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Chapter 5: Problem 21

Describe the shape of each of the following orbitals: a. \(1 s\) b. \(2 p\) c. \(5 s\)

Short Answer

Expert verified
The 1s orbital is spherical, the 2p orbitals are dumbbell-shaped with one nodal plane, and the 5s orbital is spherical with four nodes.

Step by step solution

01

Understanding the 1s Orbital

The 1s orbital is the simplest and smallest atomic orbital. It is spherical in shape and surrounds the nucleus symmetrically. There are no nodes in the 1s orbital, meaning the probability density is highest at the nucleus and decreases uniformly outward.
02

Understanding the 2p Orbital

The 2p orbitals are the first set of p orbitals and there are three of them: 2p_x, 2p_y, and 2p_z. Each 2p orbital is dumbbell-shaped and oriented along one of the three axes (x, y, or z). These orbitals have a single nodal plane that passes through the nucleus, splitting the orbital into two lobes.
03

Understanding the 5s Orbital

The 5s orbital is spherical, like the 1s orbital, but it is larger and has more complexity. The 5s orbital has four nodes. This means that within this spherical shape, there are regions where the probability of finding an electron is zero.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

1s Orbital Shape
The 1s orbital is the simplest atomic orbital. It is perfectly spherical and symmetrical around the nucleus. This spherical shape means that the electron density is evenly spread out in all directions from the nucleus.
In the 1s orbital, there are no nodes, which are areas where the probability of finding an electron is zero.
So, the highest electron density is at the nucleus, and it gradually decreases as you move away from it.
This makes the 1s orbital easy to visualize as a solid, uniform sphere of electron cloud around the nucleus.
2p Orbital Shape
The 2p orbitals are more complex than the 1s orbital. They come in three varieties: 2p_x, 2p_y, and 2p_z. Each of these orbitals is shaped like a dumbbell and is oriented along one of the three axes (x, y, or z).
One important feature of 2p orbitals is they have a nodal plane that runs through the nucleus, splitting the orbital into two lobes.
In other words, this plane is an area where there is zero probability of finding an electron.
The electrons are most likely to be found in the two lobes on either side of the nodal plane. This unique shape is crucial for understanding molecular bonding and electron distribution in atoms.
5s Orbital Shape
The 5s orbital echoes the spherical symmetry of the 1s orbital but is much larger and more complex.
It still maintains its spherical shape but with a significant addition: it has four nodes. These nodes are spherical shells where the probability of finding an electron is zero.
As a result, the electron density in the 5s orbital varies more dramatically, with regions of high and low electron density.
This complexity allows for more diverse electron arrangements compared to the simpler 1s orbital.
Understanding the 5s orbital helps in predicting the behavior of electrons in more complex atoms.

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Most popular questions from this chapter

Place the following types of electromagnetic radiation in order of increasing frequencies: TV signal, X-rays, and microwaves.

Give the symbol of the element with each of the following electron or abbreviated electron configurations: a. \(1 s^{2} 2 s^{2} 2 p^{4}\) b. \([\mathrm{Ne}] 3 s^{2}\) c. \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\) d. \([\mathrm{Ne}] 3 s^{2} 3 p^{1}\)

Select the element in each pair with the higher ionization energy. a. \(\mathrm{O}\) or \(\mathrm{Ne}\) b. \(\mathrm{K}\) or \(\mathrm{Br}\) c. \(\mathrm{Ca}\) or \(\mathrm{Ba}\) d. \(\mathrm{N}\) or \(\mathrm{Ne}\)

Give the symbol of the element that meets the following conditions: a. has five electrons in the \(3 p\) sublevel b. has four \(2 p\) electrons c. completes the \(3 s\) sublevel d. has one electron in the \(3 s\) sublevel

Use the periodic table to give the symbol of the element with each of the following electron configurations: a. \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}\) b. \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{7}\) c. \([\mathrm{Ar}] 4 s^{2} 3 d^{10}\) d. \([\mathrm{Xe}] 6 s^{2} 4 f^{14} 5 d^{10} 6 p^{3}\)
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