Given the electronegativity values of N (3.0) and O (3.5), illustrate the bond polarity in a nitrogen monoxide molecule, NO, using delta notation.

1. Identify the electronegativity values: Nitrogen (N) has an electronegativity of 3.0 and Oxygen (O) has an electronegativity of 3.5.

2. Determine the difference in electronegativity: The difference in electronegativity between N and O is 3.5 - 3.0 = 0.5.

3. Determine the bond polarity: Since the difference in electronegativity is 0.5, which is less than 1.7, the bond is polar covalent.

4. Illustrate the bond polarity using delta notation: In a polar covalent bond, the atom with the higher electronegativity is partially negative (δ-) and the atom with the lower electronegativity is partially positive (δ+). Therefore, in the NO molecule, Oxygen (O) is δ- and Nitrogen (N) is δ+.

So, the bond polarity of NO can be represented as follows: N(δ+) - O(δ-)