is considered polar covalent.
4. C-C bond: Carbon (C) has an electronegativity of 2.5, and the difference in electronegativity between two carbon atoms is zero. Since there is no electronegativity difference, the C-C bond is non-polar covalent.
You can determine the polarity of a bond by comparing the electronegativity values of the bonded atoms. The greater the electronegativity difference, the more polar the bond becomes.