The essential particles that construct all materials are electrons, neutrons and protons. Protons and neutrons form the atomic nucleus – electrons fill the atomic orbits, compensating the positive nucleus charge. Atoms are connected to each other with different kinds of bonds, depending on the atoms nature, covalent bond, ionic bond and others.
A Hydrogen atom consists of a proton and electron. By the simple model of an atom, an electron is orbiting around the atomic nucleus. Quantum mechanics state that electron movement is described by the wave function, spherically symmetrical in the isolated hydrogen atom. So the electron charge is diffusely distributed, forming a cloud.
Possible orbits for electrons in the atoms are those where the length of orbit is the whole electron wavelength:
From here we can get the orbit radiuses and energy levels corresponding to them:
According to the law of minimum potential energy of the system, an electron goes to the minimum energy state with a bounce or by successive transitions. When an electron moves between energy levels, it releases the quantity of energy, corresponding the energy difference of the levels.
Remote atoms have a discrete bar-shaped structure of energy levels (they are characterised by exact lines). Discrete structure of the energy spectrum can be proved by a variety experiments.
Atoms are around 1 or a couple of Angstrems in size. When atoms come together at a distance of around a couple of Angtrems, interaction forces work between them. The interaction forces can be forces of conversion or repulsion depending on the electrons’ motion of adjacent atoms. Atoms can connect, releasing energy, forming a stable chemical compound. Electrons of the inner atom orbits, which are full with electrons, are tightly bounded to the nucleus, and do not participate at a chemical bonding formation. Chemical features of the atoms are determined by the outer orbit, and are not totally filled in with electrons. The outer orbit electrons are called valence electrons.
With this bonding, atoms join into a molecule by sharing the electrons of their outer orbits. The density of a negatively charged cloud is the biggest between a positively charged nucleus. Electron clouds overlapping in atoms leads to sharing electrons, but follows with redistribution of electron density and a change in a system’s energy. During sharing electrons, electron clouds are involved in the space between a nucleus. Such a state with increased density of electron charge between a nucleus leads to the appearance of forces of attraction.
The basis of covalent force is an exchanging interaction, the exchange of electrons by atoms, and having quantum nature. These forces are exchanging forces, and energy is exchanging energy. The main feature of exchanging forces is the fact that they depend on the electron spins, which make connections between atoms. Covalent bonds are specifically directed and appear only between adjacent atoms.
Molecules with covalent bonds can be polar (bipolar) or non-polar, in accordance to their symmetrical or asymmetrical structure. Molecules with matching centres of positive and negative charges are non-polar. Molecules with non-matching centres are polar (or bipolar). Bipolar molecules are characterised by bipolar momentum p:
p = ql, where q is a charge, l is a distance between molecules. Covalent bond is typical for organic and non-organic compounds. Covalent bond is a high strength bond.
The ionic crystal ions with opposite signs are alternates in the crystal lattice sites. Atom electronegativity is an atom’s ability to catch electrons to form chemical bonds. Atom electronegativity is considered half the sum of its ionisation energy and its electron affinity Ea.
The alkali metals have the smallest electronegativity, they easily leave the electron and have small affinity energy. The biggest affinity energy has halogen atoms, they easily accept electrons on their valence levels.