Question

List all the possible bonds that can occur between the elements \(\mathrm{P}, \mathrm{Cs}, \mathrm{O}\), and \(\mathrm{H}\). Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form for each bond.

Short answer

The possible bonds and their types between the elements P, Cs, O, and H are: - P-Cs: Polar covalent bond - P-O: Polar covalent bond - P-H: Non-polar covalent bond - Cs-O: Ionic bond - Cs-H: Polar covalent bond - O-H: Polar covalent bond

Step-by-step solution

1. P and Cs Bond

Computing the electronegativity difference between P and Cs: \(\Delta\mathrm{EN} = |2.19 - 0.79| = 1.4\) Since 0.4 < \(\Delta\mathrm{EN}\) < 1.7, the bond between P and Cs is polar covalent.

2. P and O Bond

Calculating the electronegativity difference between P and O: \(\Delta\mathrm{EN} = |2.19 - 3.44| = 1.25\) Since 0.4 < \(\Delta\mathrm{EN}\) < 1.7, the bond between P and O is polar covalent.

3. P and H Bond

Finding the electronegativity difference between P and H: \(\Delta\mathrm{EN} = |2.19 - 2.20| = 0.01\) Since \(\Delta\mathrm{EN}\) < 0.4, the bond between P and H is non-polar covalent.

4. Cs and O Bond

Computing the electronegativity difference between Cs and O: \(\Delta\mathrm{EN} = |0.79 - 3.44| = 2.65\) Since \(\Delta\mathrm{EN}\) > 1.7, the bond between Cs and O is ionic.

5. Cs and H Bond

Calculating the electronegativity difference between Cs and H: \(\Delta\mathrm{EN} = |0.79 - 2.20| = 1.41\) Since 0.4 < \(\Delta\mathrm{EN}\) < 1.7, the bond between Cs and H is polar covalent.

6. O and H Bond

Finding the electronegativity difference between O and H: \(\Delta\mathrm{EN} = |3.44 - 2.20| = 1.24\) Since 0.4 < \(\Delta\mathrm{EN}\) < 1.7, the bond between O and H is polar covalent. In summary: - P-Cs: Polar covalent bond - P-O: Polar covalent bond - P-H: Non-polar covalent bond - Cs-O: Ionic bond - Cs-H: Polar covalent bond - O-H: Polar covalent bond