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Chapter 1: Problem 5

Using the symbols \(\delta-\) and \(\delta+\), indicate the direction of polarity in each polar covalent bond. (a) \(\mathrm{C}-\mathrm{N}\) (b) \(\mathrm{N}-\mathrm{O}\) (c) \(\mathrm{C}-\mathrm{Cl}\)

Short Answer

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Question: Determine the direction of polarity for the following polar covalent bonds using the symbols \(\delta-\) and \(\delta+\): (a) C-N, (b) N-O, (c) C-Cl. Answer: (a) C(\(\delta+\)) - N(\(\delta-\)), (b) N(\(\delta+\)) - O(\(\delta-\)), (c) C(\(\delta+\)) - Cl(\(\delta-\)).

Step by step solution

01

Determine electronegativity values of the atoms involved in each bond

Using a periodic table or an electronegativity table, look up the electronegativity values of the following elements: C, N, O, and Cl.
02

Compare electronegativity values for each bond

For each given bond (C-N, N-O, and C-Cl), compare the electronegativity values of the atoms involved. The atom with higher electronegativity will have the partial negative charge (\(\delta-\)), while the atom with lower electronegativity will have the partial positive charge (\(\delta+\)).
03

Indicate the direction of polarity in each bond

(a) For the C-N bond, since the electronegativity of N is greater than that of C, the bond polarity will be C(\(\delta+\)) - N(\(\delta-\)). (b) For the N-O bond, since the electronegativity of O is greater than that of N, the bond polarity will be N(\(\delta+\)) - O(\(\delta-\)). (c) For the C-Cl bond, since the electronegativity of Cl is greater than that of C, the bond polarity will be C(\(\delta+\)) - Cl(\(\delta-\)).

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Most popular questions from this chapter

Use VSEPR to predict the geometry of these ions. (a) \(\mathrm{NH}_{2}{ }^{-}\) (b) \(\mathrm{NO}_{2}{ }^{-}\) (c) \(\mathrm{NO}_{2}^{+}\) (d) \(\mathrm{NO}_{3}^{-}\)

(a) Draw a Lewis structure for the ozone molecule, \(\mathrm{O}_{3}\). (The order of atom attachment is \(\mathrm{O}-\mathrm{O}-\mathrm{O}\), and they do not form a ring.) Chemists use ozone to cleave carboncarbon double bonds (Section 6.5C). (b) Draw four contributing resonance structures; include formal charges. (c) How does the resonance model account for the fact that the length of each \(\mathrm{O}-\mathrm{O}\) bond in ozone \((128 \mathrm{pm})\) is shorter than the \(\mathrm{O}-\mathrm{O}\) single bond in hydrogen peroxide (HOOH, \(147 \mathrm{pm}\) ) but longer than the \(\mathrm{O}-\mathrm{O}\) double bond in the oxygen molecule \((123 \mathrm{pm})\) ?

Draw structural formulas for the three secondary amines with the molecular formula \(\mathrm{C}_{4} \mathrm{H}_{11} \mathrm{~N}\).

Show how each chemical change leads to a stable octet. (a) Sulfur forms \(\mathrm{S}^{2-}\). (b) Magnesium forms \(\mathrm{Mg}^{2+}\).

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