CHEM 103 Chapter Notes - Chapter M7Q7: Electron Configuration, Atomic Number, Boron

SECTION INTRODUCTION Electrons in atoms are not just spread out evenly in the space around a nucleus, but instead occupy specific energy levels or "regions" around the nucleus. To show where each electron is located, chemists draw "orbital diagrams" ADDITIONAL READING The Quantum Mechanical Model of the Atom (Tro: Introductory Chemistry-Sections 9.5-9.9) EXERCISES 1. In the space below, continue the chart below to draw a blank orbital diagram up to the 7s subshell. (The order of obitals from low to high energy can be determined by drawing a series of diagonal lines through the orbitals as shown. 3p 3d S-type subshells have just one orbital, while p-subshells have 3 orbitals, 4s 4p 4d 4 d-subshells have 5 orbitals, and f-subshells have orbitals. 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f 3s 2p 2s ls Rev. 12/20

Suppose hydrogen atoms absorb energy so that electrons are excited to the n (a) n 7 to n =1 (b) n 7 to n = 6 (c) n = 2 to n =1 Enter the letter (a, b, or c) for each Which transition produces a photon with the smallest energy? the highest frequency? the shortest wavelength? 7 energy level. Electrons then undergo these transitions, among others Suppose you live in a ditferent universe where a ditferent set of quantum numbers is required to describe the atoms of that unverse. These quantum numbers have the following rules: N, principal1, 2, 3, L' orbital -N M, magnetic 10,-1 How many orbitals are there altogether in the first three electron shells orbitals A possible excited state for the H atom has an electron in the Sd orbital. List all possible sets of quantum numbers n, E, and me for this electron. (Select all that apply) On- 5, 2, m -2 How many subshells that have a principal quantum number n- 4 exist in the electronic shell?