Tell whether the bonds between the following atoms are polar covalent or pure covalent bonds.

a. Si-Si b. H-O c. C-H d. C-O e. Cl-F
f. Cl-Cl g. N-H h. O-O

Si to Si and Cl to Cl are about as pure covalent as you can get. Bonds between the same elements (or elements of the same electronegativity) are essentially pure covalent. Other bonds such as those between H and O for example(H is about 2.1 and O about 3.5) are polar covalent since 3.5-2.1 is not zero.

Thank you again!

To determine whether the bonds between the given atoms are polar covalent or pure covalent, we need to compare the electronegativities of the atoms involved in each bond.

a. Si-Si: Pure covalent bond
Silicon (Si) has an electronegativity value of 1.90. Since the electronegativity difference between the two Si atoms is zero, the bond is considered pure covalent.

b. H-O: Polar covalent bond
Hydrogen (H) has an electronegativity value of 2.20, while oxygen (O) has a value of 3.44. The electronegativity difference between H and O is 1.24, which indicates a polar covalent bond.

c. C-H: Nonpolar covalent bond
Carbon (C) has an electronegativity value of 2.55, while hydrogen (H) has an electronegativity value of 2.20. The electronegativity difference between C and H is 0.35, which is considered small. Therefore, the bond is nonpolar covalent.

d. C-O: Polar covalent bond
Carbon (C) has an electronegativity value of 2.55, while oxygen (O) has a value of 3.44. The electronegativity difference between C and O is 0.89, indicating a polar covalent bond.

e. Cl-F: Polar covalent bond
Chlorine (Cl) has an electronegativity value of 3.16, while fluorine (F) has a value of 3.98. The electronegativity difference between Cl and F is 0.82, indicating a polar covalent bond.

f. Cl-Cl: Pure covalent bond
Chlorine (Cl) has an electronegativity of 3.16. Since the two Cl atoms are the same, the electronegativity difference is zero, indicating a pure covalent bond.

g. N-H: Polar covalent bond
Nitrogen (N) has an electronegativity value of 3.04, while hydrogen (H) has an electronegativity value of 2.20. The electronegativity difference between N and H is 0.84, indicating a polar covalent bond.

h. O-O: Pure covalent bond
Oxygen (O) has an electronegativity value of 3.44. Since the two O atoms are the same, the electronegativity difference is zero, indicating a pure covalent bond.

To determine whether a bond is polar covalent or pure covalent, you need to consider the electronegativity difference between the atoms involved in the bond.

Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. The electronegativity values range from 0 to 4, with larger values indicating a greater ability to attract electrons.

For polar covalent bonds, there is an unequal sharing of electrons between the atoms, resulting in a partial positive charge on one atom and a partial negative charge on the other. In pure covalent bonds, the electronegativity difference is essentially zero, and the sharing of electrons is equal.

Now let's analyze the bonds:

a. Si-Si: Silicon (Si) has an electronegativity of 1.90. Since both atoms in this bond are the same element, the electronegativity difference is zero. Therefore, the bond is pure covalent.

b. H-O: Hydrogen (H) has an electronegativity of 2.20, while oxygen (O) has an electronegativity of 3.44. The electronegativity difference is 1.24, indicating a polar covalent bond. Oxygen attracts electrons more strongly, creating a partial negative charge on the oxygen atom and a partial positive charge on the hydrogen atom.

c. C-H: Carbon (C) has an electronegativity of 2.55, while hydrogen (H) has an electronegativity of 2.20. The electronegativity difference is 0.35, which is relatively small. This indicates a pure covalent bond.

d. C-O: Carbon (C) has an electronegativity of 2.55, and oxygen (O) has an electronegativity of 3.44. The electronegativity difference is 0.89, which suggests a polar covalent bond. Oxygen attracts electrons more strongly, creating a partial negative charge on the oxygen atom and a partial positive charge on the carbon atom.

e. Cl-F: Chlorine (Cl) has an electronegativity of 3.16, while fluorine (F) has an electronegativity of 3.98. The electronegativity difference is 0.82, indicating a polar covalent bond. Fluorine attracts electrons more strongly, creating a partial negative charge on the fluorine atom and a partial positive charge on the chlorine atom.

f. Cl-Cl: Chlorine (Cl) has an electronegativity of 3.16, and in this case, both atoms are the same. Therefore, the electronegativity difference is zero, making it a pure covalent bond.

g. N-H: Nitrogen (N) has an electronegativity of 3.04, and hydrogen (H) has an electronegativity of 2.20. The electronegativity difference is 0.84, indicating a polar covalent bond. Nitrogen attracts electrons more strongly, creating a partial negative charge on the nitrogen atom and a partial positive charge on the hydrogen atom.

h. O-O: Oxygen (O) has an electronegativity of 3.44, and in this case, both atoms are the same. Therefore, the electronegativity difference is zero, making it a pure covalent bond.

Remember that the determination of polarity is not always absolute, and a bond may have a varying degree of polarity. These values are only approximate and provide a general understanding of the bond type.