Free energy is a term I use to describe the fact that matter isn’t free but made up of energy and matter. A single atom of matter has its density in atomic units (1 g) times the total amount of the energy it contains. One atomic of each element that we know of has a density in atomic units of 6.23. That means, when an electron hits an atom, that atom loses 5.23 of its energy. The remaining energy is carried by the electrons to the atoms outermost atom (and then through those atoms until we reach the center). In order to know the energy of a nucleus, all we have to do is figure out how much energy it will carry at each energy level, which is known as the “energy content.”
So, what exactly is a nucleus?
A nucleus is a very stable and relatively large, highly charged, highly radioactive atom. It contains 1 to 3 protons and 2 to 6 neutrons. Most nuclei contain only 1 or 2 protons, so there is an important limitation to how far you can go in understanding a nucleus. It’s also important to see that a nucleus only weighs about 20 times as much as a star or its fuel. A single atomic would weigh only 6,000 kg to its core, so you can’t make atomic weights a very meaningful way to say “mass and density.” A nucleus only has one number of protons and one number of neutrons, so the mass, or volume, doesn’t matter as much.
What is mass, energy, and charge?
So, how do we go any further with discussing mass, energy, and charge? Let’s think about these things with an understanding of the chemical bonding, or the interatomic and interatomic bonds and how the energy of the elements interacts inside the nucleus.
Chemistry uses molecules, atoms and electrons (the positively charged particles of the chemical bond). The protons (protons are the main atoms from the chemical table above which are the building blocks of the nucleus of a nucleus) are in a strong chemical bond, and are arranged in such a way that they form a hydrogen atom of the nucleus. The atoms in a nucleus also have specific charges (called the valence electrons), but they are not the same as the chemical bond.
These bonds are not strictly the same as a chemical bond. As an example, the valence electrons around an atom have opposite signs, the hydrogen charges being positive and the electrons being negative.
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