a. What is the bond order of the boron–oxygen bonds in the borate ion, BO $_{3} ^{3−}$ ?
b. Which molecule has the shortest carbon–carbon bond: $C_{2}H_{4}, C_2H_2,\text{ or } C_{2}H_{6}$ ?
c. Which molecule has the weakest carbon–carbon bond: $C_{2}H_{4}, C_{2}H_{2}$ , or $C_{2}H_{6}$ ?

Question

a. What is the bond order of the boron–oxygen bonds in the borate ion, BO[latex]_{3} ^{3−}[/latex]?
b. Which molecule has the shortest carbon–carbon bond: [latex]C_{2}H_{4}, C_2H_2, ext{ or } C_{2}H_{6}[/latex]?
c. Which molecule has the weakest carbon–carbon bond: [latex]C_{2}H_{4}, C_{2}H_{2}[/latex], or [latex]C_{2}H_{6}[/latex]?

Accepted Answer

You are asked to identify the bond order in a molecule or ion and to use bond order to make predictions about relative bond length or bond energy in a series of molecules or ions.
You are given the chemical formula of a molecule or ion, or a series of molecules or ions.
a. The Lewis structure for the borate ion shows three boron–oxygen single bonds. Each B—O bond has a bond order of 1.

[latex]\left[\begin{matrix} \,\,\,\, :\overset{..}{\underset{|}{O}}: \ \,\,\,\overset{..}{:\underset{..}{O}}- B- \overset{..}{\underset{..}{O}:} \end{matrix} ight] ^{3-}[/latex]

b. Bond length decreases with increasing bond order. C[latex]_{2}[/latex]H[latex]_{2}[/latex] has the highest carbon–carbon bond order and the shortest carbon–carbon bond.

[latex]\begin{matrix}&\begin{matrix} \underset{|}{H} \quad \underset{|}{H}\H- \underset{|}{C} - \underset{|}{C} - H\H\quad \, H \end{matrix}& \begin{matrix} H\qquad \qquad \quad H\\overset{\diagdown \qquad \qquad \diagup }{\underset{\diagup \qquad \qquad\diagdown }{C=C}}\H\qquad \qquad \quad H\end{matrix}& \begin{matrix}H-C\equiv C-H \end{matrix}\ ext{CC bond order:}&1&2&3 \end{matrix}[/latex]

c. Bond energy decreases with decreasing bond order. C[latex]_{2}[/latex]H[latex]_{6}[/latex] has the lowest carbon–carbon bond order and the weakest carbon–carbon bond.

Question 8.3.1: a. What is the bond order of the boron–oxygen bonds in the b......

Related Answered Questions

Determine polarity of molecules. Determine whether each of the following is polar. a. SO3 b. BrF3 ...

Verified Answer:

Identify molecular geometry. Identify molecular geometry Determine the shape of a. ICl5 b. SO3^2− ...

Verified Answer:

Identify electron-pair geometry. Determine the electron-pair geometry of a. the carbon atoms in acetic acid, CH3CO2H b. SF4 ...

Verified Answer:

Calculate enthalpy of reaction using bond energies. Calculate the enthalpy change for the following gas-phase reaction. C2H6(g) + Cl2(g) → C2H5Cl(g) + HCl(g) ...

Verified Answer:

Use the formal charge for each atom in the cyanide ion, CN^−, to predict whether H^+ is more likely to attach to carbon or nitrogen when forming hydrocyanic acid. ...

Verified Answer:

Three nonequivalent resonance structures for the chlorate ion are shown here. Assign formal charges to all atoms in the resonance structures and identify the more likely resonance structure. ...

Verified Answer:

a. What is the bond order of the nitrogen–oxygen bonds in the nitrate (NO3^−) ion? b. In which ion (NO2^− or NO3^−) are the nitrogen–oxygen bonds longer? c. In which ion (NO2^− or NO3^−) are the nitrogen–oxygen bonds stronger? ...

Verified Answer:

a. Which of the following bonds are nonpolar? C — Cl H — Cl H — H F — F P — H S — O B — F b. Which of the following bonds is most polar? C — Cl H — Cl H — H F — F P — H S — O B — F ...

Verified Answer:

Draw the Lewis structure for a. SCl2 b. CN^− ...

Verified Answer:

Draw all resonance structures for the carbonate ion, CO3^2−. ...

Verified Answer: