6. Calculate the difference in electronegativity (ΔEN) for the bonds that would form between the groups of atoms listed below. State whether the bond would be ionic, polar covalent or non-polar covalent.
a. N and Cl
b. B and Br
c. B and F
d. Al and O
e. N and F
f. C and H
g. Mg and I
h. Li and S
i. C and F
j. Na and N
a. N and Cl: The electronegativity of N is 3.0 and the electronegativity of Cl is 3.2.
ΔEN = 3.2 - 3.0 = 0.2
The bond between N and Cl would be a polar covalent bond.
b. B and Br: The electronegativity of B is 2.0 and the electronegativity of Br is 2.8.
ΔEN = 2.8 - 2.0 = 0.8
The bond between B and Br would also be a polar covalent bond.
c. B and F: The electronegativity of B is 2.0 and the electronegativity of F is 4.0.
ΔEN = 4.0 - 2.0 = 2.0
The bond between B and F would be an ionic bond.
d. Al and O: The electronegativity of Al is 1.5 and the electronegativity of O is 3.5.
ΔEN = 3.5 - 1.5 = 2.0
The bond between Al and O would be an ionic bond.
e. N and F: The electronegativity of N is 3.0 and the electronegativity of F is 4.0.
ΔEN = 4.0 - 3.0 = 1.0
The bond between N and F would be a polar covalent bond.
f. C and H: The electronegativity of C is 2.5 and the electronegativity of H is 2.1.
ΔEN = 2.1 - 2.5 = -0.4
The bond between C and H would be a non-polar covalent bond.
g. Mg and I: The electronegativity of Mg is 1.2 and the electronegativity of I is 2.7.
ΔEN = 2.7 - 1.2 = 1.5
The bond between Mg and I would be a polar covalent bond.
h. Li and S: The electronegativity of Li is 1.0 and the electronegativity of S is 2.5.
ΔEN = 2.5 - 1.0 = 1.5
The bond between Li and S would be a polar covalent bond.
i. C and F: The electronegativity of C is 2.5 and the electronegativity of F is 4.0.
ΔEN = 4.0 - 2.5 = 1.5
The bond between C and F would be a polar covalent bond.
j. Na and N: The electronegativity of Na is 0.9 and the electronegativity of N is 3.0.
ΔEN = 3.0 - 0.9 = 2.1
The bond between Na and N would be an ionic bond.
are these correct?
Yes, these calculations are correct.
a. N and Cl:
To calculate the difference in electronegativity (ΔEN), subtract the electronegativity of the less electronegative atom from the electronegativity of the more electronegative atom.
Electronegativity value for N: 3.04
Electronegativity value for Cl: 3.16
ΔEN = 3.16 - 3.04 = 0.12
The difference in electronegativity (ΔEN) for the N-Cl bond is 0.12. Since the difference is small, the bond would be considered polar covalent.
b. B and Br:
Electronegativity value for B: 2.04
Electronegativity value for Br: 2.96
ΔEN = 2.96 - 2.04 = 0.92
The difference in electronegativity (ΔEN) for the B-Br bond is 0.92. Since the difference is moderate, the bond would be considered polar covalent.
c. B and F:
Electronegativity value for B: 2.04
Electronegativity value for F: 3.98
ΔEN = 3.98 - 2.04 = 1.94
The difference in electronegativity (ΔEN) for the B-F bond is 1.94. Since the difference is relatively large, the bond would be considered ionic.
d. Al and O:
Electronegativity value for Al: 1.61
Electronegativity value for O: 3.44
ΔEN = 3.44 - 1.61 = 1.83
The difference in electronegativity (ΔEN) for the Al-O bond is 1.83. Since the difference is relatively large, the bond would be considered ionic.
e. N and F:
Electronegativity value for N: 3.04
Electronegativity value for F: 3.98
ΔEN = 3.98 - 3.04 = 0.94
The difference in electronegativity (ΔEN) for the N-F bond is 0.94. Since the difference is moderate, the bond would be considered polar covalent.
