Electrons

• Electrons demonstrate wave-particle duality, and can be described by de Broglie wavelength and planck's constant.
• Electron configuration refers to the arrangement of electrons within an atom's shells, with s orbitals having lower energy than p orbitals.
• Electron configurations describe the distribution of electrons in the available energy levels around an atom's nucleus.
• Electrons occupy the lowest available energy level first before pairing up or filling higher-energy levels.
• Electrons occupy discrete energy levels around the nucleus.
• The Bohr model is an early model that explains the structure of atoms.
• The maximum number of electrons that can occupy a particular energy level is determined by the formula 2n^2, where n is the principal quantum number.
• The shape of the electron cloud depends on the energy level of the electron and its quantum numbers.
• In the electron cloud model, electrons are not confined to specific locations but rather exist as probability clouds around the nucleus.
• The electron cloud model is used to describe the behavior of electrons within an atom or molecule.
• Hund's rule states that when filling orbitals, electrons will occupy all available orbitals first before pairing up.
• The Pauli exclusion principle states that no two electrons in an atom can have the same set of quantum numbers (n, l, m).
• The electron configuration is determined based on the number of protons in the nucleus (atomic number) and the total number of electrons in the atom.
• Atomic structure includes the atomic number, mass number, and electron configuration.
• The electron configuration of an element is determined based on its atomic number (number of protons) and the maximum number of electrons that can fit into each orbital.
• Atomic structure includes the nucleus containing protons and neutrons, surrounded by electrons arranged in shells/orbitals.
• Shells are filled from the inside out, starting with the innermost shell (1s).
• The electron cloud is not a physical object but rather represents the probability of finding an electron at any given point in space.
• The electron cloud has no definite shape or size, only regions where it is more likely to find an electron.
• The electron cloud model explains why atoms are electrically neutral despite having negatively charged electrons.
• According to the Bohr model, electrons move in circular paths called orbits around the nucleus at specific distances from it.
• Each electron has a fixed amount of energy associated with its orbital path.
• When an electron absorbs energy, it moves into a higher energy state (excited state) and emits light when returning to its original state.
• Each electron has its own unique set of four quantum numbers (principal, angular momentum, magnetic moment, and spin).
• Angular Momentum Quantum Number - describes the shape of the orbital and corresponds to the sublevel.
• The s orbital has a spherical shape with no nodes, while p orbitals have dumbbell shapes with one node along their axis.
• d orbitals are shaped like four lobes arranged at right angles to each other, with two nodes separating them into three pairs.
• f orbitals consist of seven lobes arranged as five lobes inside a sphere and two outside it, with six nodes dividing them into five groups.
• The Pauli exclusion principle states that no two electrons in an atom can have exactly the same set of four quantum numbers (principal quantum number, azimuthal quantum number, magnetic quantum number, spin).
• Hund's rule states that when there are multiple orbitals with equal energies, electrons will fill them one at a time until all orbitals are half full before starting to fill pairs.
• The electron cloud model provides insight into how electrons interact with other particles and contribute to chemical reactions.
• The electron cloud model helps explain why certain elements have different properties based on their atomic structures.
• Ionization energy is the amount of energy required to remove an electron from an isolated gaseous atom or ion.
• Hund's Rule: Orbitals fill up singly before filling up pairs.
• Aufbau Principle states that electrons fill available orbitals starting from lowest energy level first.
• Electron clouds are regions where electrons are most likely to be found around the nucleus.
• Electron clouds are regions where electrons are most likely to be found around the nucleus.
• Aufbau Principle states that electrons fill available orbitals starting from lowest energy level first.
• Hund's rule states that when multiple orbitals of equal energy exist, they will be singly occupied before any pairing occurs.
• Electron configuration is the arrangement of electrons within atomic orbitals according to the rules of the Aufbau Principle and Hund's Rule.