Which compound is most likely to be held together by a covalent bond based on the electronegativity difference between its two atoms?
(1 point)
CaBr
CaBr
NO
NO
NaCl
NaCl
CO
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Answer is
NO
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To determine which compound is most likely to be held together by a covalent bond based on the electronegativity difference between its two atoms, we need to compare the electronegativity values of the atoms in each compound.
The electronegativity is a measure of an atom's tendency to attract electrons towards itself in a chemical bond. On the Pauling scale, electronegativity values range from 0.7 (for cesium) to 4.0 (for fluorine).
For a covalent bond to form, the electronegativity difference between the two atoms should be relatively small, usually less than 1.7. A large electronegativity difference indicates an ionic bond, where electrons are completely transferred from one atom to another.
Let's compare the electronegativity values for the compounds you provided:
1. CaBr: Calcium (Ca) has an electronegativity of 1.0, while Bromine (Br) has an electronegativity of 2.8. The electronegativity difference is 1.8, which is larger than 1.7, suggesting an ionic bond.
2. NO: Nitrogen (N) has an electronegativity of 3.0, while Oxygen (O) has an electronegativity of 3.5. The electronegativity difference is 0.5, which is smaller than 1.7, indicating a covalent bond.
3. NaCl: Sodium (Na) has an electronegativity of 0.9, while Chlorine (Cl) has an electronegativity of 3.0. The electronegativity difference is 2.1, which is larger than 1.7, suggesting an ionic bond.
4. CO: Carbon (C) has an electronegativity of 2.5, while Oxygen (O) has an electronegativity of 3.5. The electronegativity difference is 1.0, which is smaller than 1.7, indicating a covalent bond.
Based on the electronegativity differences, the compound most likely to be held together by a covalent bond is CO (carbon monoxide).