Unit 5 electrons pt 2

2. The distance from the outermost (valence) electrons and the nucleus of an atom. Periodic trend that increases as you move down and decreases as you move across (to the right) the periodic table.
3. a fundamental property of all electrons that causes them to have magnetic fields associated with them
5. a rule stating that when filling orbitals of equal energy, electrons will occupy empty orbitals singly before pairing with other electrons
7. an unstable state for an atom or a molecule in which energy has been absorbed but not reemitted, raising an electron from the ground state into an high energy orbital
10. the tendency to lose electrons in a chemical reaction. Periodic trend that increases as you move down and decreases as you move across (to the right) the periodic table.
12. the electrons that are not in the outermost principal shell of an atom
14. a number that indicates the shell that an electron occupies

1. the state of an atom or molecule in which the electrons occupy the lowest possible energy orbitals available
4. an electron configuration in which electrons are represented as arrows in boxes corresponding to orbitals of a particular atom
6. states that no more than 2 electrons can occupy an orbital and that the 2 electrons must have opposite spins
7. a representation that shows the occupation of orbitals by electrons for a particular element
8. the amount of energy required to remove an electron from the atom in the gaseous state. Periodic trend that decreases as you move down and increases you move across (to the right) the periodic table.
9. the shell indicated by the principal quantum number
11. the electrons in the outermost principal shell of an atom they are involved in chemical bonding
13. in quantum mechanics, specifies the shape of the orbital and is represented by different letters