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Chapter 5: Problem 22

Describe the shape of each of the following orbitals: a. \(3 p\) b. \(6 s\) c. \(4 p\)

Short Answer

Expert verified
3p and 4p orbitals have a dumbbell shape; 6s orbital has a spherical shape.

Step by step solution

01

Understand the Shape of the 3p Orbital

p orbitals have a dumbbell shape. The 3p orbital is just a higher energy level version of the p orbital and maintains the same dumbbell shape, but it is larger in size compared to the 2p orbital.
02

Understand the Shape of the 6s Orbital

s orbitals have a spherical shape. The 6s orbital is at a much higher energy level and is significantly larger than the 1s, 2s, and lower s orbitals, but it retains the spherical shape.
03

Understand the Shape of the 4p Orbital

Similar to the 3p orbital, the 4p orbital also has a dumbbell shape. It is larger in size than the 3p orbital because it is at a higher energy level.

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Key Concepts

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

3p orbital shape
The 3p orbital belongs to the p orbital family which has a distinctive dumbbell shape. This shape arises due to the angular momentum of electrons and their wave-like properties. The 3p orbital is situated at the third energy level and is larger compared to the 2p orbital. The nodes, or regions where there is zero probability of finding an electron, increase as the energy level increases. So, the 3p orbital has more complex nodal structures compared to 2p, making it essential to visualize this in three dimensions. Understanding the dumbbell shape of the p orbital helps in grasping how electrons are distributed in atoms and how these shapes influence molecular geometry.
6s orbital shape
s orbitals are characterized by their spherical shape, indicating that the probability of finding an electron at a certain distance from the nucleus is the same in all directions. The 6s orbital is especially interesting because it is located at the sixth energy level, meaning it is significantly larger and more diffuse than lower energy s orbitals like 1s or 2s. Despite its large size, it maintains the spherical symmetry. Because of the higher energy level, 6s orbitals also have more nodes, appearing as concentric spherical shells where the probability density drops to zero.
4p orbital shape
Much like its counterparts, the 4p orbital maintains a dumbbell shape. This orbital is at the fourth energy level, indicating a larger size and more nodal planes compared to the 3p orbital. The size and shape of the 4p orbital are crucial for understanding chemical bonding and molecular structure, as p orbitals often form pi bonds during overlapping. The visualization of the 4p orbital's increased complexity helps in understanding electron spatial distributions and their influence on the chemical properties of molecules.

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Most popular questions from this chapter

Select the element with higher ionization energy in each pair. (5.6) a. Cs or Ba b. \(\mathrm{Cl}\) or \(\mathrm{At}\) c. Si or \(\mathrm{P}\) d. Be or Ca

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. \([\mathrm{Ne}] 3 s^{2} 3 p^{1}\)

a. How many \(3 d\) electrons are in Fe? (5.4) b. How many \(5 p\) electrons are in Ba? c. How many \(4 d\) electrons are in I? d. How many \(7 s\) electrons are in Ra?

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

Indicate the maximum number of electrons in the following: a. \(2 p\) orbital b. \(3 p\) sublevel c. \(n=4\) energy level d. \(5 d\) sublevel
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