Atoms

• Isotopes are atoms with different numbers of neutrons but the same number of protons, resulting in slightly different masses.
• Neutrons have no charge and are also located in the nucleus of atoms.
• Aufbau principle states that electrons fill available energy levels from lowest to highest energy.
• The Pauli exclusion principle states that no two identical fermions can occupy the same quantum state.
• The nucleus is the central part of an atom, containing protons and neutrons.
• The number of electrons in each energy level determines the configuration of an atom.
• The valence electrons of an atom are the electrons in the outermost energy level or shell.
• Protons are positively charged particles found within atomic nuclei.
• The atomic mass is calculated by adding up the number of protons and neutrons in an atom's nucleus.
• Electron configuration refers to how many electrons are found in each energy level or shell surrounding the nucleus.
• Atomic structure consists of three main parts: the nucleus (protons and neutrons), electrons orbiting around the nucleus, and subatomic particles such as quarks and gluons that make up protons and neutrons.
• Electrons orbit around the nucleus at various distances from it.
• Cations are positive ions with fewer electrons than protons.
• Ions are electrically charged atoms formed when one or more electrons are lost or gained.
• Neutral atoms have equal numbers of protons and electrons.
• An element is defined based on its atomic number, which represents the number of protons in its atoms.
• Electron configurations describe how many electrons are present on each shell or subshell within an atom.
• Protons carry positive charges (+1) and are located in the nucleus of an atom.
• Electron shells or orbitals are regions around the nucleus where electrons are found.
• Atoms bohr
• The Bohr model describes the structure of hydrogen atoms as having one electron moving in circular paths around a single proton at the center.
• In the Bohr model, energy levels correspond to different distances between the electron and the proton.
• When an electron absorbs enough energy from light, it can jump up to higher energy levels.
• When an electron absorbs enough energy, it can jump from a lower-energy level to a higher-energy level.
• If an electron jumps back down to a lower-energy level, it releases that same amount of energy.
• Valence electrons