NAME:
CLASS PERIOD
Study Guide Ch4
Quantum Mechanics/ Neils Bohr
due test day
How many Quantum Numbers for each electron? _________
Name the four Quantum Numbers:
______________________ ________________________
_________________
________________
PRINCIPLE QUANTUM NUMBER p.101
Relates to the average distance of an electron from the nucleus. Main energy level symbolized by “n”. Electrons
of a main energy level occupy the same electron shell. The total number electrons that can exist in a given shell
or main energy level is 2n2. Main energy level is also the period number on periodic chart. Energy increases as
the distance from nucleus increases.
Write the total number of electrons that can exist in each energy level. 2n2
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# of energy level
# of electrons
Divide correct number of electrons per shelf for the following elements.
Ca _______________________
B ________________________
Na _______________________
ANGULAR MOMEMTUM QUANTUM NUMBER p.102
Relates to the shape of the sublevels.
Name of orbitals
______
_______
_______
_______
Shape of orbitals
______
_______
_______
_______
MAGNETIC QUANTUM NUMBER p.103
Describes orientation of the orbital in space around the nucleus.
Identify the letters of orbitals
P
D
SPIN QUANTUM NUMBERS;
Describes the spin of an electron in an orbital. A single orbital can hold a maximum of two electrons.
Write the two ways it may be written:
_______________________
________________________
ELECTRON CONFIGURATION
SECTION 4.3 P 105
Like all systems in nature, electrons in atoms tend to assume arrangements that have the lowest possible energies.
The lowest energy arrangement of the electrons for each element is called the element’s
_____________ __________________ ___________________ _______________. P. 105
The 4 notations used to indicate electron configurations are:
l. Orbital Notation
Example:
2.
Na
B
O
Electron Configuration Notation
Example:
3.
Br
B
N
Al
O
Noble-Gas Notation
Example:
P
Na
Al
O
4. Lewis Dot Notation
Written in which only the valence electrons of an atom are shown
C
Na
F
B