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Electron Configuration Practice: Chemistry Exercises and Questions, Exams of Chemistry

Davao Doctors College (DDC)Chemistry

Configuration Writing Practice. A. Write a ground state electron configuration for each neutral atom. Ground state means that all of the lowest possible energy ...

Typology: Exams

2021/2022

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Electron Configuration Practice Name: __________________________
Chemistry Due Date: _________
How to write an electron configuration:
A. Determine the total number of electrons to be represented.
B. Use the Aufbau principle to fill the orbitals with electrons for elements 1-23. Refer to
electron configuration periodic table for elements after 23
C. The sum of the superscripts should equal the total number of electrons. Example:
12Mg ls2 2s2 2p6 3s2
I. Configuration Writing Practice
A. Write a ground state electron configuration for each neutral atom. Ground state
means that all of the lowest possible energy levels (up to the proper number of
electrons for the element) are filled.
1. Na: ______________________________________________________
2. Pb: ______________________________________________________
3. Sr: ______________________________________________________
4. U: ______________________________________________________
5. N: ______________________________________________________
6. Ag: ______________________________________________________
7. Ti: ______________________________________________________
8. Ce: ______________________________________________________
9. Cl: ______________________________________________________
10. Hg: ______________________________________________________
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Download Electron Configuration Practice: Chemistry Exercises and Questions and more Exams Chemistry in PDF only on Docsity!

Chemistry Due Date: _________ How to write an electron configuration: A. Determine the total number of electrons to be represented. B. Use the Aufbau principle to fill the orbitals with electrons for elements 1-23. Refer to electron configuration periodic table for elements after 23 C. The sum of the superscripts should equal the total number of electrons. Example:

12Mg ls^2 2s^2 2p^6 3s^2

I. Configuration Writing Practice A. Write a ground state electron configuration for each neutral atom. Ground state means that all of the lowest possible energy levels (up to the proper number of electrons for the element) are filled.

  1. Na: ______________________________________________________
  2. Pb: ______________________________________________________
  3. Sr: ______________________________________________________
  4. U: ______________________________________________________
  5. N: ______________________________________________________
  6. Ag: ______________________________________________________
  7. Ti: ______________________________________________________
  8. Ce: ______________________________________________________
  9. Cl: ______________________________________________________
  10. Hg: ______________________________________________________

Chemistry Due Date: _________ B. Write a ground state electron configuration for these ions. Remember that ions have a change in the total number of electrons (positive have lost electrons and negative have gained). Example: N3-is 1s^2 2s^2 2p^6. It has three extra electrons

11. O2-: ______________________________________________________

  1. Fe2+: ______________________________________________________

13. B3+: ______________________________________________________

  1. Ni2+: ______________________________________________________

15. K+: ______________________________________________________

  1. Co^3 +: ______________________________________________________

C. For the following electron configurations determine the possible elements (or ions) they may represent

  1. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^4 : ______________________
  2. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 : ______________________
  3. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^10 : ______________________
  4. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5 : ______________________
  5. [Kr] 5s^2 4d^10 5p^3 : ______________________
  6. [Ar] 4s^1 : ______________________
  7. [Xe] 6s^2 4f^10 : ______________________
  8. (^) [Ne] 3s^2 3p^1 : ______________________

Chemistry Due Date: _________ E. In the space below, write the full (unabbreviated) electron configurations of the following elements:

  1. sodium ________________________________________________

  2. iron ________________________________________________

  3. bromine ________________________________________________

  4. barium ________________________________________________

  5. neptunium ________________________________________________

F. In the space below, write the Noble Gas (abbreviated) electron configurations of the following elements:

  1. cobalt ________________________________________________

  2. silver ________________________________________________

  3. tellurium ________________________________________________

  4. radium ________________________________________________

  5. lawrencium ________________________________________________

G. Determine what elements are denoted by the following electron configurations:

  1. 1s^2 2s^2 2p^6 3s^2 3p^4 ____________________

  2. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^1 ____________________

  3. [Kr] 5s^2 4d^10 5p^3 ____________________

  4. [Xe] 6s^2 4f^14 5d^6 ____________________

  5. [Rn] 7s^2 5f^11 ____________________

Chemistry Due Date: _________ H. Determine which of the following electron configurations are not valid: State which rule has been violated.

  1. 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4d^10 4p^5 ____________________

  2. 1s^2 2s^2 2p^6 3s^3 3d^5 ____________________

  3. [Ra] 7s^2 5f^8 ____________________

  4. [Kr] 5s^2 4d^10 5p^5 ____________________

  5. [Xe] ___________________

I. Write the full electron configuration, short-hand electron configuration, and fill in the orbital diagrams, for the following elements.

  1. Nitrogen _____________________________________________________________

1s 2s 2p 3s

  1. Chlorine______________________________________________________________

1s 2s 2p 3s 3p

  1. Sodium ______________________________________________________________

1s 2s 2p 3s 3p

  1. Neon ________________________________________________________________

1s 2s 2p 3s 3p

Chemistry Due Date: _________