Name: ____________________________ When is this due? __________________ Date: ______ Period: _______ Electron Configuration Practice Worksheet II 1. Write the ground state electron configuration for each neutral atom. Remember ground state means that all of the lowest possible energy levels (up to the proper number of electrons for the element) are filled. a) Na b) Pb c) Sr d) N 2. Write the ground state electron configuration for each neutral atom in Nobel Gas Notation. Remember ground state means that all of the lowest possible energy levels (up to the proper number of electrons for the element) are filled. a) Na b) Pb c) Sr d) N Name: ____________________________ When is this due? __________________ Date: ______ Period: _______ 3. Write the ground state electron configuration for the following ions. Remember ions have a change in total number of electrons (positive ions, cations, have lost an electron and negative ions, anions, have gained an ion). [Example: N-3 is 1s22s23p6 and has 3 extra electrons] a) O-2 b) Fe+2 c) Cl-1 d) K+ 4. Use the Pauli Exclusion Principle and Hund’s Rule to identify how many unpaired electrons are present in the following atomic structures : The Pauli Exclusion Principle states that a maximum of two electrons can occupy a single atomic orbital to form paired electrons, but only if the two electrons have opposite spins. Hund’s Rule states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbital. a) Si b) Cl c) Mn d) Ru Name: ____________________________ When is this due? __________________ Date: ______ Period: _______ 5. When writing the electron configuration of an element, why would we fill the 4s orbital before we fill the 3d orbital? 6. The elements silicon, gallium, arsenic, germanium, aluminum, cadmium, sulfur, and selenium are all used in the manufacture of various semiconductor devises. Write the ground state electron configuration for germanium. 7. Identify which element would have the following electron configuration as a ground state atom? [Ne]3s2 3p3 8. Fill out the information below? s-orbital Draw the general shape of the orbital How many electrons can it hold? What is the lowest energy level in which it can exist? p-orbital d-orbital f-orbital Name: ____________________________ When is this due? __________________ Date: ______ Period: _______ 9. Draw the Electron Configuration for Ru. Energy Level sorbitals p-orbitals d-orbitals f-orbitals n=5 ____ 5s ____ ____ ____ 5p ____ ____ ____ ____ ____ 5d ____ ____ ____ ____ ____ ____ ____ 5f n=4 ____ 4s ____ ____ ____ 4p ____ ____ ____ ____ ____ 4d ____ ____ ____ ____ ____ ____ ____ 4f n=3 ____ 3s ____ ____ ____ 3p ____ ____ ____ ____ ____ 3d n=2 ____ 2s ____ ____ ____ 2p n=1 ____ 1s 10. Fill out the chart below: Element Atomic Number Na 11 S 16 K Number of electrons in each level 1st 2nd 3rd 4th 2 8 1 1st 2nd 3rd 2 8 6 1st 2nd 3rd 4th 5th 1st 2nd 3rd 4th 5th 1st 2nd 3rd 4th 5th 1st 2nd 3rd 4th 5th 1st 2nd 3rd 4th 5th 4th 5th 5th Al Cl Xe Ca Electron Configuration Number of ethat can be lost or gained Number of electrons left after ionization Charge on the ion 1s22s22p63s1 Lose 1 10 +1 1s22s22p63s23p4 Gain 2 18 -2