- Emission Spectrum
- An incomplete spectrum, in the form of a series of colored lines, is unique for each element.
- Bohr Model
- Suggests that electrons exist only in a series of distinct energy levels known as orbitals at increasing distances from the nucleus.
- Principal Energy Levels
- The orbits or energy levels in atomic models; are also known as energy shells.
- Ground State
- The lowest energy level of an electron in the Bohr model.
- Excited State
- Atoms that have absorbed energy and moved some of their electrons to higher energy levels.
- Quantum-Mechanical Model
- The current model of the atom in which protons and neutrons are located in the nucleus with electrons in orbitals around the nucleus. Orbitals represent the regions of the highest probability.
- Photons
- Einstein’s theories suggested that light consisted of massless particles called photons.
- Wave-Particle Duality
- Electrons act as both a particle and a wave.
- Heisenberg Uncertainty Principle
- A fundamental property of all submicroscopic systems is described as the impossibility of simultaneously knowing both the energy (or momentum) and the exact position of a particle.
- Orbitals
- Three-dimensional regions of the most probable position for an electron.
- Principal Quantum Number
- Identifies the principal or main energy level of an electron.
- Energy Sublevels
- Divisions of principal energy levels within an atom that are further divided into orbitals.
- Electron Configuration
- The arrangement of electrons in an atom of an element in its ground state.
- Aufbau Principle
- Electrons must fill the lowest available energy sublevels before any can be placed in higher energy sublevels.
- Orbital Notation
- Horizontal lines representing the orbitals labeled by sublevel. Each electron is written as an up or down arrow on the line.
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