Textbook Question
Write the Lewis structure for each molecule. d. CH3SH (C and S central)
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Ch.9 - Chemical Bonding I: The Lewis Model
Chapter 9, Problem 56
Determine whether the bond between each of the following pairs of atoms would be pure covalent, polar covalent, or ionic: a. C and N b. N and S c. K and F d. N and N.
Verified step by step guidance1
<Determine the electronegativity of each atom in the pair.>
<Calculate the difference in electronegativity between the two atoms.>
<Use the difference to classify the bond: pure covalent (0), polar covalent (0 < difference < 2), or ionic (difference >= 2).>
<Apply this method to each pair: a. C and N, b. N and S, c. K and F, d. N and N.>
<Summarize the bond type for each pair based on the calculated differences.>
Related Practice
Textbook Question
Write the Lewis structure for each molecule. a. CH2O b. C2Cl4 c. CH3NH2 d. CFCl3 (C central)
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Textbook Question
Determine if a bond between each pair of atoms would be pure covalent, polar covalent, or ionic. a. Br and Br
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Textbook Question
Refer to Figure 9.10 to estimate the percent ionic character of the CO bond.
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Textbook Question
Draw the Lewis structure for BrF with an arrow representing the dipole moment. Refer to Figure 9.10 to estimate the percent ionic character of the BrF bond.
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Textbook Question
Refer to Figure 9.10 to estimate the percent ionic character of the BrF bond.
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