1. an incomplete spectrum, in the form of a series of colored lines, that is unique for each element
- ground state
- photons
- emission spectrum
- valence electrons
2. suggests that electrons exist only in a series of distinct energy levels known as orbitals at increasing distances from the nucleus
- electron configuration
- bohr model
- hund’s rule
- pauli exclusion principle
3. the orbits or energy levels in atomic models; also known as energy shells
- energy sublevels
- electron configuration
- principal quantum number
- principal energy levels
4. the lowest energy level of an electron in the bohr model
- electron configuration
- ground state
- excited state
- pauli exclusion principle
5. atoms that have absorbed energy and moved some of their electrons to higher energy levels
- ground state
- energy sublevels
- excited state
- emission spectrum
6. 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 highest probability
- quantum-mechanical model
- electron configuration
- atomic model
- bohr model
7. einstein’s theories suggested that light consisted of mass-less particles called photons
- electrons
- anions
- photons
- protons
8. electrons act as both a particle and a wave
- wave-particle duality
- wave attenuation capability
- aufbau principle
- emission spectrum
9. a fundamental property of all submicroscopic systems described as the impossibility of simultaneously knowing both the energy, or momentum, and the exact position of a particle
- heisenburg uncertainty principle
- aufbau principle
- principal energy levels
- pauli exclusion principle
10. three-dimensional regions of the most probable position for an electron
- orbitals
- photons
- valence electrons
- electron configuration
11. identifies the principal or main energy level of an electron
- pauli exclusion principle
- principal energy levels
- principal quantum number
- electron configuration
12. divisions of principal energy levels within an atom that are further divided into orbitals
- principal energy levels
- energy sublevels
- valence electrons
- ground state
13. the arrangement of electrons in an atom of an element in its ground state
- orbital notation
- ground state
- valence electrons
- electron configuration
14. electrons must fill the lowest available energy sublevels before any can be placed in higher energy sublevels
- aufbau principle
- electron configuration
- hund’s rule
- pauli exclusion principle
15. horizontal lines representing the orbitals labeled by sublevel. Each electron is written as an up or down arrow on the line
- orbital notation
- electron dot notation
- electron configuration
- noble gas notation
16. the fact that two electrons in the same orbital must have opposite spins
- heisenburg uncertainty principle
- hund’s rule
- aufbau principle
- pauli exclusion principle
17. abbreviated form of electron configuration
- hund’s rule
- noble gas notation
- electron configuration
- orbital notation
18. states that as electrons fill a sublevel, all orbitals receive one electron with the same spin before they begin to pair up
- hund’s rule
- bohr model
- pauli exclusion principle
- aufbau principle
19. electrons on the outermost energy level of an atom
- anions
- cations
- electron configuration
- valence electrons
20. dots that represent valence electrons around the element’s symbol
- orbital notation
- shorthand notation
- electron configuration
- electron dot notation
21. positive ions
- cations
- anions
- valence electrons
- protons
22. negative ions
- cations
- photons
- electrons
- anions\
