Quantum Model Practice Problems

 

1.    Carbon (C)

a.     Draw an energy level diagram for this element. (orbital box notation)

b.     Write the electronic configuration for this element.(spectroscopic notation, no noble gas abbreviation)

 

 

 

 

 

c.      Relate the electronic structure of the element to the position the element has on the periodic table.

 

 

d.     Draw a quantum model of this element atom. (Use a different color for each energy level.)

 

 

 

2.    Chlorine (Cl)

a.     Draw an energy level diagram for this element. (orbital box notation)

b.     Write the electronic configuration for this element.(spectroscopic notation, no noble gas abbreviation)

 

 

 

 

 

c.      Relate the electronic structure of the element to the position the element has on the periodic table.

 

 

d.     Draw a quantum model of this element atom. (Use a different color for each energy level.)

 

 

 

3.    Magnesium (Mg)

a.     Write the electronic configuration for this element.(spectroscopic notation,  no noble gas abbreviation)

 

 

 

 

 

b.     Relate the electronic structure of the element to the position the element has on the periodic table.

 

 

c.       

                                               i.     Excite this atom: Write the electronic configuration, no noble gas abbreviation, so one of the electrons in the 1s orbital is moved to the excited state by absorbing a photon of 4.00 x 10-19 Joules.

 

 

 

 

                                              ii.     Now describe at least two different ways the atom can return to the ground state. Write the electronic configurations of the atom as it returns to ground state for each of your methods and discuss the number of photons and the energy of the photons released in each method.

METHOD #1 (SINGLE PHOTON)

 

 

 

 

METHOD #2 (MULTIPLE PHOTONS)

4.    Potassium (K)

a.     Draw an energy level diagram for this element. (orbital box notation)

b.     Write the electronic configuration for this element.(spectroscopic notation, no noble gas abbreviation)

 

 

 

 

 

c.      Relate the electronic structure of the element to the position the element has on the periodic table.

 

 

d.     Draw a quantum model of this element atom. (Use a different color for each energy level.)

 

 

 

5.    Vanadium (V)

a.     Draw an energy level diagram for this element. (orbital box notation)

b.     Write the condensed electronic configuration for this element.(spectroscopic notation, noble gas abbreviation)

 

 

 

 

 

c.      Relate the electronic structure of the element to the position the element has on the periodic table.

 

 

d.     Draw a quantum model of this element atom. (Use a different color for each energy level.)

 

 

 

6.     Thallium (Tl)

a.     Electronic configuration without a noble gas abbreviation, spectroscopic Notation.

 

 

 

 

 

b.     Electronic configuration a noble gas abbreviation, spectroscopic Notation.

 

 

 

c.      Relate the electronic configuration to the position of the element in the periodic table.

 

 

 

 

7.     Explain how each of the 3 rules is used to fill the energy diagram. 

 

 

 

 

 

 

8.     Give an example of degenerate orbitals and explain how they relate to HundŐs rule.  (Use carbon as an example.)

 

 

 

9.     Explain the importance of probability in the quantum model of the atom. 

 

 

10. Fluoride (F1-)

a.     Draw an energy diagram for a fluoride ion (Fluorine atom who has taken on an extra electron). 

 

b.     Write the electron configuration for this ion. 

 

 

c.      Draw a quantum model for this ion.