Answer
See the explanation
Work Step by Step
a. C-O bond:
The electronegativity difference between carbon (2.55) and oxygen (3.44) is significant, indicating a polar covalent bond. The oxygen atom, being more electronegative, will have a partial negative charge (δ-), while the carbon atom will have a partial positive charge (δ+).
b. P-H bond:
The electronegativity difference between phosphorus (2.19) and hydrogen (2.20) is small, indicating a relatively non-polar covalent bond. The bond will have a slight polarity, with the hydrogen atom having a slightly positive charge (δ+) and the phosphorus atom having a slightly negative charge (δ-).
c. H-Cl bond:
The electronegativity difference between hydrogen (2.20) and chlorine (3.16) is significant, indicating a polar covalent bond. The chlorine atom, being more electronegative, will have a partial negative charge (δ-), while the hydrogen atom will have a partial positive charge (δ+).
d. Br-Te bond:
The electronegativity difference between bromine (2.96) and tellurium (2.10) is significant, indicating a polar covalent bond. The bromine atom, being more electronegative, will have a partial negative charge (δ-), while the tellurium atom will have a partial positive charge (δ+).
e. Se-S bond:
The electronegativity difference between selenium (2.55) and sulfur (2.58) is small, indicating a relatively non-polar covalent bond. The bond will have a slight polarity, with the sulfur atom having a slightly positive charge (δ+) and the selenium atom having a slightly negative charge (δ-).
