Which of BeF2 or BF3 has a larger percentage ionic character, given the electronegativities of the elements below?F: 4.0Be: 1.6B: 2.0
Question
Which of BeF₂ or BF₃ has a larger percentage ionic character, given the electronegativities of the elements below?
- F: 4.0
- Be: 1.6
- B: 2.0
Solution
To determine the ionic character of a bond, we can use the difference in electronegativity between the two atoms involved. The greater the difference, the more ionic the bond is.
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Calculate the difference in electronegativity for BeF2: The electronegativity of Be is 1.6 and that of F is 4.0. So, the difference is 4.0 - 1.6 = 2.4.
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Calculate the difference in electronegativity for BF3: The electronegativity of B is 2.0 and that of F is 4.0. So, the difference is 4.0 - 2.0 = 2.0.
Comparing the two differences, BeF2 has a larger difference in electronegativity (2.4) than BF3 (2.0). Therefore, BeF2 has a larger percentage of ionic character than BF3.
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