3.8:
Electron Behavior
Electrons are tiny, negatively charged particles that exist in an electron cloud around a positively charged nucleus. Within the cloud, electrons reside in distinct areas called shells or energy levels.
The energy levels are often visualized using the simplified Bohr or planetary model, where they are represented as rings around the nucleus, though they actually have complex shapes.
The electrons in these shells have increasing energy as they move further away from the nucleus.
In the first energy level, there can be a maximum of two electrons. The second shell can hold a maximum of eight electrons. Additional electrons in an atom fill increasingly higher energy levels.
The electrons in the outermost occupied shell are called valence electrons, and they determine the chemical properties of an element.
Valence electrons may be shared between atoms to form covalent bonds or transferred to form ionic bonds.
3.8:
Electron Behavior
Electrons are negatively charged subatomic particles attracted to and orbit around the positively-charged nucleus of an atom. They reside in spaces associated with energy levels called shells and are further organized into subshells and orbitals within each shell.
Electrons Orbit the Nucleus
Electrons are found in specific locations outside of the nucleus. The shell in which an electron resides indicates the general energy level of the electron: those closer to the nucleus have less energy, while those further out have more energy. The subshell describes the location and energy level of the electron more precisely, and the orbital describes the shape of an area of probability in which an electron orbits the nucleus. The electrons, which are closest to the nucleus, have the least amount of energy, and as their distance from the nucleus increases, so does the amount of energy that the electron carries. Farther from the nucleus, there is more space for electrons to orbit so that the outer shells can hold more electrons than the inner shells. The outermost electrons of an atom reside in the valence shell and are referred to as valence electrons. These electrons can form ionic and covalent bonds with other atoms.
Discovering the Electron
In the late 1890s, J. J. Thomson performed a series of experiments using cathode ray tubes that would lead to the discovery of the electron-the first subatomic particle. A cathode ray tube is a glass tube with two electrodes connected to a power source supplying electricity. A vacuum removes most of the air from the interior of the tube. When the voltage is applied across the electrodes, a beam of particles travels from the negatively charged cathode to the positively charged electrode anode. The anode has a small hole so that the rays can pass through. A phosphorus coating on the opposite end of the tube glows when the cathode rays strike it.
Thomson directed the cathode ray between two metal plates, one with a positive charge and one with a negative charge, and measured the ray's position at the far end of the tube. When the ray passed between the two plates, it was deflected away from the negatively charged plate, bending in the direction of the positively-charged plate. Since like charges repel, and opposite charges attract, this indicated that the particles in the cathode ray possessed a negative charge.
Further experiments to calculate the mass-to-charge ratio of the cathode particles revealed that the mass of each negatively-charged particle was about 1/2000 of the mass of any known atom. Because of this, Thomson concluded that there must be many electrons present in any given atom. Later, the discovery of protons and neutrons would explain an atom's distribution of mass and overall neutral charge.
This text is adapted from Openstax, Chemistry 2e, Section 6.3: Development of quantum theory.