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Chemistry

Unit 3 Concept 2: Electron Configurations

QuestionAnswer
Differentiate between Bohr's model of the atom and the quantum model of the atom. The bohr model said that electrons travel on distinct paths. The quantum model shows that electrons move sporadically throughout the electron cloud.
List and define the four quantum numbers used to describe orbitals s orbital = 2 e- p orbital = 6 e- d orbital = 10 e- f orbital = 14 e-
Summarize the organization of the first three shells of the electron cloud. Include their orbitals and how many total electrons they can hold. 1st Shell = 1s2 2nd Shell = 1s2 1p6 3rd Shell = 1s2 1p6 1d10
Explain the three laws that determine the electron configuration of an atom. Aufbau principle: e- fill the lowest energy orbital first Hund's rule: orbitals of equal energy each get 1 e- before any orbital gets a second Pauli Exclusion principle: no two e- in the same atom can have the same set of quantum numbers
Summarize what starts happening in the fourth period that makes the configuration of electrons more complicated. 4s2 has slightly less energy than 3d10 so 4s2 gets filled first.
Write the electron configuration for the following: a. Berylium b. Chlorine c. Chromium* d. Iodine 1s2 2s2 1s2 2s2 2p6 3s2 3p5 1s2 2s2 2p6 3s2 3p6 4s1 3d5 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5
Write the Noble Gas configuration for the following: a. Bromine b. Copper* c. Nickel [Ar] 4s2 3d10 4p5 [Ar] 4s1 3d10 [Ar] 4s2 3d8
Quantum theory a mathematical description for the waves properties of e- and other tiny particles.
Orbital a 3d region around the nucleus that shos where e- probbly is
Electron configuration The most stable arrangment of e- in an atom's electron cloud.
Created by: Kamryn7
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