Objectives: a) Define Aufbau principle, Pauli Exclusion Principle, and Hund's Rule. b) List and describe the four quantum numbers. c) Count valence electrons d) Write electron configurations 1-2) The Atomic Hotel I. The Atomic Hotel is a special hotel designed for electrons. The hotel has a strict policy called the Aufbau principle that states "ground" floors must be filled first and in order. It costs more to get rooms on higher floors. In the atomic world energy is money so "excited" electrons get rooms on higher floors, thus the exception to hotel policy. Looking back through the old guest logs the following layouts can be sketched. Determine which electrons had more "money". Label those electrons as excited. 1 1 1L 1L 1L May 23, 1998 June 19, 1999 September 10, 1991 A B

Objectives: a) Define Aufbau principle, Pauli Exclusion Principle, and Hund's Rule. b) List and describe the four quantum numbers. c) Count valence electrons d) Write electron configurations 1-2) The Atomic Hotel I. The Atomic Hotel is a special hotel designed for electrons. The hotel has a strict policy called the Aufbau principle that states "ground" floors must be filled first and in order. It costs more to get rooms on higher floors. In the atomic world energy is money so "excited" electrons get rooms on higher floors, thus the exception to hotel policy. Looking back through the old guest logs the following layouts can be sketched. Determine which electrons had more "money". Label those electrons as excited. 1 1 1L 1L 1L May 23, 1998 June 19, 1999 September 10, 1991 A B

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 30QAP: Consider the following representation of a set of p orbitals for an atom: mg...

See similar textbooks

Similar questions

Consider the following representation of a set of p orbitals for an atom: mg src=Images/HTML_99425-11-30QAP_image001.jpg alt="" align="top"/> ich of the following statements is(are) true? The areas represented by the p orbitals are positively charged clouds with negatively charged electrons embedded within these clouds. The nucleus is located at the center point of each axis. The electrons move along the elliptical paths as indicated by the p orbitals above. The atom could not be hydrogen because its electron is found in the 1s orbital.
Identify each of the following orbitals and determine the n and l quantum numbers. Explain your answers. a. b.
How many electrons could be held in the second shell of an atom if the spin quantum number ms could have three values instead of just two? (Hint: Consider the Pauli exclusion principle.)
Objectives: a) Define Aufbau principle, Pauli Exclusion Principle, and Hund's Rule. b) List and describe the four quantum numbers. c) Count valence electrons d) Write electron configurations
Please type all work Question 8 Explain the error in the following electron configuration for Sr2+, and provide the correct electron configuration. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2
1. Bohr's atomic model limitations 2. what did Chadwick do that Bohr didn't and how was Chadwick inspired. 3.conclusion about Bohr atomic structure how it affected the scientific world add diagrams when needed
True or false. (Would help if false questions are explained :)) 1. Hund's rule states that when placing electrons in orbitals, electrons must spin in the same direction to minimize repulsion. 2. The Aufbau principle does not tell us how to place electrons in degenerate orbitals. 3. In the H atom, the 6d orbitals are degenerate with the 6s orbital. 4. The H atom is unique because it does not have any 7p orbitals. 5. The electron configuration for an atom only applies to the ground state of an atom.
Which is the correct electron configuration for Sb 2+ in its ground state? Key Concept: Aufbau principle. Electron configuration for ions is determined the same way as with atoms. Count up the total number of electrons in the atom and start filling orbitals from low energy to higher energy. A 1s22s22p63s23p64s23d64p64d105p4 B 1s22s22p63s23p64s23d104p45s24d105p2 C 1s22s22p63s23p64s23d104p65s24d105p1 D 1s22s22p53s23p64s23d104p64d105p1
Four possible electron configurations for a nitrogen atom areshown below, but only one schematic represents the correctconfiguration for a nitrogen atom in its ground state.Which one is the correct electron configuration? Whichconfigurations violate the Pauli exclusion principle?Which configurations violate Hund’s rule?
Play a game to memorize the order in which orbitals fill. Have each group member in turn state the name of the next orbital to fill and the maximum number of electrons it can hold (for example, “1s two,” “2s two,” “2p six,” etc.). If a member gets stuck, other group members can help, consulting Figure 8.5 and the accompanying text summary if necessary. However, when a member gets stuck, the next player starts back at “1s two.” Keep going until each group member can list all the orbitals in order up to “6s two.”
The figure below has several different electron configurations for carbon. Fill in the answers to the questions with A, B, C, or D. In questions that have more than one possible answer give the answers in alphabetic order.Hint: The figure below will display properly when printed. See attachment Which electron configuration is the lowest ground state configuration? Which electron configuration is a violation of Hund's rule? and Which electron configuration is a violation of the Pauli exclusion principle? Which electron configuration is a valid excited state? and Which electron configuration is absolutely forbidden?
What is the abbreviated electron configuartion for mercury(II) ion ? A. [Xe] 4f145d10 B. [Xe] 6s24f145d106p2 C. [Xe] 5d10 D. [Xe] 6s25d106p2