Question

draw the lewis structure of the following molecule. use it to give the information

c₄h₁₀

number of single bonds

number of double bonds

number of sigma bonds

number of pi bonds

number of unshared electrons

Explanation:

Step1: Determine the structure of \(C_4H_{10}\)

\(C_4H_{10}\) is butane. Its Lewis structure has a chain of four carbon atoms. Each carbon atom forms four bonds. The structure is \(H - C - C - C - C - H\), with hydrogens attached to complete the four - bond requirement for each carbon.

Step2: Count single bonds

In the \(C_4H_{10}\) structure, there are 3 \(C - C\) single bonds and 10 \(C - H\) single bonds. So the total number of single bonds is \(3 + 10=13\).

Step3: Count double bonds

Since \(C_4H_{10}\) is an alkane (saturated hydrocarbon), there are 0 double bonds.

Step4: Count sigma bonds

All single bonds are sigma bonds. So the number of sigma bonds is 13 (same as the number of single bonds).

Step5: Count pi bonds

Pi bonds are present in double or triple bonds. Since there are no double or triple bonds in \(C_4H_{10}\), the number of pi bonds is 0.

Step6: Count unshared electrons

Carbon has 4 valence electrons and hydrogen has 1 valence electron. In \(C_4H_{10}\), all valence electrons are used in bonding. Each \(C - C\) bond uses 2 electrons and each \(C - H\) bond uses 2 electrons. The total number of valence electrons is \(4\times4 + 1\times10=26\). The number of bonding electrons is \(13\times2 = 26\). So the number of unshared electrons is 0.

Answer:

Number of single bonds: 13
Number of double bonds: 0
Number of sigma bonds: 13
Number of pi bonds: 0
Number of unshared electrons: 0