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Ionic Character Comparison: Analyzing NaBr vs. HBr and BrCl vs. FCl
Chapter 1, Problem 1.37(choose chapter or problem)
For each pair of compounds below, identify the one that would be expected to have more ionic character. Explain your choice.
(a) NaBr or HBr
(b) BrCl or FCl
Questions & Answers
QUESTION:
For each pair of compounds below, identify the one that would be expected to have more ionic character. Explain your choice.
(a) NaBr or HBr
(b) BrCl or FCl
ANSWER:Step 1 of 2
a) For compound NaBr
The electronegativity of sodium - 0.9
The electronegativity of bromine - 2.8
The electronegativity difference of NaBr compound is 1.9
For compound BBr
The electronegativity of hydrogen - 2.2
The electronegativity of bromine - 2.8
The electronegativity difference of HBr compounds is 0.6.
Therefore, NaBr has more ionic character than Hbr because sodium bromide has a high electronegativity difference than hydrogen bromide.
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Ionic Character Comparison: Analyzing NaBr vs. HBr and BrCl vs. FCl
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Discover the analysis of ionic character in compounds based on electronegativity differences. Learn about the contrasts between NaBr vs. HBr and BrCl vs. FCl. Grasp why NaBr and FCl showcase greater ionic character than their paired compounds.