f. C and H:
Electronegativity value for C: 2.55
Electronegativity value for H: 2.20
ΔEN = 2.55 - 2.20 = 0.35
The difference in electronegativity (ΔEN) for the C-H bond is 0.35. Since the difference is small, the bond would be considered nonpolar covalent.
g. Mg and I:
Electronegativity value for Mg: 1.31
Electronegativity value for I: 2.66
ΔEN = 2.66 - 1.31 = 1.35
The difference in electronegativity (ΔEN) for the Mg-I bond is 1.35. Since the difference is relatively large, the bond would be considered ionic.
h. Li and S:
Electronegativity value for Li: 0.98
Electronegativity value for S: 2.58
ΔEN = 2.58 - 0.98 = 1.60
The difference in electronegativity (ΔEN) for the Li-S bond is 1.60. Since the difference is relatively large, the bond would be considered ionic.
i. C and F:
Electronegativity value for C: 2.55
Electronegativity value for F: 3.98
ΔEN = 3.98 - 2.55 = 1.43
The difference in electronegativity (ΔEN) for the C-F bond is 1.43. Since the difference is relatively large, the bond would be considered polar covalent.
j. Na and N:
Electronegativity value for Na: 0.93
Electronegativity value for N: 3.04
ΔEN = 3.04 - 0.93 = 2.11
The difference in electronegativity (ΔEN) for the Na-N bond is 2.11. Since the difference is relatively large, the bond would be considered ionic.
To calculate the difference in electronegativity (ΔEN) for the bonds and determine if they are ionic, polar covalent, or non-polar covalent, you will need to refer to the electronegativity values of the elements involved. The most commonly used electronegativity scale is the Pauling scale.
1. N and Cl:
The electronegativity of N is 3.0, and the electronegativity of Cl is 3.0. The difference in electronegativity (ΔEN) is 3.0 - 3.0 = 0.0. Since the ΔEN is zero, the bond formed between N and Cl is non-polar covalent.
2. B and Br:
The electronegativity of B is 2.0, and the electronegativity of Br is 2.8. The difference in electronegativity (ΔEN) is 2.8 - 2.0 = 0.8. This indicates a moderately polar covalent bond.
3. B and F:
The electronegativity of B is 2.0, and the electronegativity of F is 3.9. The difference in electronegativity (ΔEN) is 3.9 - 2.0 = 1.9. This suggests a highly polar covalent bond.
4. Al and O:
The electronegativity of Al is 1.5, and the electronegativity of O is 3.5. The difference in electronegativity (ΔEN) is 3.5 - 1.5 = 2.0. This indicates a highly polar covalent bond.
5. N and F:
The electronegativity of N is 3.0, and the electronegativity of F is 3.9. The difference in electronegativity (ΔEN) is 3.9 - 3.0 = 0.9. This suggests a moderately polar covalent bond.
6. C and H:
The electronegativity of C is 2.5, and the electronegativity of H is 2.1. The difference in electronegativity (ΔEN) is 2.5 - 2.1 = 0.4. This indicates a non-polar covalent bond.
7. Mg and I:
The electronegativity of Mg is 1.2, and the electronegativity of I is 2.5. The difference in electronegativity (ΔEN) is 2.5 - 1.2 = 1.3. This suggests a moderately polar covalent bond.
8. Li and S:
The electronegativity of Li is 1.0, and the electronegativity of S is 2.5. The difference in electronegativity (ΔEN) is 2.5 - 1.0 = 1.5. This indicates a moderately polar covalent bond.
9. C and F:
The electronegativity of C is 2.5, and the electronegativity of F is 3.9. The difference in electronegativity (ΔEN) is 3.9 - 2.5 = 1.4. This suggests a moderately polar covalent bond.
10. Na and N:
The electronegativity of Na is 0.9, and the electronegativity of N is 3.0. The difference in electronegativity (ΔEN) is 3.0 - 0.9 = 2.1. This indicates a highly polar covalent bond.
Remember, the classification of bonds as ionic, polar covalent, or non-polar covalent is based on the range of electronegativity differences. Here is a general guideline:
- ΔEN below 0.4: Non-polar covalent bond
- ΔEN between 0.4 and 1.7: Polar covalent bond
- ΔEN above 1.7: Ionic bond