A Small Taste Of Quantum Chemistry

in science •  3 years ago  (edited)

Ever since the discovery of quantum mechanics, it seems the structure of the world around us is anything but intuitive.
Let’s take a gander at our intuitive understanding of ‘solids’ for example, let’s say a rock.
A rock is probably as solid of an object as most of us can imagine.
We perceive it as a continuous structure of uninterrupted matter, extremely dense and rigid.
But is it?

Solid materials are actually constructed out of peculiar elements called atoms, and even more peculiar elements called electrons.
One famous early notion which has since been superseded, was proposed by famous scientist Niels Bohr.
The Bohr model suggested that electrons orbit around atoms, in 'ordained' motion, much like planets around a star.

Bohr Model


What quantum mechanics has to teach us, is When we talk about electrons surrounding an atom, we actually talk about a ‘cloud of probabilities’.
Probabilities of what? Probabilities of where the electron is at any given moment. That’s right.
The electrons aren’t actually there, they are only probably there.
Take a look at the following diagram of 'probability densities' - the changes in color indicate how probable it would be for an electron to occupy a certain position around the atom.

Quantum Weirdness

Not only that solid matter is not as rigid we perceive it to be, it is actually built (if you will) by clouds of probabilities surrounding minuscule entities.
These ‘clouds’ come in many crazy shapes, and are named atomic orbitals.
The geometric shapes of atomic orbitals are calculated using what is called ‘quantum numbers’ which stem from advanced mathematics, and have visual representations.

You can use this great tool to further explore atomic orbitals

So far we have discussed a single atom with a cloud of probabilities surrounding it, but we all know that matter is constructed out of a huge amounts of these elementary particles, so what would that look like in the quantum world? Even weirder.
It seems that when atoms band together to create molecules, their ‘clouds’ combine and interact to form completely new probability fields called molecular orbitals (no surprise there).
What if we were to compare the size of an atom to the size of an electron.
Intuitively and by the classical model, the atom is bigger than the electron by orders of magnitude, but when we look at electrons as a field of probabilities, what would ‘bigger’ even mean?

Go deeper down the rabbit hole:

Quantum physics: What is really real?
Introduction to quantum mechanics

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Quantum chemistry is fascinating.
I remember after working through the solution to the Schrödinger equation for the hydrogen atom that I found it so beautiful, so elegant and precise! Furthermore it provides a systematic understanding of the properties of the different elements, and why they're grouped the way they are in the periodic table.


Keep writing. I want to read more!

Much obliged

cool i love it keep up the good work thank you..