Electronic Structure: Study with Video Lessons, Practice Problems & Examples

The electronic structure of an atom consists of shells, subshells, and orbitals. The shell indicates the size and energy, while subshells (s, p, d, f) define the shape of orbitals. Within these orbitals, electrons can be located, each exhibiting a spin that can be either clockwise or counterclockwise. Understanding this structure is crucial for locating specific electrons and analyzing their behavior, which is fundamental in fields like chemistry and physics.

Electronic Structure Concept 1

When we discuss the atom, we can take a look at its electronic structure. We're going to say the modern description of the electronic structure of an atom is based on the following principles. First, we have the shell. The shell is the orbit that the electrons take as they travel around the nucleus. Once we go past the shell, we go to our next level within it, the subshell or sublevel. This is the region where a group of electrons in an atom are located within the same shell. Now what's important here is that the subshells use certain variables. These variables are the letters s, p, d, and f. Finally, we have our orbit itself. This orbital itself, this is the region within a subshell where specific electrons can be found. So basically, as we go from shell to subshell to orbital, we're looking more and more into the atom to find the exact location of a particular electron. Now that we've gone over the basic structure of an atom in terms of these three terms, let's click on the next video and look at an actual atom.

Electronic Structure Concept 2

The goal of revealing the electronic structure of an atom is to help us locate a particular electron. Now, when we take a look at the atom, we're going to say that the black circle that shows the atom represents our shell. The shell gives us the size and energy involved. Once we go past the shell, we're going to go past the shell, to this blue part here. This blue part here represents our subshell. The subshell gives us the shape of an orbital within a subshell. Okay? So it gives us the shape. Once we go past that, we go into the red portion. This red portion represents our orbital. The orbital itself gives us the orientation of electrons in these in a set of orbitals. And then finally, when we go past that, we go to this green. We know that is an electron, and electrons within an orbital can spin either clockwise or counterclockwise. When we get to the electron, we can examine the spin the electron takes. So when we're talking about electronic structure, the breakdown is we're looking at the atom. The atom, we go past it and we look at its shells. From its shells, we can look at its subshells. Beyond the subshells, we look at its orbitals. And within the orbitals is where we find our particular electron. And we can look at how the electron spins either clockwise or counterclockwise. So this is the whole basic idea of electronic structure. We're examining an atom in hopes of finding an electron and examining how it spins either clockwise or counterclockwise within a particular orbital.

Electronic Structure Example 1

If the path of an electron within an orbital can be seen as an ellipse, what best describes this image? An ellipse, if you didn't know, somewhat resembles the figure 8. You can draw it vertically or horizontally. And when we're talking about ellipses, it is indeed a shape. Now, which one of the terms do we use to discuss the shape of an orbital? We know that size and energy are based on the shell. Energy level is synonymous with energy level, which is the same as shell. Here, "electron" wouldn't be accurate. The answer has to be "subshell". The subshell talks about the shape of a given orbital, and here ellipses will be one of those shapes.

Which term can best describe the electron shown in the following image?

• A. Shell
• B. Subshell
• C. Sublevel
• D. Electron

Here’s what students ask on this topic:

What is the electronic structure of an atom?

The electronic structure of an atom describes the arrangement of electrons around the nucleus. It consists of shells, subshells, and orbitals. Shells indicate the size and energy level of the electrons. Subshells, labeled as s, p, d, and f, define the shape of the orbitals within a shell. Orbitals are regions within subshells where specific electrons can be found. Each electron in an orbital has a spin, which can be either clockwise or counterclockwise. Understanding this structure helps locate specific electrons and analyze their behavior, which is fundamental in chemistry and physics.

What are the differences between shells, subshells, and orbitals in an atom?

Shells, subshells, and orbitals are different levels of organization for electrons in an atom. Shells are the broadest level, indicating the size and energy of the electrons. Subshells are within shells and are labeled as s, p, d, and f, defining the shape of the orbitals. Orbitals are the most specific regions within subshells where electrons are likely to be found. Each orbital can hold a maximum of two electrons with opposite spins. This hierarchical structure helps in locating and understanding the behavior of electrons in an atom.

How do subshells differ in terms of shape and energy?

Subshells differ in both shape and energy. The s subshell is spherical, the p subshell is dumbbell-shaped, the d subshell has a more complex clover shape, and the f subshell is even more complex. In terms of energy, within a given shell, the energy increases from s to f. For example, in the second shell, the 2s subshell has lower energy than the 2p subshell. These differences in shape and energy are crucial for understanding how electrons are distributed in an atom and how they interact in chemical reactions.

What is the significance of electron spin in an orbital?

Electron spin is a fundamental property of electrons within an orbital. Each orbital can hold a maximum of two electrons, and these electrons must have opposite spins, one clockwise and one counterclockwise. This is due to the Pauli Exclusion Principle, which states that no two electrons in an atom can have the same set of quantum numbers. The spin of electrons affects their magnetic properties and plays a crucial role in the formation of chemical bonds and the behavior of atoms in magnetic fields.

How do you determine the electron configuration of an atom?

To determine the electron configuration of an atom, follow the Aufbau principle, which states that electrons fill orbitals starting from the lowest energy level to the highest. Use the order of filling: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p. Apply Hund's rule, which states that electrons will fill degenerate orbitals singly before pairing up. Also, consider the Pauli Exclusion Principle, ensuring no two electrons in the same orbital have the same spin. This method helps in predicting the arrangement of electrons in an atom.