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Chapter 10: Problem 32

What overall shape do the \(2 p\) and \(3 p\) orbitals have? How do the \(2 p\) orbitals differ from the \(3 p\) orbitals? How are they similar?

Short Answer

Expert verified
The 2p and 3p orbitals both have a dumbbell-like shape with three possible orientations: px, py, and pz. They are similar in shape and orientation due to both being a result of l=1. However, they differ in that 3p orbitals are in a higher energy level (n=3) than 2p orbitals (n=2), resulting in the 3p orbitals being larger and more diffuse. Additionally, 3p orbitals have a node, which 2p orbitals do not.

Step by step solution

01

1. Understanding Orbitals

Orbitals are regions around the nucleus of an atom where electrons are most likely to be found. The shape of an orbital is determined by the combination of the principal quantum number 'n' (which defines the energy level) and the azimuthal quantum number 'l' (which defines the shape). In the case of 2p and 3p orbitals, the p orbitals correspond to l=1. The main difference between the 2p and 3p orbitals is the principal quantum number (n=2 for 2p and n=3 for 3p).
02

2. Shape of p Orbitals

The p orbitals have a dumbbell-like shape along the x, y, or z-axis. There are three possible orientations for p orbitals: px, py, and pz, oriented along the x, y, and z-axis respectively.
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3. Similarities between 2p and 3p Orbitals

The main similarities between the 2p and 3p orbitals are: 1. Both 2p and 3p orbitals have the same dumbbell-like shape. 2. Both have three possible orientations: px, py, and pz. 3. Both are a result of l=1 which corresponds to p orbitals.
04

4. Differences between 2p and 3p Orbitals

The main differences between the 2p and 3p orbitals are: 1. The 3p orbitals are in a higher energy level than the 2p orbitals, as the principal quantum number for 3p is n=3 while for 2p it is n=2. 2. The 3p orbitals are larger and more diffuse compared to the 2p orbitals, due to the higher energy level of 3p orbitals. 3. The 3p orbitals have a node, which 2p orbitals do not. Nodes are surfaces where the probability of finding an electron is zero.

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Most popular questions from this chapter

Why do the metallic elements of a given period (horizontal row) typically have much lower ionization energies than do the nonmetallic elements of the same period?

One bit of evidence that the present theory of atomic structure is "correct" lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit paramagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. On the basis of the electron orbital diagrams for the following elements, indicate which atoms would be expected to be paramagnetic, and tell how many unpaired electrons each atom contains. a. phosphorus, \(Z=15\) b. iodine, \(Z=53\) c. germanium, \(Z=32\)

When an atom in an excited state returns to its ground state, what happens to the excess energy of the atom?

The lowest possible energy state of an atom is called the ________ state.

Though all the elements in a given period (horizontal row) of the periodic table have their valence electrons in the same types of orbitals, the sizes of the atoms decrease from left to right within a period. Explain why.
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