Understanding the arrangement of electrons in atoms might seem simple, but the reality is quite complex. Many believe electrons move around the nucleus, but they actually remain in fixed positions. In today’s article, we’ll explore how electrons are situated within atoms.
Various atomic models, such as Rutherford’s and Bohr’s, have been introduced to explain the structure of atoms. However, none of these models provided a fully accurate depiction. Irwin Suringer’s model offers a more comprehensive explanation of electron orbits in atoms.
According to Suringer’s model, electrons, neutrons, and protons should be viewed as waves. While it may be challenging to conceive everyday objects as waves, according to this theory, even the mobile device in your hand can be considered a wave.
Let’s consider the example of a hydrogen atom, which contains one electron. This electron will remain at the S level, and the S orbital has a spherical shape. Consequently, the electron will be located in the S orbital.
For helium, which has two electrons, both will occupy the S orbital. Each orbital can accommodate two electrons. As we move to lithium with three electrons, the first two will be in the 1S orbital, and the third electron will be in the 2S orbital.
As we progress to boron, with five electrons, three orbitals are required, as each orbital can only hold a maximum of two electrons. Carbon, with six electrons, will have the last two electrons in the PX and PY orbitals.
As the number of electrons increases, the number of orbitals also increases. For instance, there are three types of p orbitals, and each can hold two electrons, totaling six electrons. Similarly, there are five different shapes of d orbitals and seven different shapes of f orbitals, each capable of holding two electrons.
Electrons in atoms have the ability to move between orbits, transitioning to higher or lower levels. However, this requires a significant force to be applied. It’s important to note that protons, being much smaller in size, do not require any orbitals.
