Download QUANTUM NUMBERS WORKSHEET Element 1s 2s 2p 3s 3p 3d 4s

QUANTUM NUMBERS WORKSHEET
Element
1s
2s
2p
3s
3p
3d
4s
4p
4d
4f
5s
1.)
K
_
___
_
__ _____
_
___ _____ _______
_
2.)
O
_
_

___
_
___ _____
_
___ _____ _______
_
3.)
Ar
_
_
__
_
___ _____
_
___ _____ _______
_
4.)
Br
_
_
___
_
___ ____
_
___ _____ _______
_
5.)
Rb
_
_
___
_
___ _____
_
___ _____ _______
_
6.)
Co
_
_
___
_
___ _____
_
__ _____ _______
_
7.)
Se
_
_
__
_
___ _____
_
___ _____ _______
_
8.)
B
_
_
___
_
___ ____
_
___ _____ _______
_
9.)
P
_
_
__
_
___ _____
_
___ _____ _______
_
** Each question below corresponds to the number in the table. **
For 1 – 3, give the four quantum numbers for the electron indicated.
1.) n = 3
l=1
m=0
s = +1/2
2.) n = 2
l=0
m=0
3.) n = 2
l=1
m=1
s = +1/2
s = -1/2
For 4 – 9, draw in the electron with the following sets of quantum numbers.
4.) n = 3
l=2 m=0 s=+½
5.) n = 3
l=1
m=+2
6.) n = 4
l=1
8.) n = 3
l=2
m = + 1s = - 1/2
m = - 1 s = - 1/2
s = + 1/2
#5 does not exist - set of quantum #s not possible
7.) n = 2
l=1
m=0
s = + 1/2
9.) n = 2
l=1
m=-1
s = - 1/2
10.) Does an electron with this set of quantum numbers exist in the element calcium?
n=4
l=1 m=0
s=-½
no - describes a 4p electron - Ca does not have any 4p electrons
Determine the element whose outermost electron (last electron added) is being defined by the following
quantum numbers.
11.) n = 2
l =0 m = 0
s = -1/2
Be
(note change to n value)
12.) n = 4
l =1
m=1
13.) n = 3
l =1
m = -1
14.) n = 4
l=0
m=0
15.) n = 3
l=2
m = -2
s = -1/2
s = +1/2
s = +1/2
s = -1/2
Kr
E=h.ν
c=λ.ν
h = 6.626 x 10-34 J.s
c = 3.00 x 108 m/s
Al
K
Fe
Unit 4 Review Worksheet
Section I - Problems
Given:
1. What is the frequency of a wave with a wavelength of 3.5 x 10-4 m? 8.6 x 1011 Hz
2. What is the energy of a photon with a frequency of 5.41 x 1017 Hz? 3.58 x 10-16 J
3. What type of electromagnetic radiation is described in question 2? x-rays/ultraviolet
Section II - Electromagnetic Spectrum
1. Label both ends of the spectrum with high/low frequency, high/low energy, and long/short wavelength
radio waves
long λ
low ν
low E
microwaves
infrared light
ROYGBIV
ultraviolet light x-rays
gamma rays
short λ
high ν
high E
2. Which has a higher energy, gamma or x-rays?
3. Which has a shorter wavelength, radio or ultraviolet?
4. Which has a lower frequency, yellow or green light?
5. In the equation E = h . ν, energy and frequency are ____directly____ proportional.
6. In the equation c = λ . ν, wavelength and frequency are _____inversely_____ proportional.
7. The symbol for wavelength is _λ_.
8. Electrons give off energy in the form of a _quantum/photon_ when returning to the ground state.
9. Which scientist proposed the idea that electrons travel around the nucleus in fixed paths? Bohr
10. When an electron moves from the ground state to the excited state, energy is _absorbed_.
11. Bohr chose the element _hydrogen_ to prove his theory.
12. The dual wave-particle nature of electrons describes how the electrons in atoms can behave as
_waves_ and _particles_.
Section III - Electrons
1. What is an electron cloud? area around the nucleus where electrons are located
2. Who proposed the uncertainty principle? Heisenberg
3. Who is credited with the idea that electrons are placed in the lowest energy level first? Aufbau
4. What rule requires that each of the "p" orbitals (at a particular energy level) receive one electron
before any of the orbitals can have two electrons? Hund’s Rule
5. What is the maximum number of electrons in any orbital? 2
6. The principal quantum number, n, indicates the _energy level_.
7. The maximum number of electrons in an energy level can be determined by the equation _2n2_
That means the maximum number of electrons in the 3rd energy level is ________18_________.
8. The number of sublevels in any energy level can be determined by _# of the energy level_.
9. The number of orbitals in an energy level can be determined by the equation ___n2___.
So, the 3rd energy level has __9__ orbitals. (_1_ is/are "s" orbitals, _3_ is/are "p" orbitals, and _5_
is/are "d" orbitals)
10. List the four sublevels according to increasing energy. s --> p --> d --> f
11. The "s" sublevel is shaped like a __sphere__ and has _1_ orbitals.
12. A "p" sublevel is shaped like a __dumbbell__ and has __3__ orbitals.
13. The "d" sublevel has __5__ orbitals and the "f" sublevel has __7__ orbitals.
Section IV - Electron configuration, noble gas configuration, valence electrons, orbital notations
1. What is the electron configuration for phosphorus? 1s2 2s2 2p6 3s2 3p3
2. How many total electrons are in a neutral atom of phosphorus? 15
3. Write the noble gas configuration for phosphorus. [Ne] 3s2 3p3
4. What is the highest occupied energy level for phosphorus? 3
5. What is the atomic number of phosphorus? 15
6. Draw the orbital notation for phosphorus.
7. Circle the last electron added to phosphorus. What are the four quantum numbers for this electron?
n=3
l=1
m=1
s = +1/2
8. How many electrons are in the highest occupied energy level of phosphorus? 5
9. How many inner-shell electrons does phosphorus have? inner-shell electrons = non-valence electrons
total electrons (15) - valence electrons (5) = 10 inner-shell electrons
10. In which orbitals are the inner-shell electrons located?
11. Draw the electron dot diagram for phosphorus.
Section V - Quantum numbers (Honors level only)
1. How many electrons can be described by the quantum numbers n = 3 and l = 1? 6
2. How many electrons in an atom can have the quantum numbers n = 2 and l = 3? 0
3. How many electrons can have the value n = 3? 18
4. How many electrons in an atom have the quantum numbers n = 4 and l = 2? 10
5. Which of the following sets of quantum numbers does NOT represent a possible set of quantum
numbers?
(There may be more than one correct answer.)
n
l
m
s
1
(A)
4
8
-4
/2
1
(B)
6
5
-5
/2
1
(C)
3
2
2
/2
1
(D)
6
0
1
/2
(A) not possible because l value is too large for when n = 4
(D) not possible because m value must be between -l and +l