This set of questions was taken from a tutorial page of the Department of Chemistry and Physics at Slippery Rock University. The original URL is http://www.geocities.com/sruchem/ . Thanks to the people at SRU!
Electronic Structure of Atoms
a. For each pair of types of electromagnetic radiation given, circle the type having the
b. For each pair of types of electromagnetic radiation given, circle the type having the
2. According to the Bohr Theory, the seventh line of the Paschen series in the emission spectrum of hydrogen gas occurs when an electron goes from an orbit having an n value of __________ to an orbit having an n value of __________.
3. a. When n = 5, what are the possible values of l? __________________________
b. When l = 5, what are the possible values for ml? __________________________
c. When n = 2, what are the possible values for ml? __________________________
4. State whether each of the following combinations of quantum numbers is allowed or not according to the rules you learned in the text. If it is not allowed, explain why.
a. n = 3, l =2, and ml = -2 ____________________________________________
b. n = 6, l = 0, and ml = 1 ____________________________________________
c. n = 2, l = 1, and ml = 0 ____________________________________________
d. n = -1, l = 1, and ml = 1 ____________________________________________
5. a. What is the maximum number of p orbitals that are found in a given electron shell of
an atom? __________
b. What is the maximum number of d orbitals that are found in a given electron shell of
an atom? __________
6. According to Heisenberg’s Uncertainity Principle, we cannot simultaneously determine the position and momentum of an object. Why don’t we observe this effect in our everyday life?
7. Calculate (a) the frequency and (b) the energy of a photon of light having a wavelength of 590 nanometers.
8. Calculate the de Broglie wavelength (in nanometers) of a golf ball moving with a speed of 145 km/s, if the mass of the golf ball is 45.7 grams.
9. Calculate the energy and the frequency of the fourth line in the Paschen Series of the emission spectrum of the hydrogen atom in kJ/mole. The electrons that produce this series of lines move from higher energy states to the n = 3 state. (R = 1.0974 x 107 m-1)
10. Which element is the first p block element? ____________________
11. Which element is the first d block element? ____________________
12. Write electron configurations for each of these elements below using both orbital box diagrams and spectroscopic notation. Also indicate for each element whether it is paramagnetic or diamagnetic. You may use rare gas notation in part c to simplify your answer.
a. magnesium (atomic number = 12)
b. phosphorus (atomic number = 15)
c. cobalt (atomic number = 27)
13. Use spectroscopic notation to represent the electron configuration of the following elements. Indicate for each element whether or not it is paramagnetic. Use rare gas notation if you wish.
a. The element zirconium, atomic number = 40, is found in a number of minerals that have been known since biblical times, but the pure element wasn’t isolated until 1914.
b. The radioactive element polonium, atomic number = 84, was the first element discovered by Mme. Curie and was named for Poland, her native country.
c. Iodine, element 53, can cause health problems either by being present or being absent. A small amount of iodine in the dies it necessary to prevent goiter, but iodine vapor is irritating to the eyes and can cause lesions on the skin.
14. Write down a complete set of four quantum numbers for each of the electrons beyond the nearest rare gas for the elements
a. praseodymium (atomic number = 59)
b. scandium (atomic number = 21)
15. What is the maximum number of electrons in an atom that could have each of the following sets of quantum numbers (assuming all possible values for the other quantum numbers)? If the answer is none, explain why this is so.
a. n = 2, l = 2, ml = 0 _________________________________________
b. n = 5, l = 2 _________________________________________
c. n = 6, l = 2, ml = 1, ms = +1/2 _________________________________________
16. The electron configurations of A and B, two unknown elements, are
A = . . . 3s23p5 B = . . . 3s23p2
a. Indicate whether each element is a metal, a metalloid, or a nonmetal
A __________ __________ B ____________________
b. Which of these is expected to have a smaller atomic radius? ___________
c. Predict the formula of a likely compound formed only by these two elements.
17. Name each of the following elements based on the information provided.
a. electronic configuration is
b. the alkali metal with the largest ionization energy ______________
c. the element whose +4 ion has the configuration [Kr]4d3 ______________
d. the first element (that is the one with the lowest atomic number) that has f electrons in
its ground state electronic configuration. ______________
18. Use spectroscopic notation (and the appropriate noble gas symbol) to represent the electronic configuration for each of the following ions:
Copyright © Michael Richmond. This work is licensed under a Creative Commons License.