To determine the type of bond that will form between the elements in each set based on their electronegativity differences, we begin by calculating the differences using standard electronegativity values:
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Calcium (Ca) and Chlorine (Cl) in CaCl2:
- Electronegativity of Ca: 1.00
- Electronegativity of Cl: 3.16
- Difference: |1.00 - 3.16| = 2.16
- This difference indicates an ionic bond.
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Fluorine (F) and Fluorine (F) in F2:
- Electronegativity of F: 3.98
- Difference: |3.98 - 3.98| = 0
- This difference indicates a nonpolar covalent bond.
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Nitrogen (N) and Fluorine (F) in NF3:
- Electronegativity of N: 3.04
- Electronegativity of F: 3.98
- Difference: |3.04 - 3.98| = 0.94
- This difference indicates a polar covalent bond.
Now, we can match these findings with the options provided in Column B:
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Calcium (Ca) and Chlorine (Cl) in CaCl2:
- The electronegativity difference is 2.16. The bond will be ionic (closest option: e).
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Fluorine (F) and Fluorine (F) in F2:
- The electronegativity difference is 0. The bond will be nonpolar covalent (option: c).
-
Nitrogen (N) and Fluorine (F) in NF3:
- The electronegativity difference is 0.94. The bond will be polar covalent (closest option: a).
Summary:
- Calcium (Ca) and Chlorine (Cl) - Difference: 2.16 - Ionic (Option e)
- Fluorine (F) and Fluorine (F) - Difference: 0 - Nonpolar covalent (Option c)
- Nitrogen (N) and Fluorine (F) - Difference: 0.94 - Polar covalent (Option a)
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