Noodle Day Packet
This packet is called the “Noodle Day Packet” because October 6th is National Noodle Day, so
lets take a quiz and eat pasta! (oh sorry, no eating in class). You must complete all the
materials in this packet (they are all review) by Tuesday, October 6th and be prepared for a
quiz. There will be an Edpuzzle to help review the problems if you need extra help (not
mandatory).
We will be reviewing basic atomic structure, orbital diagrams, electron configurations, and
abbreviated electron configurations in this review.
You need to complete the following and be ready for a quiz on Tuesday.
Complete the following:
1. Read through the Atomic Structure Notes and review the concepts.
2. Complete the orbital diagram practice problems and check with the key.
3. Read through the review on electron configurations and complete the practice
problems.
4. Complete the Electron Configurations Homework and check it with the attached key.
5. Read through the Abbreviated Electron Configurations Notes and complete the practice
problems.
6. Complete the Abbreviated Electron Configurations Homework and check it with the
attached key.
A Basic Review of Atomic Structure
There are four basic shapes of orbitals:




s-orbital – spherically shaped, only one type
p-orbitals – dumb-bell shaped, three types
d-orbitals– complex shapes, five types
f-orbitals – very complex shapes, seven types
Anatomy of an atom:
All atoms are made up of Principle Energy Levels (labeled n=1). Each of those levels is made up of Sublevels
 n = 1 has 1 sublevel (s)
 n = 2 has 2 sublevels (s and p)
 n = 3 has 3 sublevels (s, p, and d)
 n = 4 has 4 sublevels (s, p, d, and f)
 etc
Each of the sublevels is made up of orbitals
 n = 1 has 1 orbital
 n = 2 has 4 orbitals
 n = 3 has 9 orbitals
 n = 4 has 16 orbitals
 etc
Each orbital can hold up to two electrons so
 n = 1 can hold 2 electrons
 n = 2 can hold 8 electrons
 n = 3 can hold 18 electrons
 n = 4 can hold 32 electrons
 etc
There are three basic rules to follow when writing electron configurations:
1. The Aufbau Principle – electrons are added one at a time to the lowest energy orbital available until all the
electrons for the atom have been accounted for
2. The Pauli Exclusion Principle – an orbital can hold a maximum of two electrons
3. Hund’s Rule – electrons occupy equal energy orbital so that a maximum number of unpaired electrons (single
electrons in an orbital) results
Rules about energy:
Generally speaking, it requires less energy for an electron to reside on the 1st energy
level than the second and so on.
Also, it requires less energy for an electron to reside in a s-orbital than in a p-orbital and
so on.
HOWEVER!! This is generally true. You must use the following diagram to help you
when placing electrons in the lowest sublevels available.
We will use an orbital diagram to show the above rules in action. We will start with drawing the orbital diagram for Sr:
First we must identify the number of electrons for Sr: 38 electrons
Next, you will start to fill the sublevels by starting at the bottom of the first arrow
(1s) and continue by following the order shown by the arrows. Remember, s
will have just one line, p will have 3 lines, d will have 5 lines, and f will have 7
lines.
___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___
1s 2s 2p
3s 3p
4s 3d
4p
5s
What is the orbital diagram for bromine? (Cover the answer and try it yourself first!)
___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___
1s 2s 2p
3s 3p
4s 3d
4p
Practice Problems:
Draw the orbital diagrams for the following atoms and then check your answers with the key:
Al, F, K, Pd
___ ___ ___ ___ ___ ___ ___ ___ ___
1s 2s 2p
3s 3p
___ ___ ___ ___ ___
1s 2s 2p
 Al (13 electrons)
 F (9 electrons)
___ ___ ___ ___ ___ ___ ___ ___ ___ ___
1s 2s 2p
3s 3p
4s
 K (19 electrons)
KEY
Don’t look at these
answers until you have
tried them yourself!!!
___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ Pd (48e)
1s 2s 2p
3s 3p
4s 3d
4p
5s 4d
Electron Configurations
Electron configurations are very similar to orbital diagrams except you write them
horizontally instead of vertically and you use superscripts to represent numbers of
electrons instead of lines with arrows.
Since there is only one type of s-orbital, the maximum number that can be written as a
superscript for s is 2. Since there are three types of p-orbitals, the maximum number
that can be asa superscript for p is 6. Since there are five types of d-orbitals, the
maximum number that can be written as a superscript for d is 10. And since there are
seven types of f-orbitals, the maximum number that can be written as a superscript for
f is 14.
YOU ARE RESPONSIBLE FOR BEING ABLE TO
REDRAW THIS CHART BY YOURSELF!!!!
Examples of electron configurations:
a) F 1s22s22p5
b) Ga 1s22s22p63s23p64s23d104p1
Complete the following practice problems THEN check your answers below:
1. Be
2. Au
3. C
4. Na
5. Mo
6. Ca+2
7. F-1
Answers: 1)1s22s2 2)1s22s22p63s23p64s23d104p65s24d105p66s24f145d9
7)1s22s22p6
3)1s22s22p2
4)1s22s22p63s1
5)1s22s22p63s23p64s23d104p65s24d4
6)1s22s22p63s23p6
Once you have completed the examples, complete the homework sheet and
check it with the key!
Abbreviated Electron Configurations
1s22s22p63s2
[Ne]3s2
The electron configuration on the left is a full electron configuration. The electron configuration on the right is the
abbreviated electron configuration. Both show the important part of the electron configuration…the valence electrons.
Steps for writing an abbreviated electron configuration:
1. Write the symbol for the closest noble gas in [brackets].
2. Determine the number of electrons left to place by subtracting the number of electrons in the noble gas used
form the total number of electrons in the atom/ion.
3. Write the number of the energy level that the valence electrons are on for the atom/ion next to the noble gas
symbol.
4. Then write an “s” (the s-orbital will always be the next type of orbital).
5. Pick up on the arrow chart at whatever sublevel you are on.
Example Problems:
1.
2.
3.
4.
5.
N
S
Sr
Co
Br-1
[He]2s22p3
[Ne]3s23p4
[Kr]5s2
[Ar]4s23d7
[Ar]4s23d104p6
Practice Problems:
1. Zr
2. K
3. Bi
4. Ge
5. Sb
6. Pt
7. B
Answers: 1) [Kr]5s24d2
2) [Ar]4s1
3) [Xe]6s24f145d106p3 4) [Ar]4s23d104p2 5) [Kr]5s24d105p3
6) [Xe]6s24f145d8
7) [He]2s22p1
Once you have completed the examples, complete the homework sheet and
check it with the key!
Abbr. Electron Configuration HW
Write the electron configurations for each of the following:
# of
electrons
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
Fr
I-1
Rb
P-3
Cu
Na
Si
Xe
Zr+2
Ag
Ti
Se
Al+3
Ba
Ge
Abbreviated Electron Configuration