Question 1

How does bond order affect bond length?

Accepted Answer

For the same atom pair, increasing bond order generally shortens the bond. For example, C-C is about 154 pm, C=C is about 134 pm, and C≡C is about 120 pm. These are approximate values because bond length also depends on the molecular environment.

Question 2

Why is a triple bond stronger than a double bond?

Accepted Answer

A single bond contains one sigma bond, a double bond adds one pi bond, and a triple bond adds two pi bonds. For the same atoms, these additional bonding components hold the nuclei closer and increase the average bond enthalpy.

Question 3

How is bond order calculated for a homonuclear diatomic molecule?

Accepted Answer

Bond order is one-half of the difference between bonding and antibonding electron counts: BO = 1/2(Nb - Na). This gives H2 bond order 1, O2 bond order 2, and N2 bond order 3.

Question 4

What does a bond-enthalpy value represent?

Accepted Answer

Bond enthalpy is the enthalpy change required to break one mole of a stated bond in the gaseous state. The values used in this lab are average bond enthalpies, so they are not universal constants for every molecule containing that bond.

Question 5

What is shown by the potential-energy curve of a bond?

Accepted Answer

The horizontal axis is internuclear distance and the vertical axis is potential energy. The minimum of the curve gives the equilibrium bond length, while the energy difference between the minimum and separated atoms represents the bond energy.

Bond Length & Energy Lab — Bond Order ko Feel Karo

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