Configurations of Electrons

Configurations of Electrons and Quantum #s KEY      A typical electron configuration consists of numbers, letters, and superscripts (example‐1s22s22p5), and describes how electrons are arranged in an atom. The coefficient number (in front) indicates the (energy level, sub‐energy level, number of electrons). (circle one) A letter indicates the (energy level, sub‐energy level, number of electrons). (circle one) A superscript indicates the number of electrons in the orbital. For the element represented by the electron configuration: 1s22s22p5, identify the following: (a.) # Energy Levels where electrons can be found two (b.) # Electrons in 2p 5 (c.) Total Electrons 9 (d.) Element Fluorine Identifying Elements from Electron Configuration Identify the element described by each electron configuration. 1. 1s22s22p63s1 2 2 6 2 6 2 10 6 2 Sodium (Na) Ruthenium (Ru) Nickel (Ni) Barium Arsenic (As) 6 2. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 3. 1s22s22p63s23p64s23d8 4. [Xe] 6s2 5. [Ar]4s23d104p3 Electron Configuration Errors Determine if the following electron configurations are correct (Y/N). If NO, explain what is wrong. 6. 1s22s22p63s23p64s24d104p65s1 N should be 3 7. 1s22s22p63s3 N 3s can only hold 2e‐, not 3e‐ 8. [Rn] 7s25f96d2 N 6d1 comes before 5f which should also hold 10e‐ 9. [Ar] 5s24d105p5 N Krypton is the noble gas to use 20. [Xe] 6s24f10 N 5d1 comes before 4f which should also hold 9e‐ Electron Configurations for Neutral Atoms Write the entire, full electron configuration (do not use the Noble Gas shortcut) for each neutral atom given. Neutral atoms have the same number of protons and electrons. 21. 22. Na Sr 1s22s22p63s1 1s22s22p63s23p64s23d104p65s2 23. 24. Cl Ti 1s22s22p63s23p5 1s22s22p63s23p64s23d2 25. Pd 1s22s22p63s23p64s23d104p65s24d8 Electron Configurations for Neutral Atoms Use the Noble Gas shortcut to write the electron configuration for each neutral atom given. 26. 27. 28. 29. Na Sr Cl Ti [Ne]3s1 [Kr]5s2 [Ne]3s23p5 [Kr]4s23d2 30. Pd [Kr]5s24d8 More Quantum Practice  Quantum #s predict the location of a specific electrons by identifying where we can find the electron 90_ % of the time.  The electrons with the highest amount of energy are the electrons most likely to react in chemistry.  These electron is called the valence electrons, and are the electrons that fill last in Aufbau diagrams and electron configurations. 31. Which electron is highest in energy? (circle one) 1s1 2s1 2p1 3p1 2d1 3d1 32. Arrange the following in order of lowest energy to highest energy. 3s1 3p1 4s1 3d1 4p1 4d1 33. For this element, 1s22s22p63s23p64s23d8 , the electrons that have the highest energy are located in which energy level ? third (write number) 34. For this element, 1s22s22p63s23p64s23d8 , the electrons that fill last are located in which type of sub‐energy level? d (write letter) For this element, 1s22s22p63s23p64s23d8 , how many valence electrons are there? 10 For this element, 1s22s22p63s23p64s23d8 , determine Principle (n) and Angular Quantum (l) #s of the electron with the highest amount of energy. 35. 35. 36. n = _3__ Complete the table for each element l = ___2__ Element # valence e‐ Sodium 1 3 s Strontium 2 5 s Chlorine 7 3 p Titanium 4 3 d Palladium 10 4 d Principle Quantum # Angular Quantum # for the electron with for the electron with the highest energy the highest energy