📝 Quiz Pages

• Atomic structure describes the arrangement of protons, neutrons, and electrons within atoms and how this determines their chemical properties.
• Atomic orbitals are three-dimensional regions around the nucleus where electrons are most likely to be found.
• Quantum states describe the energy levels and spatial distributions of electrons in atoms using quantum numbers.
• The Pauli principle states that no two electrons in an atom can have the same set of four quantum numbers.
• Electronic notation is the systematic way of representing the electron configuration of atoms using orbital designations.
• The Bohr model describes the atom as a nucleus with electrons orbiting in fixed energy levels or shells.
• Heisenberg's uncertainty principle states that you cannot simultaneously know both the exact position and momentum of an electron.
• Effective nuclear charge is the net positive charge experienced by an electron after accounting for shielding by other electrons.
• The photoelectric effect demonstrates the particle nature of light, where photons can eject electrons from metal surfaces.
• Alkali metals are highly reactive Group 1 elements with one valence electron that they readily lose to form +1 cations.
• Alkaline earth metals are Group 2 elements with two valence electrons that form +2 cations.
• Halogens are highly reactive Group 17 elements with seven valence electrons that readily gain one electron to form -1 anions.
• Noble gases are Group 18 elements with complete valence shells, making them chemically inert under normal conditions.
• Transition metals are d-block elements that can form multiple oxidation states due to their partially filled d orbitals.
• Ionization energy is the minimum energy required to remove an electron from a gaseous atom or ion.
• Electron affinity is the energy change that occurs when an electron is added to a gaseous atom.
• Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond.
• Atomic size refers to the size of neutral atoms, which generally decreases across periods and increases down groups.
• Ionic size refers to the size of ions, with cations being smaller and anions being larger than their neutral atoms.