QQuestionChemistry
QuestionChemistry
"An electronegativity difference ≥ 1.7 indicates an ________ (sometimes you see 2.0 instead of 1.7). An electronegativity difference ≤ 0.5 is generally considered ___________. If it is somewhere in the middle, it is considered ________.
ionic bond, covalent bond, polar covalent bond
ionic bond, polar covalent bond, covalent bond
covalent bond, ionic bond, polar covalent bond
covalent bond, polar covalent bond, ionic bond"
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Answer
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Step 1:: Understand the problem and its context
The problem provides a range of electronegativity differences and asks us to categorize the type of bond based on these differences. Electronegativity is a property that describes an atom's ability to attract electrons in a covalent bond. The higher the electronegativity, the more an atom attracts electrons.
Step 2:: Define the bond types
- Ionic bond: A bond where one atom (usually a metal) donates an electron to another atom (usually a nonmetal) to form a stable octet. The electronegativity difference is generally large (≥ 1.7). - Covalent bond: A bond where atoms share electrons to form a stable octet. The electronegativity difference is small or zero (≤ 0.5). - Polar covalent bond: A bond where atoms share electrons unequally, leading to a charge imbalance. This happens when the electronegativity difference is in the middle (0.5 < x < 1.7).
Step 3:: Categorize the bond types
Given the electronegativity difference ranges from the problem: - If the electronegativity difference is greater than or equal to 1.7, it forms an ionic bond: ionic bond, polar covalent bond, ionic bond - If the electronegativity difference is less than or equal to 0.5, it forms a covalent bond: covalent bond, ionic bond, covalent bond - If the electronegativity difference is between 0.5 and 1.7, it forms a polar covalent bond: covalent bond, polar covalent bond, ionic bond
Final Answer
The correct answer is: covalent bond, polar covalent bond, ionic bond.
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