Textbook Question
Determine if a bond between each pair of atoms would be pure covalent, polar covalent, or ionic. a. Ba and O
Ch.10 - Chemical Bonding I: The Lewis Model
Chapter 10, Problem 62b
Refer to Figure 10.10 to estimate the percent ionic character of the ClF bond.
Verified step by step guidance1
Identify the electronegativity difference between Cl and F. The electronegativity of Cl is approximately 3.0 and for F it is approximately 4.0.
Calculate the electronegativity difference: |4.0 - 3.0| = 1.0.
Locate the value of 1.0 on the x-axis (Electronegativity Difference) of the provided graph.
Find the corresponding point on the y-axis (Percent Ionic Character) that aligns with the electronegativity difference of 1.0.
Estimate the percent ionic character of the ClF bond by reading the y-axis value at the point where the electronegativity difference is 1.0.
Verified Solution
Video duration:
1m
This video solution was recommended by our tutors as helpful for the problem above.Was this helpful?
Related Practice
Textbook Question
Refer to Figure 10.10 to estimate the percent ionic character of the Hbr bond.
Textbook Question
Draw the Lewis structure for ClF with an arrow representing the dipole moment.
Textbook Question
Write the Lewis structure for each molecule or ion. b. OH-
649
views
Textbook Question
Write the Lewis structure for each molecule or ion. c. BrO-
520
views
Textbook Question
Write the Lewis structure for each molecule or ion. d. C2H4
795
views