Electron Configuration Practice Worksheet Answer Key

Posted on

In this page, we are going to share information about Electron Configuration practice worksheet answer key. If you really want to know that information, you have to read this entire article. Make sure you will not miss any information about Electron Configuration practice.

Electron Configuration Practice Worksheet

Please write the unabbreviated electron configurations from the below elements:

  1. Copper_______________________________________________
  2. Iodine _______________________________________________
  3. Potassium ____________________________________________
  4. Bismuth ______________________________________________
  5. Zirconium _____________________________________________

Please write the abbreviated electron configurations from the below elements:

  1. Iridium ________________________________________________
  2. Chlorine _______________________________________________
  3. Nobelium ______________________________________________
  4. Caesium _______________________________________________
  5. Magnesium _____________________________________________

The below electron configurations belong to which elements:

  1. 1s22s22p63s1 ____________________________________________
  2. 1s22s22p63s23p64s23d104p65s24d6 ___________________________
  3. [Kr] 5s24d10 _____________________________________________
  4. [Xe] 6s24f145d106p2  _______________________________________
  5. [Rn] 7s25f146d4  __________________________________________

Please determine if the following electron configurations are correct or not:

  1. 1s22s22p63s23p64s24d104p65s1 _______________________________
  2. 1s22s22p63s3 _____________________________________________
  3. [Rn] 7s25f96d2 ____________________________________________
  4. [Ar] 5s24d105p5 ___________________________________________
  5. [Xe] 6s24f10  ______________________________________________

Electron Configuration Practice Worksheet Answer Key

  1. The answer key for the first question is 1s22s22p63s23p64s23d9
  2. The answer key for the second question is 1s22s22p63s23p64s23d104p65s24d105p5
  3. The answer key for the third question is 1s22s22p63s23p64s1
  4. The answer key for the fourth question is 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p3
  5. The answer key for the fifth question is 1s22s22p63s23p64s23d104p65s24d2
  6. The answer key for the sixth question is [Xe] 6s24f145d7
  7. The answer key for the seventh question is [Ne] 3s23p5
  8. The answer key for the eighth question is [Rn] 7s25f14
  9. The answer key for the ninth question is [Xe] 6s1
  10. The answer key for the tenth question is [Ne] 3s2
  11. The answer key for the eleventh question is sodium
  12. The answer key for the twelfth question is ruthenium
  13. The answer key for the thirteenth question is cadmium
  14. The answer key for the fourteenth question is lead
  15. The answer key for the fifteenth question is seaborgium
  16. The answer key for the sixteenth is no, it should be 3d10
  17. The answer key for the seventeenth question is no, there can only be 2 electrons in an s-orbital
  18. The answer key for the eighteenth question is no, 5f shell must be filled before the 6d shell
  19. The answer key for the nineteenth question is no, the short-cut should be [Kr], not [Ar]
  20. The answer key for the twentieth question is yes

About Electronic configurations

What is electron configuration in atomic physics and quantum chemistry? You have to know that the electron configuration in atomic physics and quantum chemistry is the distribution of electrons of an atom or molecule in atomic or molecular orbitals. For instance, the electron configuration of the neon atom is 1s2 2s2 2p6, meaning that the 1s, 2s and 2p subshells are occupied by 2, 2 and 6 electrons respectively.

The electronic configurations explain each electron as moving independently in an orbital, in an average field made by all other orbitals. Mathematically, configurations are explained by Slater determinants or configuration state functions.

Based on the laws of quantum mechanics, for systems with just one electron, a level of energy is associated with each electron configuration and in certain situations, electrons are going to be able to move from one configuration to another configuration by emission or absorption from a quantum of energy in the form of a photon.

We suggest you to learn about the electron configuration of different atoms. It is very useful to understand the structure of the periodic table of elements. Also, this is very useful for explaining the chemical bonds which hold atoms together. In the bulk materials, this same idea will be able to assist explaining the peculiar properties of lasers and semiconductors.

How to Write an Electron Configuration?

Need to know that symbols utilized to write the electron configuration start with the shell number followed by the type of orbital and then the superscript shows how lots of electrons are in the orbital.

For example: He1s2

  • He = The thing you are finding the electron configuration for
  • 1 = Level
  • s = orbital
  • 2 = of electrons in the orbital

Please look at the periodic table, you are able to see that Oxygen has eight electrons. Based on the order of fill above, those eight electrons will fill in the following order 1s, 2s and then 2p. So, Oxygen’s electron configuration will be O 1s22s22p4.

Special Cases: The configurations of ions present a special case of electron configuration, also demonstrate the reason for the formation of those ions in the first place. If you want to write the full electron configuration for an anion, then you are only adding additional electrons and the configuration is continued.

In an example, we know that Oxygen always forms 2- ions when it creates an ion. This will add 2 electrons to its normal configuration creating the new configuration: O2- 1s22s22p6. With 10 electrons you have to note that oxygen’s electron configuration is exactly the same as Neon’s now. In fact, ions form due to they are able to become more stable with gaining or lossing of electrons to become like the noble gases. At this time, you are able to see how they become the same.

Also, the electron configurations for Cations are created based on the number of electrons. However, there is a slight difference in the way they are configured. Firstly, you are able to write their normal electron configuration. Then, when you remove electrons, you have to take them from the outermost shell. Keep in mind that it is not always the same way they were added. For example: Iron has 26 electrons, so its normal electron configuration will be: Fe 1s22s22p63s23p64s23d6. When you make a 3+ ion for Iron, you need to take the electrons from the outermost shell first so that will be the 4s shell not the 3d shell.

When writing several of the lower table configurations, the total configuration is able to be fairly long. In those cases, you are able to use the previous noble gas to abbreviate the configuration. You only need to finish the configuration from where the noble gas leaves it.

Leave a Reply

Your email address will not be published. Required fields are marked *