Ch.7 - Quantum MechanicsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Sections
Wavelength and Frequency
Speed of Light
The Energy of Light
Electromagnetic Spectrum
Photoelectric Effect
De Broglie Wavelength
Heisenberg Uncertainty Principle
Bohr Model
Emission Spectrum
Bohr Equation
Introduction to Quantum Mechanics
Quantum Numbers: Principal Quantum Number
Quantum Numbers: Angular Momentum Quantum Number
Quantum Numbers: Magnetic Quantum Number
Quantum Numbers: Spin Quantum Number
Quantum Numbers: Number of Electrons
Quantum Numbers: Nodes
Additional Practice
Diffraction vs Refraction
Quantum Numbers: Emission Spectrum
Dimensional Boxes

Test your skills on the following problems. 

Emission vs. Absorption

Example #1: Which of the following transitions (in a hydrogen atom) represent emission of the smallest or shortest wavelength?

a)  n = 4 to n = 2

b)  n = 3 to n= 4

c)  n = 1 to n = 2

d)  n = 7 to n = 5

e)  n = 2 to n = 5

Example #2: Which of the following transitions represent absorption of a photon with the highest frequency?

a)  n = 3 to n = 1

b)  n = 2 to n = 4

c)  n = 1 to n =2

d)  n = 6 to n = 3

e)  n = 1 to n = 3

Quantum Numbers

Example #3: Provide the n, l and ml value for each of the given orbitals.

a) 7s      n =  ?                             b) 5d     n =  ?

              l  =   ?                                         l =  ?

             ml =   ?                                        ml =  ?

 

c) 2p     n =    ?                            d) 4f      n =  ?

             l  =   ?                                          l  =   ?

             ml =     ?                                      ml =  ?

Example #4: Which statement about the four quantum numbers is false?

a)  n = principal quantum number,            n = 1 to infinity

b)  l = azimuthal quantum number,           l = 0,1,2, . . ., (n+1)

c)  mL = magnetic quantum number, mL = (-l), . . .,0,. . ., (+l)

d)  ms = spin quantum number,    ms = + 1/2  or − 1/2

e)  The first three quantum numbers deal with the atomic orbitals except for the ms quantum   number, which deals with the electrons in the atomic orbitals.

Example #5: Each of the following sets of quantum numbers gives information on a specific orbital. Find the error in each.

a. n = 4, l = 0 , ml = 1, ms = – 1/2

b. n = 5, l = 2 , ml = - 1, ms = 1

c. n = 7, l = 7, ml = - 5, ms = – 1/2

d. n = 0, l = 5, ml = - 3, ms = 1/2

Example #6: How many electrons can have the following quantum sets?

a) n = 4, mL = -1 

b) n = 5, mL = 0 , mS = – 1/2

c) n = 9, l = 4, mS = – 1/2

d) n = 2, mS = 1/2

Example #7: For n = 2, what are the possible sublevels?

a) 0

b) 0, 1

c) 0, 1, 2

d) 0, 1,2, 3

Quantum Numbers & Atomic Shape

Example #8: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 2, l = 1, ml = 0

b) n = 3, l = 2, ml = –1

c) n = 4, l = 0, ml = +1

d) n = 1, l = 1, ml = 0

Example #9: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 3, l = 2, ml = 0, ms = – 1/2

b) n = 3, l = 1, ml = – 3, ms = 1

c) n = 4, l = 0, ml = 0, ms = – 1/2

d) n = 4, l = 2, ml = – 3, ms = 1/2

Example #10: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 3, l = 3, ml = 0, ms = 1/2

b) n = 1, l = 3, ml = – 3, ms = 1

c) n = 7, l = 3, ml = – 4, ms = – 1/2

d) n = 6, l = 3, ml = – 3, ms = – 1/2

Paramagnetism vs. Diamagnetism

Example #11: Give the electron configuration for the following element and its ion. For the ion, state if it is paramagnetic or   diamagnetic:

Ag and Ag+

Example #12: Give the electron configuration for the following element and its ion. For the ion, state if it is paramagnetic or   diamagnetic:

 Cl and Cl+

Electron Configurations

Example #13: Which of the following represents an “excited” state?

a) Cl: 1s22s22p63s23p5

b) Be: 1s22s2

c) Na: 1s22s22p63p1

d) N: 1s22s22p3

Example #14: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Br (33rd electron)      n = ,        l = ,        ml = ,        ms =

Example #15: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Ca (19th electron)         n = ,        l = ,          ml = ,             ms =

Example #16: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Cu (27th electron)        n = ,         l = ,        ml = ,            ms =

Example #17: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Mo3+ (38th electron)       n = ,         l = ,       ml = ,         ms =

Example #18: For a multi-electron atom, arrange the electron subshells of the following listing in order of increasing energy:

6s, 4f, 2p, 5d.