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Chapter 22: Problem 53

Explain why two \(\mathrm{N}\) atoms can form a double bond or a triple bond, whereas two \(\mathrm{P}\) atoms normally can form only a single bond.

Short Answer

Expert verified
Two Nitrogen atoms can form either double or triple bonds due to their ability to share 2 or 3 valence electrons respectively since they are in the second energy level. Phosphorus atoms, being in the third energy level, are larger in size and even though they have the same number of valence electrons as Nitrogen, they normally form only single bonds because P-P-P bonding is less efficient due to the presence of more orbitals.

Step by step solution

01

Understanding Atomic Structure

The atomic structure consists of protons, neutrons and electrons. The thing to notice here is that the key element in bond is the presence of valence electrons. The number of valence electrons can determine the type of bonds an atom can form.
02

Comparing Nitrogen and Phosphorus

The Nitrogen atom (N) has 5 valence electrons in the second energy level which has a capacity for 8 electrons. Therefore, it needs 3 more electrons to obtain stable configuration. In the case of Phosphorus (P), it has 5 valence electrons but they are in third energy level. The third level can hold up to 8 electrons in the S and P orbitals and also has more orbitals in its d sub-levels that can accommodate more electrons.
03

Determine Bond Formation

A Nitrogen atom can share 3 of its valence electrons with another Nitrogen atom to form a triple bond. It can also share two for a double bond. However, in the case of Phosphorus, even though it has 5 valence electrons, due to its larger size and the presence of d orbitals, the P-P-P bonding is less efficient, which explains why two Phosphorus atoms normally form only a single bond.

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Most popular questions from this chapter

Metal chlorides can be prepared in a number of ways: (a) direct combination of metal and molecular chlorine, (b) reaction between metal and hydrochloric acid, (c) acid-base neutralization, (d) metal carbonate treated with hydrochloric acid, (e) precipitation reaction. Give an example for each type of preparation.

Compare the physical and chemical properties of the hydrides of each of the following elements: \(\mathrm{Na}\), \(\mathrm{Ca}, \mathrm{C}, \mathrm{N}, \mathrm{O}, \mathrm{Cl}\).

Sodium hydroxide is hygroscopic-that is, it absorbs moisture when exposed to the atmosphere. A student placed a pellet of \(\mathrm{NaOH}\) on a watch glass. A few days later, she noticed that the pellet was covered with a white solid. What is the identity of this solid? (Hint: Air contains \(\mathrm{CO}_{2}\).)

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Describe the bonding in the \(\mathrm{C}_{2}^{2-}\) ion in terms of the molecular orbital theory.
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