1.
Principle that states electrons will fill in an atom in order of increasing orbital energy
2.
Rule that states that electrons will fill in one to an equivalent energy orbital first before pairing up
3.
Hund’s rule states that the first electrons placed into equal energy orbitals must be ______________.
4.
The Pauli Exclusion Principle states that electrons that occupy the same orbital must have opposite _______.
5.
The physical area of space occupied by 2 electrons
6.
The shape of an “s” type orbital
7.
The shape of a “p” type orbital
8.
The number of orbitals in an “s” type sublevel
9.
The number of orbitals in a“p” type sublevel
10.
The number of orbitals in a “d” type sublevel
11.
The number of orbitals in an “f” type sublevel
12.
The maximum number of electrons that can be held in an “s” type sublevel
13.
The maximum number of electrons that can be held in a “p” type sublevel
14.
The maximum number of electrons that can be held in an “d” type sublevel
15.
The maximum number of electrons that can be held in an “f” type sublevel
16.
The term used to describe orbitals that have equivalent energy
17.
The abbreviated way of writing electron configurations begins with this kind of element
18.
The symbol placed around the element used at the beginning of an abbreviated electron configuration.
19.
Has the electron configuration 1s²2s¹
20.
Has the abbreviated configuration [Ne]3s²3p⁵
21.
Groups 1 & 2 make up this sublevel section on the Periodic Table
22.
Groups 13-18 make up this sublevel section on the Periodic Table
23.
The transition metal section of the Periodic Table makes up this sublevel section
24.
This sublevel section appears as two long rows typically found belowthe periodic table
