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Chapter 7: Q73E (page 400)

Question: Complete the following Lewis structure by adding bonds (not atoms), and then indicate the longest bond:

Short Answer

Expert verified

The Lewis Structure with longest \({\rm{C - C}}\) bond is as follows 鈥�

Step by step solution

01

Concept Introduction

Chemical bonding is the creation of a chemical compound by forming a chemical link between two or more atoms, molecules, or ions. The atoms in the resultant molecule are held together by chemical bonds.

02

Adding the bonds

Observe the Lewis structure 鈥�

Add the single and double bonds wherever required 鈥�

Since single bond is longest as compared to double and triple, therefore \({\rm{C - C}}\) is the single bond which is the longest.

Therefore, \({\rm{C - C}}\) are the longest bonds.

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Most popular questions from this chapter

Which compound in each of the following pairs has the larger lattice energy? Note: \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\) and \({\rm{L}}{{\rm{i}}^{\rm{ + }}}\) have similar radii; \({{\rm{O}}^{{\rm{2 - }}}}\) and \({{\rm{F}}^{\rm{ - }}}\) have similar radii. Explain your choices.

(a) \({\rm{MgO}}\) or \({\rm{MgSe}}\)

(b) \({\rm{LiF}}\) or \({\rm{MgO}}\)

(c) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{O}}\) or \({\rm{LiCl}}\)

(d) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{Se}}\) or \({\rm{MgO}}\)

Question: Calculate the formal charge of each element in the following compounds and ions:

(a) \({{\rm{F}}_{\rm{2}}}{\rm{CO}}\)

(b) \({\rm{N}}{{\rm{O}}^{\rm{ - }}}\)

(c) \({\rm{BF}}_{\rm{4}}^{\rm{ - }}\)

(d) \({\rm{SnCl}}_{\rm{3}}^{\rm{ - }}\)

(e) \({{\rm{H}}_{\rm{2}}}{\rm{CC}}{{\rm{H}}_{\rm{2}}}\)

(f) \({\rm{Cl}}{{\rm{F}}_{\rm{3}}}\)

(g) \({\rm{Se}}{{\rm{F}}_{\rm{6}}}\)

(h) \({\rm{PO}}_{\rm{4}}^{{\rm{3 - }}}\)

Which compound in each of the following pairs has the larger lattice energy? Note: \({\rm{B}}{{\rm{a}}^{{\rm{2 + }}}}\) and \({{\rm{K}}^{\rm{ + }}}\) have similar radii; \({{\rm{S}}^{{\rm{2 - }}}}\) and \({\rm{C}}{{\rm{l}}^{\rm{ - }}}\) have similar radii. Explain your choices.

(a) \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) or \({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{O}}\)

(b) \({{\rm{K}}_{\rm{2}}}{\rm{S}}\) or \({\rm{BaS}}\)

(c) \({\rm{KCl}}\) or \({\rm{BaS}}\)

(d) \({\rm{BaS}}\) or \({\rm{BaC}}{{\rm{l}}_{\rm{2}}}\)

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the 鈥渞eal鈥� and 鈥渕odel鈥� modes. Explain the difference observed.

Draw the Lewis structures and predict the shape of each compound or ion:

(a) \({\rm{C}}{{\rm{O}}_{\rm{2}}}\)

(b) \({\rm{NO}}_{\rm{2}}^{\rm{ - }}\)

(c) \({\rm{S}}{{\rm{O}}_{\rm{3}}}\)

(d) \({\rm{S}}{{\rm{O}}_{\rm{3}}}^{{\rm{2 - }}}\)
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